When clothes have stains, bleach is often added to the

Problem 4SC How many moles of aspirin, C9H8O4, contain 0.480 mole of O?

Problem 5QP Balance each of the following equations: a. Mg(s) + AgNO3(aq) ? Mg(NO3)2(aq) + Ag(s) b. CuCO3(s) ? CuO(s) + CO2(g) c. d. Pb(NO3)2(aq) + NaCl(aq) ? PbCl2(s) + NaNO3(aq) e. Al(s) + HCl(aq) ? AlCl3(aq) + H2(g)

Problem 5SC Calculate the molar mass of salicylic acid, C7H6O3.

Problem 6QP Balance each of the following equations: a. Zn(s) + H2SO4(aq) ? ZnSO4(aq) + H2(g) b. N2(g) + I2(g) ? NI3(g) c. K2SO4(aq) + BaCl2(aq) ? BaSO4(s) + KCl(aq) d. e. Al2(SO4)3(aq) + KOH(aq) ? Al(OH)3(s) + K2SO4(aq)

Problem 6SC Silver metal is used in the manufacture of tableware, mirrors, jewelry, and dental alloys. If the design for a piece of jewelry requires 0.750 mole of silver, how many grams of silver are needed? Silver metal is used to make jewelry

Problem 7CI Some of the isotopes of silicon are listed in the following table: (3.4, 3.5, 3.7, 4.2, 4.4, 5.8) Isotope % Natural Abundance Atomic Mass (amu) Half-Life Radiation Emitted 26.99 4.2 s Positron 92.23 27.98 Stable None 4.67 28.98 Stable None 3.10 29.97 Stable None 30.98 2.6 h Beta a. In the following table, indicate the number of protons, neutrons, and electrons for each isotope listed: Isotope Number of Protons Number of Neutrons Number of Electrons ________________ b. What is the electron configuration of silicon? c. Calculate the atomic mass for silicon, using the isotopes that have a natural abundance. d. Write the balanced nuclear equations for the decay of and e. Draw the electron-dot formula and predict the shape of SiCl4. f. How many hours are needed for a sample of with an activity of 16 µCi to decay to 2.0 µCi?

Problem 7QP Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction: a. b. Br2(g) + BaI2(s) ? BaBr2(s) + I2(g) c. d. BaCl2(aq) + K2CO3(aq) ? BaCO3(s) + 2KCl(aq)

Problem 7SC Using the equation in Sample Problem 6.7, calculate the number of moles of oxygen that must react to produce 0.756 mole of water. Sample Problem 6.7 Propane gas (C3H8), a fuel used in camp stoves, soldering torches, and specially equipped automobiles, reacts with oxygen to produce carbon dioxide, water, and energy. How many moles of CO2 can be produced when 2.25 moles of C3H8 react? Propane Solution Step 1 State the given and needed quantities. Analyze the Problem Step 2 Write a plan to convert the given to the needed quantity (moles or grams). Step 3 Use coefficients to write mole?mole factors; write molar mass factors if needed. Step 4 Set up the problem to give the needed quantity (moles or grams). The answer is given with three SFs because the given quantity, 2.25 moles of C3H8, has three SFs. The values in the mole?mole factor are exact.

Problem 8CI K+ is an electrolyte required by the human body and found in many foods as well as salt substitutes. One of the isotopes of potassium is potassium-40, which has a natural abundance of 0.012% and a half-life of 1.30 × 109 y. The isotope potassium-40 decays to calcium-40 or to argon-40. A typical activity for potassium-40 is 7.0 ?Ci per gram. Potassium chloride is used as a salt substitute. a. Write a balanced nuclear equation for each type of decay. b. Identify the particle emitted for each type of decay. c. How many K+ ions are in 3.5 oz of KCl? d. What is the activity of 25 g of KCl in becquerels?

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction: a. H2(g) + Br2(g) \(\longrightarrow\) 2HBr(g) b. AgNO3(aq) + NaCl(aq) \(\longrightarrow\) AgCl(s) + NaNO3(aq) c. 2H2O2(aq) \(\longrightarrow\) 2H2O(g) + O2(g) d. Zn(s) + CuCl2(aq) \(\longrightarrow\) Cu(s) + ZnCl2(aq)

Calculate each of the following: a. number of C atoms in 0.500 mole of C b. number of \(\mathrm{SO}_2\)molecules in 1.28 moles of (\mathrm{SO}_2\) c. moles of Fe in \(5.22 \times 10^{22}\) atoms of Fe

Problem 28QP Calculate each of the following: a. number of Co atoms in 2.2 moles of Co b. number of CO2 molecules in 0.0180 mole of CO2 c. moles of Cr in 4.58 × 1023 atoms of Cr

Calculate each of the following in 2.00 mol of \(\mathrm{H}_{3} \mathrm{PO}_{4}\): a. moles of H b. moles of O c. atoms of P d. atoms of O

Problem 30QP Calculate each of the following quantities in 0.185 mole of (C3H7)2O: a. moles of C b. moles of O c. atoms of H d. atoms of C

Problem 31QP Calculate the molar mass for each of the following: a. KC4H5O6 (cream of tartar) b. Fe2O3 (rust) c. C19H20FNO3 (Paxil, an antidepressant) d. Al2(SO4)3 (antiperspirant) e. Mg(OH)2 (antacid) f. C16H19N3O5S (amoxicillin, an antibiotic)

Problem 32QP Calculate the molar mass for each of the following: a. FeSO4 (iron supplement) b. Al2O3 (absorbent and abrasive) c. C7H5NO3S (saccharin) d. C3H8O (rubbing alcohol) e. (NH4)2CO3 (baking powder) f. Zn(C2H3O2)2 (dietary supplement)

Problem 33QP Calculate the mass, in grams, for each of the following: a. 2.00 moles of Na b. 2.80 moles of Ca c. 0.125 mole of Sn d. 1.76 moles of Cu

Problem 34QP Calculate the mass, in grams, for each of the following: a. 1.50 moles of K b. 2.5 moles of C c. 0.25 mole of P d. 12.5 moles of He

Problem 35QP Calculate the mass, in grams, for each of the following: a. 0.500 mole of NaCl b. 1.75 moles of Na2O c. 0.225 mole of H2O d. 4.42 moles of CO2

Problem 67QP Nitrogen and hydrogen react to form ammonia. N2(g) + 3H2(g) ? 2NH3(g) Determine the limiting reactant in each of the following mixtures of reactants: a. 3.0 mol of N2 and 5.0 mol of H2 b. 8.0 mol of N2 and 4.0 mol of H2 c. 3.0 mol of N2 and 12.0 mol of H2

Problem 36QP Calculate the mass, in grams, for each of the following: a. 2.0 moles of MgCl2= b. 3.5 moles of C3H8 c. 5.00 moles of C2H6O d. 0.488 mole of C3H6O3

Problem 68QP Iron and oxygen react to form iron(III) oxide. 4Fe(s) + 3O2(g) ? 2Fe2O3(s) Determine the limiting reactant in each of the following mixtures of reactants: a. 2.0 mol of Fe and 6.0 mol of O2 b. 5.0 mol of Fe and 4.0 mol of O2 c. 16.0 mol of Fe and 20.0 mol of O2

Problem 69QP For each of the following reactions, 2.00 moles of each reac-tant is present initially. Determine the limiting reactant, and calculate the moles of product in arentheses that would form. a. 2SO2(g) + O2(g) ? 2SO3(g) (SO3) b. 3Fe(s) + 4H2O(l) ? Fe3O4(s) + 4H2(g) (Fe3O4) c.

Problem 70QP For each of the following reactions, 3.00 moles of each reac-tant is present initially. Determine the limiting reactant, and calculate the moles of product in parentheses that would form. a. 4Li(s) + O2(g) ? 2Li2O(s) (Li2O) b. Fe2O3(s) + 3H2(g) ?2Fe(s) + 3H2O(l) (Fe) c. Al2S3(s) + 6H2O(l) ?2Al(OH)3(aq) + 3H2S(g) (H2S)

Problem 71QP For each of the following reactions, 20.0 g of each reactant is present initially. Determine the limiting reactant, and calculate the grams of product in parentheses that would be produced. a. 2Al(s) + 3Cl2(g) ?2AlCl3(s) (AlCl3) b. 4NH3(g) + 5O2(g) ?4NO(g) + 6H2O(g) (H2O) c. CS2(g) + 3O2(g) ?CO2(g) + 2SO2(g) (SO2)

Problem 72QP For each of the following reactions, 20.0 g of each reactant is present initially. Determine the limiting reactant, and calculate the grams of product in parentheses that would be produced. a. 4Al(s) + 3O2(g) ? 2Al2O3(s) (Al2O3) b. 3NO2(g) +H2O(l) ?2HNO3(aq) +NO(g) (HNO3) c. C2H5OH(l) +3O2(g) ?2CO2(g) +3H2O(g) (H2O)

Problem 73QP a. Why do chemical reactions require activation energy? b. In an exothermic reaction, is the energy of the products higher or lower than that of the reactants? c. Draw an energy diagram for an exothermic reaction.

Problem 74QP a. What is measured by the heat of reaction? b. In an endothermic reaction, is the energy of the products higher or lower than that of the reactants? c. Draw an energy diagram for an endothermic reaction.

Problem 75QP Classify the following as exothermic or endothermic reactions: a. A reaction releases 550 kJ. b. The energy level of the products is higher than that of the reactants. c. The metabolism of glucose in the body provides energy.

Problem 76QP Classify the following as exothermic or endothermic reactions: a. The energy level of the products is lower than that of the reactants. b. In the body, the synthesis of proteins requires energy. c. A reaction absorbs 125 kJ.

Problem 107AQP How many moles are in 25.0 g of each of the following compounds? (6.5) a. CO2 b. Al(OH)3 c. MgCl2

Problem 108AQP How many moles are in 4.00 g of each of the following compounds? (6.5) a. NH3 b. Ca(NO3)2 c. SO3

Problem 109AQP At a winery, glucose (C6H12O6) in grapes undergoes fermentation to produce ethanol (C2H6O) and carbon dioxide. (6.6, 6.7) Glucose in grapes ferments to produce ethanol. a. How many grams of glucose are required to form 124 g of ethanol? b. How many grams of ethanol would be formed from the reaction of 0.240 kg of glucose?

Problem 110AQP Gasohol is a fuel that contains ethanol (C2H6O), which burns in oxygen (O2) to give carbon dioxide and water. (6.6, 6.7) a. Write the balanced equation for the combustion of ethanol. b. How many moles of O2 are needed to completely react with 4.0 moles of C2H6O? c. If a car produces 88 g of CO2, how many grams of O2 are used up in the reaction? d. If you add 125 g of C2H6O to your fuel, how many grams of CO2 and H2O can be produced from the ethanol?

Problem 111AQP When ammonia (NH3) reacts with fluorine, the products are dinitrogen tetrafluoride and hydrogen fluoride. (6.1, 6.6, 6.7) a. Write the balanced equation for the reaction. b. How many moles of each reactant are needed to produce 4.00 moles of HF? c. How many grams of F2 are required to react with 25.5 g of NH3? d. How many grams of N2F4 can be produced when 3.40 g of NH3 reacts?

Problem 112AQP When peroxide (H2O2) is used in rocket fuels, it produces water and oxygen (O2). (6.1, 6.6, 6.7) a. Write the balanced equation for the reaction. b. How many moles of peroxide are needed to produce 3.00 moles of water? c. How many grams of peroxide are required to produce 36.5 g of O2? d. How many grams of water can be produced when 12.2 g of peroxide reacts?

Problem 113AQP Ethane gas, C2H6, reacts with chlorine gas, Cl2, to form hexachloroethane gas, C2Cl6, and hydrogen chloride gas.(6.1, 6.6, 6.7) a. Write the balanced equation for the reaction. b. How many moles of chlorine gas must react to produce 1.60 moles of hexachloroethane? c. How many grams of hydrogen chloride are produced when 50.0 g of ethane reacts? d. How many grams of hexachloroethane are produced when 50.0 g of ethane reacts?

Problem 114AQP Propane gas, C3H8, a fuel for many barbecues, reacts with oxygen to produce water and carbon dioxide. Propane has a density of 2.02 g/L at room temperature. (6.1, 6.4, 6.6, 6.7) Propane is converted to carbon dioxide and water when used as a fuel in a barbecue. a. Write the balanced equation for the reaction. b. How many grams of water form when 5.00 L of propane gas completely react? c. How many grams of CO2 are produced from 18.5 g of oxygen gas and excess propane? d. How many grams of H2O can be produced from the reaction of 8.50 × 1022 molecules of propane gas?

Problem 115AQP Acetylene gas, C2H2, burns in oxygen to produce carbon dioxide and water. If 62.0 g of CO2 is produced when 22.5 g of C2H2 reacts with sufficient oxygen, what is the percent yield of CO2 for the reaction? (6.1, 6.6, 6.7, 6.8)

Problem 116AQP When 50.0 g of iron(III) oxide reacts with carbon monoxide, 32.8 g of iron is produced. What is the percent yield of Fe for the reaction? (6.6, 6.7, 6.8) Fe2O3(s) + 3CO(g) ? 2Fe(s) + 3CO2(g)

Acetone (propanone), a clear liquid solvent with an acrid odor, is used to remove nail polish, paints, and resins. It has a low boiling point and is highly flammable. The combustion of acetone has a \(\Delta H\) of –28.5 kJ/g. Acetone has a density of 0.786 g/mL. (1.10, 5.5, 5.7, 6.1, 6.2, 6.4, 6.5, 6.7, 6.9) a. What is the molecular formula of acetone? b. What is the molar mass of acetone? c. Identify the bonds C — C, C — H, and C — O in a molecule of acetone as polar covalent or nonpolar covalent. d. Write the balanced equation for the combustion of acetone. e. How many grams of oxygen gas are needed to react with 15.0 mL of acetone? f. How much heat, in kilojoules, is given off for the reaction in part e?

Problem 12QP Complete the equation for each of the following types of reactions, and then balance: a. combination: Ca(s) + O2(g) ? ________ b. c. decomposition: PbO2(s) ? ________ + ________ d. single replacement: KI(s) + Cl2(g) ? _________ + ________ e. double replacement: CuCl2(aq) + Na2S(aq) ? ________ + NaCl(aq)

Problem 12CI The active ingredient in Tums is calcium carbonate. One Tums tablet contains 500. mg of calcium carbonate. (1.8, 1.9, 5.2, 5.3, 5.4, 6.4, 6.5, 6.6) The active ingredient in Tums neutralizes excess stomach acid. a. What is the formula for calcium carbonate? b. What is the molar mass of calcium carbonate? c. How many moles of calcium carbonate are in one roll of Tums that contains 12 tablets? d. If a person takes two Tums tablets, how many grams of calcium are obtained? e. If the daily recommended quantity of Ca2+ to maintain bone strength in older women is 1500 mg, how many tablets will supply the needed calcium?

Problem 13QP Identify each of the following as an oxidation or a reduction reaction: a. Na+ (aq) + e? ? Na(s) b. Ni(s) ? Ni2+ (aq) + 2e? c. Cr3+ (aq) + 3 e? ? Cr(s) d. 2H+ (aq) + 2 e? ? H2(g)

Problem 14CI The compound butyric acid gives rancid butter its characteristic odor. (1.10, 5.5, 5.7, 6.1, 6.2, 6.4, 6.5, 6.7, 6.8) Butyric acid produces the characteristic odor of rancid butter. a. If black spheres are carbon atoms, white spheres are hydrogen atoms, and red spheres are oxygen atoms, what is the formula of butyric acid? b. What is the molar mass of butyric acid? c. How many grams of butyric acid contain 3.28 × 1023 atoms of O? d. How many grams of carbon are in 5.28 g of butyric acid? e. Butyric acid has a density of 0.959 g/mL at 20 °C. How many moles of butyric acid are contained in 1.56 mL of butyric acid? f. Write a balanced equation for the combustion of butyric acid with oxygen gas to form carbon dioxide and water. g. How many grams of oxygen are needed to completely react 1.58 g of butyric acid? h. What mass of carbon dioxide is formed when 100. g of butyric acid and 100. g of oxygen react?

Problem 14QP Indicate whether each of the following is an oxidation or a reduction reaction: a. O2(g) + 4 e? ? 2O2?(aq) b. Al(s) ? Al3+(aq) + 3 e? c. Fe3+(aq) + e? ? Fe2+(aq) d. 2Br?(aq) ? Br2(l) + 2 e?

Problem 15CI Tamiflu®(Oseltamivir), C16H28N2O4, is an antiviral drug used to treat influenza. The preparation of Tamiflu begins with the extraction of shikimic acid from the seedpods of the Chinese spice, star anise (Illicium verum). From 2.6 g of star anise, 0.13 g of shikimic acid can be obtained and used to produce one capsule containing 75 mg of Tamiflu. The usual adult dosage for treatment of influenza is two capsules of Tamiflu daily for 5 days. (5.5, 5.7, 6.1, 6.2, 6.4, 6.5) Shikimic acid is the basis for the antiviral drug in Tamiflu. The spice called star anise is a plant source of shikimic acid. a. What is the formula of shikimic acid? (Black spheres = C, white spheres = H, and red spheres = O) b. What is the molar mass of shikimic acid? c. How many moles of shikimic acid are contained in 130 g of shikimic acid? d. How many capsules containing 75 mg of Tamiflu could be produced from 155 g of star anise? e. What is the molar mass of Tamiflu? f. How many kilograms of Tamiflu would be needed to treat all the people in a city with a population of 500 000 if each person takes two Tamiflu capsules a day for 5 days?

Problem 15QP In the following reactions, identify which reactant is oxidized and which is reduced: a. Zn(s) + Cl2(g) ? ZnCl2(s) b. Cl2(g) + 2NaBr(aq) ? 2NaCl(aq) + Br2(l) c. 2PbO(s) ? 2Pb(s) + O2(g) d. 2Fe3+(aq) + Sn2+(aq) ? 2Fe2+(aq) + Sn4+(aq)

Problem 16QP In the following reactions, identify which reactant is oxidized and which is reduced: a. 2Li(s) + F2(g) ? 2LiF(s) b. Cl2(g) + 2KI(aq) ? 2KCl(aq) + I2(s) c. Mg(s) + Cu2+(aq) ? Mg2+(aq) + Cu(s) d. Fe(s) + CuSO4(aq) ? FeSO4(aq) + Cu(s)

Problem 16CI When clothes have stains, bleach is often added to the wash to react with the soil and make the stains colorless. One brand of bleach contains 5.25% sodium hypochlorite by mass (active ingredient) with a density of 1.08 g/mL. The liquid bleach solution is prepared by bubbling chlorine gas into a solution of sodium hydroxide to produce sodium hypochlorite, sodium chloride, and water. (1.10, 5.2, 5.4, 6.1, 6.4, 6.5, 6.8) The active component of bleach is sodium hypochlorite. a. What is the chemical formula and molar mass of sodium hypochlorite? b. How many hypochlorite ions are present in 1.00 gallon of bleach solution? c. Write the balanced equation for the preparation of bleach. d. How many grams of NaOH are required to produce the mass of sodium hypochlorite in 1.00 gallon of bleach? e. If 165 g of Cl2 is passed through a solution containing 275 g of NaOH and 162 g of sodium hypochlorite is produced, what is the percent yield of sodium hypochlorite for the reaction?

Problem 47QP The reaction of hydrogen with oxygen produces water. 2H2(g) + O2(g) ? 2H2O(g) a. How many moles of O2 are required to react with 2.0 mol of H2? b. How many moles of H2 are needed to react with 5.0 mol of O2? c. How many moles of H2O form when 2.5 mol of O2 reacts?

Problem 48QP Ammonia is produced by the reaction of nitrogen and hydrogen. N2(g) + 3H2(g) ? 2NH3(g) a. How many moles of H2 are needed to react with 1.0 mol of N2? b. How many moles of N2 reacted if 0.60 mol of NH3 is produced? c. How many moles of NH3 are produced when 1.4 mol of H2 reacts?

Problem 49QP Carbon disulfide and carbon monoxide are produced when carbon is heated with sulfur dioxide. 5C(s) + 2SO2(g) ? CS2(l) + 4CO(g) a. How many moles of C are needed to react with 0.500 mol of SO2? b. How many moles of CO are produced when 1.2 mol of C reacts? c. How many moles of SO2 are required to produce 0.50 mol of CS2? d. How many moles of CS2 are produced when 2.5 mol of C reacts?

Problem 52QP Nitrogen gas reacts with hydrogen gas to produce ammonia by the following equation: N2(g) + 3H2(g) ? 2NH3(g) a. If you have 3.64 g of H2, how many grams of NH3 can be produced? b. How many grams of H2 are needed to react with 2.80 g of N2? c. How many grams of NH3 can be produced from 12.0 g of H2?

Problem 50QP In the acetylene torch, acetylene gas (C2H2) burns in oxygen to produce carbon dioxide and water. 2C2H2(g) + 5O2(g) ? 4CO2(g) + 2H2O(g) a. How many moles of O2 are needed to react with 2.00 mol of C2H2? b. How many moles of CO2 are produced when 3.5 mol of C2H2 reacts? c. How many moles of C2H2 are required to produce 0.50 mol of H2O? d. How many moles of CO2 are produced from 0.100 mol of O2?

Problem 53QP Ammonia and oxygen react to form nitrogen and water. 4NH3(g) + 3O2(g) ? 2N2(g) + 6H2O(g) a. How many grams of O2 are needed to react with 13.6 g of NH3? b. How many grams of N2 can be produced when 6.50 g of O2 reacts? c. How many grams of water are formed from the reaction of 34.0 g of NH3?

Problem 51QP Sodium reacts with oxygen to produce sodium oxide. 4Na(s) + O2(g) ? 2Na2O(s) a. How many grams of Na2O are produced when 57.5 g of Na reacts? b. If you have 18.0 g of Na, how many grams of O2 are required for reaction? c. How many grams of O2 are needed in a reaction that produces 75.0 g of Na2O?

Iron(III) oxide reacts with carbon to give iron and carbon monoxide. \(\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{C}(s) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}(\mathrm{g})\) a. How many grams of C are required to react with 16.5 g of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\)? b. How many grams of CO are produced when 36.0 g of C reacts? c. How many grams of Fe can be produced when 6.00 g of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) reacts?

Problem 55QP Nitrogen dioxide and water react to produce nitric acid, HNO3, and nitrogen oxide. 3NO2(g) + H2O(l) ? 2HNO3(aq) + NO(g) a. How many grams of H2O are required to react with 28.0 g of NO2? b. How many grams of NO are produced from 15.8 g of H2O? c. How many grams of HNO3 are produced from 8.25 g of NO2?

Problem 56QP Calcium cyanamide, CaCN2, reacts with water to form calcium carbonate and ammonia. CaCN2(s) + 3H2O(l)? CaCO3(s) + 2NH3(g) a. How many grams of H2O are needed to react with 75.0 g of CaCN2? b. How many grams of NH3 are produced from 5.24 g of CaCN2? c. How many grams of CaCO3 form if 155 g of H2O reacts?

Problem 87UTC If green spheres represent chlorine atoms and red spheres represent oxygen atoms, (6.1, 6.2) a. write the formula for each of the reactants and products. b. write the balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

Problem 89UTC Using the models of the molecules, (black = C, white = H, yellow = S, green = Cl), determine each of the following: (6.4, 6.5) 1 2 a. molecular formula b. molar mass c. number of moles in 10.0 g

If blue spheres represent nitrogen atoms and purple spheres represent iodine atoms, (6.1, 6.2) a. write the formula for each of the reactants and products. b. write the balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

Problem 90UTC Using the models of the molecules, (black = C, white = H, yellow = S, red = O), determine each of the following: (6.4, 6.5) 1 2 a. molecular formula b. molar mass c. number of moles in 10.0 g

Problem 91UTC A dandruff shampoo contains dipyrithione, C10H8N2O2S2, an antibacterial and antifungal agent. (6.5) This dandruff shampoo contains dipyrithione. a. What is the molar mass of dipyrithione? b. How many moles of dipyrithione are in 25.0 g? c. How many moles of carbon are in 25.0 g of dipyrithione?

Problem 92UTC Ammonium sulfate, (NH4)2SO4, is used in fertilizers to provide nitrogen for the soil. (6.4, 6.5) a. How many formula units are in 0.200 mole of ammonium sulfate? b. How many H atoms are in 0.100 mole of ammonium sulfate? c. How many moles of ammonium sulfate contain 7.4 × 1025 atoms of N? d. What is the molar mass of ammonium sulfate?

Problem 93UTC Propane gas, C3H8, a hydrocarbon, is used as a fuel for many barbecues. (6.4, 6.5) a. How many grams of the compound are in 1.50 moles of propane? b. How many moles of the compound are in 34.0 g of propane? c. How many grams of carbon are in 34.0 g of propane? d. How many atoms of H are in 0.254 g of propane?

Problem 94UTC Allyl sulfide, (C3H5)2S, is the substance that gives garlic its characteristic odor. (6.4, 6.5) The characteristic odor of garlic is due to a sulfur-containing compound. a. How many moles of sulfur are in 23.2 g of (C3H5)2S? b. How many atoms of H are in 0.75 mole of (C3H5)2S? c. How many grams of carbon are in 4.20 × 1023 molecules of (C3H5)2s? d. How many atoms of C are in 15.0 g of (C3H5)2S?

Problem 95AQP Balance each of the following equations and identify the type of reaction: (6.1, 6.2) a. NH3(g) + HCl(g) ? NH4Cl(s) b. Fe3O4(s) + H2(g) ?Fe(s) + HO(g) c. Sb(s) + Cl2(g) ?AbCl3(s) d. e. KBr(aq) + Cl2(aq) ?KCl(aq) + Br2(l) f. Al2(SO4)3(aq) + NaOH(aq) ? Na2SO4(aq) + Al(OH)3(s)

Problem 96AQP Balance each of the following equations and identify the type of reaction: (6.1, 6.2) a. Li3N(s) ? Li(s) + N2(g) b. Mg(s) + N2(g) ? Mg3N2(s) c. Mg(s) + H3PO4(aq) ? Mg3(PO4)2(s) + H2(g) d. e. Al(s) + Cl2(g) ?AlCl3(s) f. MgCl2(aq) + AgNO3(aq) ? Mg(NO3)2(aq) + AgCl(s)

Problem 128CQ Consider the equation for the reaction of sodium and nitrogen to form sodium nitride. (6.1, 6.2, 6.6, 6.7, 6.8) Na(s) + N2(g) ? Na3N(s) a. Balance the equation. b. If 80.0 g of sodium is reacted with 20.0 g of nitrogen gas, what mass of sodium nitride forms? c. If the reaction in part b has a percent yield of 75.0%, how many grams of sodium nitride are actually produced?

Problem 127CQ Consider the following equation: (6.1, 6.2, 6.6, 6.7, 6.8) Al(s) + O2(g) ? Al2O3(s) a. Balance the equation. b. Identify the type of reaction. c. How many moles of oxygen are needed to react with 4.50 moles of Al? d. How many grams of aluminum oxide are produced when 50.2 g of aluminum reacts? e. When 13.5 g of aluminum is reacted with 8.00 g of oxygen, how many grams of aluminum oxide can form? f. If 45.0 g of aluminum and 62.0 g of oxygen undergo a reaction that has a 70.0% yield, what mass of aluminum oxide forms?

Problem 8SC Using the equation in Sample Problem 6.8, calculate the grams of CO2 that can be produced when 25.0 g of O2 reacts. Sample Problem 6.8 When acetylene, C2H2, burns in oxygen, high temperatures are produced that are used for welding metals. How many grams of CO2 are produced when 54.6 g of C2H2 is burned? Solution Step 1 State the given and needed quantities. Analyze the Problem Step 2 Write a plan to convert the given to the needed quantity (mole or grams). grams of C2H2 Step 3 Use coefficients to write mole?mole factors; write molar mass factors if needed.

Problem 9QP Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction: a. Mg(s) + 2AgNO3(aq) ? Mg(NO3)2(aq) + 2Ag(s) b. 4Fe(s) + 302(g) ? 2Fe2O3(s) c. d. e. Al2(SO4)3(aq) + 6KOH(aq) ? 2Al(OH)3(s) + 3K2SO4(aq) f. KOH(aq) + HBr(aq) ? KBr(aq) + H2O(l)

Problem 9SC For the reaction in Sample Problem 6.9, what is the percent yield if 8.00 g of CO2 produces 10.5 g of LiHCO3? Sample Problem 6.9 On a space shuttle, LiOH is used to absorb exhaled CO2 from breathing air to form LiHCO3. LiOH(s) + CO2(g) ? LiHCO3(s) What is the percent yield of the reaction if 50.0 g of LiOH gives 72.8 g of LiHCO3?

Of much concern to environmentalists is the radioactive noble gas radon-222, which can seep from the ground into basements of homes and buildings. Radon-222 is a product of the decay of radium-226 that occurs naturally in rocks and soil in much of the United States. Radon-222, which has a half-life of 3.8 days, decays by emitting an alpha particle. Radon-222, which is a gas, can be inhaled into the lungs where it is strongly associated with lung cancer. Environmental agencies have set the maximum level of radon-222 in a home at 4 picocuries per liter (pCi/L) of air. (4.2, 4.3, 4.4) A home detection kit is used to measure the level of radon-222. a. Write the balanced nuclear equation for the decay of Ra-226. b. Write the balanced nuclear equation for the decay of Rn-222. c. If a room contains 24 000 atoms of radon-222, how many atoms of radon-222 remain after 15.2 days? d. Suppose a room in a home has a volume of 72 000 L \((7.2 \times 10^4 ~\mathrm L)\). If the radon level is 2.5 pCi/L, how many alpha particles are emitted in one day?

Problem 10CI A sterling silver bracelet, which is 92.5% silver by mass, has a volume of 25.6 cm3 and a density of 10.2 g/cm3. (1.8, 1.9, 1.10, 3.5, 6.4) Sterling silver is 92.5% silver by mass. a. What is the mass, in kilograms, of the bracelet? b. How many atoms of silver are in the bracelet? c. Determine the number of protons and neutrons in each of the two stable isotopes of silver:

Classify each of the following as a combination, decomposition, single replacement, double replacement or combustion reaction: a. CuO(s) + 2HCl(aq) \(\longrightarrow\) CuCl2(aq) + H2O(l) b. 2Al(s) + 3Br2(g) \(\longrightarrow\) 2AlBr3(s) c. Pb(NO3)2(aq) + 2NaCl(aq) \(\longrightarrow\) PbCl2(s) + 2NaNO3(aq) d. C6H12O6(aq) \(\longrightarrow\) 2CO2(aq) + 2CO2(g) e. NaOH(aq) + HCl(aq) \(\longrightarrow\) NaCl(aq) + H2O(l) F. \(\mathrm{C}_{6} \mathrm{H}_{12}(l)+9 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)\)

Problem 10SC Hydrogen sulfide burns with oxygen to give sulfur dioxide and water. How many grams of sulfur dioxide can be produced from the reaction of 8.52 g of H2S and 10.6 g of O2?

Problem 11QP Complete the equation for each of the following types of reactions, and then balance: a. combination: Mg(s) + Cl2(g) ? _______ b. decomposition: HBr(g) ?________ + Br2(g) c. single replacement: Mg(s) + Zn(NO3)2(aq) ? _______ + _______ d. double replacement: K2S(aq) + Pb(NO3)2(aq) ? _______ + _______ e.

Problem 11CI Consider the loss of electrons by atoms of element X in Group 2A (2), Period 3, and a gain of electrons by atoms of element Y in Group 7A (17), Period 3. (3.6, 3.7, 5.1, 5.2, 5.3, 5.7) a. Which reactant has the higher electronegativity? b. What are the ionic charges of X and Y in the product? c. Write the electron configurations of the atoms X and Y. d. Write the electron configurations of the ions of X and Y. e. Write the formula and name for the ionic compound formed by the ions of X and Y.

Problem 11SC Mercury(II) oxide decomposes to mercury and oxygen. a. Is the reaction exothermic or endothermic? b. How many kilojoules are needed to react 25.0 g of mercury(II) oxide?

Problem 37QP a. The compound MgSO4 is called Epsom salts. How many grams will you need to prepare a bath containing 5.00 moles of Epsom salts? b. In a bottle of soda, there is 0.25 mole of CO2. How many grams of CO2 are in the bottle?

Problem 38QP a. Cyclopropane, C3H6, is an anesthetic given by inhalation. How many grams are in 0.25 mole of cyclopropane? b. The sedative Demerol hydrochloride has the formula C15H22ClNO2. How many grams are in 0.025 mole of Demerol hydrochloride?

Problem 39QP How many moles are contained in each of the following? a. 50.0 g of Ag b. 0.200 g of C c. 15.0 g of NH3 d. 75.0 g of SO2

Problem 40QP How many moles are contained in each of the following? a. 25.0 g of Ca b. 5.00 g of S c. 40.0 g of H2O d. 12.2 g of O2

Problem 41QP How many moles of S are in each of the following quantities? a. 25 g of S b. 125 g of SO2 c. 30.1 g of Al2S3

Problem 42QP How many moles of C are in each of the following quantities? a. 75 g of C b. 32.6 g of C2H6 c. 88 g of CO2

Problem 43QP Caffeine, C8H10N4O2, is obtained from tea, coffee, and energy drinks. Coffee beans are a source of caffeine. a. How many grams of caffeine are in 0.850 mole? b. How many moles of caffeine are in 28.0 g of caffeine? c. How many moles of carbon are in 28.0 g of caffeine? d. How many grams of nitrogen are in 28.0 g of caffeine?

Problem 44QP Fructose, C6H12O6, a monosaccharide, is found in honey and fruits. a. How many grams of fructose are in 1.20 moles of fructose? b. How many moles of fructose are in 15.0 g of fructose? c. How many moles of carbon are in 15.0 g of fructose? d. How many grams of oxygen are in 15.0 g of fructose?

Problem 45QP Write all of the mole-mole factors for each of the following equations: a. 2SO2(g) + O2(g) ? 2SO3(g) b. 4P(s) + 5O2(s) ? 2P2O5(s)

Problem 46QP Calculate the total masses of the reactants and the products for each of the following equations: a. 2SO2(g) + O2(g) ? 2SO3(g) b. 4P(s) + 5O2(g) ? 2P2O5(s)

Problem 77QP Classify the following as exothermic or endothermic reactions and give ?H for each: a. b. Ca(OH)2(s) + 65.3 kJ ?CaO(s) + H2O(l) c. 2Al(s) + Fe2O3(s) ?Al2O3(s) + 2Fe(s) + 205 kcal

Problem 78QP Classify the following as exothermic or endothermic reactions and give ?H for each: a. b. 2Na(s) + Cl2(g) ?2NaCl(s) + 819 kJ c. PCl5(g) + 67 kJ ? PCl3(g) + Cl2(g)

Problem 80QP Methanol (CH3OH), which is used as a cooking fuel, undergoes combustion to produce carbon dioxide and water. How many kilojoules are released when 75.0 g of methanol is burned?

Problem 79QP The equation for the formation of silicon tetrachloride from silicon and chlorine is: Si(s) + 2Cl2(g) ? SiCl4(g) ?H = ?657 kJ How many kilojoules are released when 125 g of Cl2 reacts with silicon?

Problem 81UTC Balance each of the following by adding coefficients; identify the type of reaction for each: a. b.

Problem 83UTC If red spheres represent oxygen atoms and blue spheres represent nitrogen atoms, (6.1, 6.2) a. write the formula for each of the reactants and products. b. write the balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

Problem 82UTC Balance each of the following by adding coefficients; identify the type of reaction for each: a. b.

Problem 84UTC If purple spheres represent iodine atoms and white spheres represent hydrogen atoms, (6.1, 6.2) a. write the formula for each of the reactants and products. b. write the balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

Problem 86UTC If green spheres represent chlorine atoms, yellow-green spheres represent fluorine atoms, and white spheres represent hydrogen atoms, (6.1, 6.2) a. write the formula for each of the reactants and products. b. write the balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

Problem 85UTC If blue spheres represent nitrogen atoms and purple spheres represent iodine atoms, (6.1, 6.2) a. write the formula for each of the reactants (solid) and products. b. write the balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

Problem 118CQ When nitrogen dioxide (NO2) from car exhaust combines with water in the air, it forms nitrogen oxide and nitric acid (HNO3), which causes acid rain. 3NO2(g) + H2O(l) ? NO(g)+ 2HNO3(aq) a. How many moles of NO2 are needed to react with 0.250 mol of H2O? b. How many grams of HNO3 are produced when 60.0 g of NO2 completely reacts? c. How many grams of HNO3 can be produced if 225 g of NO2 is mixed with 55.2 g of H2O?

Problem 120CQ If 35.8 g of CH4 and 75.5 g of S react, how many grams of H2S are produced? CH4(g) + 4S(g) ? CS2(g) + 2H2S(g)

Problem 121CQ The formation of nitrogen oxide, NO, from N2(g) and O2(g), requires 21.6 kcal of heat. (6.9) N2(g) + O2(g) ? 2NO(g) ?H = + 21.6 kcal a. How many kilocalories are required to form 3.00 g of NO? b. What is the complete equation (including heat) for the decomposition of NO? c. How many kilocalories are released when 5.00 g of NO decomposes to N2 and O2

Problem 122CQ The formation of rust (Fe2O3) from solid iron and oxygen gas releases 1.7 × 103 kJ. (6.9) 4Fe(s) + 3O2(g) ? 2Fe2O3(s) ?H = 1.7 × 103 kJ a. How many kilojoules are released when 2.00 g of Fe reacts? b. How many grams of rust form when 150 kcal are released? c. What is the complete equation (including heat) for the formation of rust?

Problem 123CQ Write a balanced equation for each of the following reaction descriptions and identify each type of reaction: (6.1, 6.2) a. An aqueous solution of lead(II) nitrate is mixed with aqueous sodium phosphate to produce solid lead(II) phosphate and aqueous sodium nitrate. b. Gallium metal heated in oxygen gas forms solid gallium(III) oxide. c. When solid sodium nitrate is heated, solid sodium nitrite and oxygen gas are produced. d. Solid bismuth(III) oxide and solid carbon react to form bismuth metal and carbon monoxide gas.

Problem 124CQ A toothpaste contains 0.24% by mass sodium fluoride (NaF) used to prevent dental caries and 0.30% by mass triclosan, C12H7Cl3O2, a preservative and antigingivitis agent. One tube contains 119 g of toothpaste. (6.4, 6.5) Components in toothpaste include triclosan and NaF. a. How many moles of NaF are in the tube of toothpaste? b. How many fluoride ions (F?) are in the tube of toothpaste? c. How many grams of sodium ion (Na+) are in 1.50 g of toothpaste? d. How many molecules of triclosan are in the tube of toothpaste?

Problem 125CQ A gold bar is 2.31 cm long, 1.48 cm wide, and 0.0758 cm thick. (6.4, 6.5) a. If gold has a density of 19.3 g/mL, what is the mass, in grams, of the gold bar? b. How many atoms of gold are in the bar? c. When the same mass of gold combines with oxygen, the oxide product has a mass of 5.61 g. How many moles of O are combined with the gold?

Problem 126CQ The gaseous hydrocarbon acetylene, C2H2, used in welders’ torches, releases a large amount of heat when it burns according to the following equation: (6.6, 6.7, 6.8) a. How many moles of water are produced from the complete reaction of 2.50 moles of oxygen? b. How many grams of oxygen are needed to react completely with 2.25 g of acetylene? c. How many grams of carbon dioxide are produced from the complete reaction of 78.0 g of acetylene? d. If the reaction in part c produces 186 g of CO2, what is the percent yield of CO2 for the reaction?

Balance the following equation: \(\mathrm{Al}(s)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{AlCl}_{3}(s)\)

Problem 1QP Determine whether each of the following equations is balanced or not balanced: a. S(s) + O2(g) ? SO3(g) b. 2Al(s) + 3Cl2(g) ? 2AlCl3(s) c. 2NaOH(s) + H2SO4(aq) ? Na2SO4(aq) + H2O(l) d.

Problem 2QP Determine whether each of the following equations is balanced or not balanced: a. PCl3(l) + Cl2(g) ? PCls(s) b. CO(g) + 2H2(g) ? CH3OH(l) c. 2KClO3(s) ?2KCl(s) + O2(g) d. Mg(s) + N2(g) ? Mg3N2(s)

Problem 2SC Balance the following equation: Sb2S3(s) + HCl(aq) ? SbCl3(s) + H2S(g)

Problem 3SC How many moles of water, H2O, contain 2.60 × 1023 molecules of water?

Balance each of the following equations: a. \(\mathrm{N}_2(g)+\mathrm{O}_2(g) \longrightarrow \mathrm{NO}(g)\) b. \(\mathrm{HgO}(s) \longrightarrow \mathrm{Hg}(l)+\mathrm{O}_2(g)\) c. \(\mathrm{Fe}(s)+\mathrm{O}_2(\mathrm{~g}) \longrightarrow \mathrm{Fe}_2 \mathrm{O}_3(s)\) d. \(\mathrm{Na}(s)+\mathrm{Cl}_2(g) \longrightarrow \mathrm{NaCl}(s)\) e. \(\mathrm{Cu}_2 \mathrm{O}(s)+\mathrm{O}_2(g) \longrightarrow \mathrm{CuO}(s)\)

Problem 4QP Balance each of the following equations: a. Ca(s) + Br2(l) ? CaBr2(s) b. P4(s) + O2(g) ? P4O10(s) c. d. Sb2S3(s) + HCl(aq) ? SbCl3(s) + H2S(g) e. Fe2O3(s) + C(s) ? Fe(s) + CO(g)

Problem 18QP Chlorine (Cl2) is used as a germicide to kill microbes in swimming pools. If the product is Cl?, was the elemental chlorine oxidized or reduced?

Problem 17QP In the mitochondria of human cells, energy is provided by the oxidation and reduction of the iron ions in the cytochromes. Identify each of the following reactions as an oxidation or reduction: a. Fe3+ +e??Fe2+ b. Fe2+? Fe3+ + e?

Problem 19QP When linoleic acid, an unsaturated fatty acid, reacts with hydrogen, it forms a saturated fatty acid. Is linoleic acid oxidized or reduced in the hydrogenation reaction?

In one of the reactions in the citric acid cycle, which provides energy for ATP synthesis, succinic acid is converted to fumaric acid. \(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{4} \longrightarrow \mathrm{C}_{4} \mathrm{H}_{4} \mathrm{O}_{4}+2 \mathrm{H}\) Succinic Acid Fumaric Acid The reaction is accompanied by a coenzyme, flavin adenine dinucleotide \(\mathrm{FAD}+2 \mathrm{H} \longrightarrow \mathrm{FADH}_{2}\) a. Is succinic acid oxidized or reduced? b. Is FAD oxidized or reduced? c. Why would the two reactions occur together?

Problem 21QP Calculate each of the following: a. number of Ag atoms in 0.200 mole of Ag b. number of C3H8O molecules in 0.750 mole of C3H8O c. number of Cr atoms in 1.25 moles of Cr

Problem 22QP Calculate each of the following: a. number of Ni atoms in 3.4 moles of Ni b. number of Mg(OH)2 formula units in 1.20 moles of Mg(OH)2 c. number of Li atoms in 4.5 moles of Li

Problem 23QP Calculate each of the following: a. moles of Al in 3.26 × 1024 atoms of Al b. moles of C2H5OH in 8.50 × 1024 molecules of C2H5OH c. moles of Au in 2.88 × 1023 atoms of Au

Problem 24QP Calculate each of the following: a. moles of Cu in 7.8 × 1021 atoms of Cu b. moles of C2H6 in 3.75 × 1023 molecules of C2H6 c. moles of Zn in 5.6 × 1024 atoms of Zn

Problem 25QP Quinine, C20H24N2O2, is a component of tonic water and bitter lemon. a. How many moles of hydrogen are in 1.0 mol of quinine? b. How many moles of carbon are in 5.0 mol of quinine? c. How many moles of nitrogen are in 0.020 mol of quinine?

Problem 26QP Aluminum sulfate, Al2(SO4)3, is used in some antiperspirants. a. How many moles of sulfur are present in 3.0 mol of Al2(SO4)3? b. How many moles of aluminum ions are present in 0.40 mol of Al2(SO4)3? c. How many moles of sulfate ions (SO42?) are present in 1.5 mol of Al2(SO4)3?

Problem 58QP When the gases dihydrogen sulfide and oxygen (O2) react, they form the gases sulfur dioxide and water. a. Write the balanced equation for the reaction. b. How many grams of oxygen are required to react with 2.50 g of dihydrogen sulfide? c. How many grams of sulfur dioxide can be produced when 38.5 g of oxygen reacts? d. How many grams of oxygen are required to produce 55.8 g of water?

Problem 59QP Carbon disulfide is produced by the reaction of carbon and sulfur dioxide. 5C(s) + 2SO2(g) ? CS2(g) + 4CO(g) a. What is the percent yield of carbon disulfide if the reaction of 40.0 g of carbon produces 36.0 g of carbon disulfide? b. What is the percent yield of carbon disulfide if the reaction of 32.0 g of sulfur dioxide produces 12.0 g of carbon disulfide?

Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide. \(\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}_{2}(g)\) a. What is the percent yield for iron if the reaction of 65.0 g of iron(III) oxide produces 38.0 g of iron? b. What is the percent yield for carbon dioxide if a reaction of 75.0 g of carbon monoxide produces 85.0 g of carbon dioxide?

Problem 62QP Propane (C3H8) burns in oxygen to produce carbon dioxide and water. C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g) Calculate the mass of CO2 that can be produced if the reaction of 45.0 g of propane and sufficient oxygen has a 60.0% yield.

Problem 61QP Aluminum reacts with oxygen to produce aluminum oxide. 4Al(s) + 3O2(g) ? 2Al2O3(s) Calculate the mass of Al2O3 that can be produced if the reaction of 50.0 g of aluminum and sufficient oxygen has a 75.0% yield.

Problem 63QP When 30.0 g of carbon is heated with silicon dioxide, 28.2 g of carbon monoxide is produced. What is the percent yield of carbon monoxide for this reaction? SiO2(s) + 3C(s) ? SiC(s) + 2CO(g)

When 56.6 g of calcium is reacted with nitrogen gas, 32.4 g of calcium nitride is produced. What is the percent yield of calcium nitride for this reaction? \(3 \mathrm{Ca}(s)+\mathrm{N}_{2}(g) \longrightarrow \mathrm{Ca}_{3} \mathrm{~N}_{2}(s)\)

Problem 65QP A taxi company has 10 taxis. a. On a certain day, only eight taxi drivers show up for work. How many taxis can be used to pick up passengers? b. On another day, 10 taxi drivers show up for work but three taxis are in the repair shop. How many taxis can be driven?

Problem 66QP A clock maker has 15 clock faces. Each clock requires one face and two hands. a. If the clock maker has 42 hands, how many clocks can be produced? b. If the clock maker has only eight hands, how many clocks can be produced?

Problem 97AQP Predict the products and write a balanced equation for each of the following: (6.1, 6.2) a. single replacement: Zn(s) + HCl(aq) ?____ + _____ b. c. double replacement: NaOH(aq) + HCl(aq) ?____+ _____ d. combination: Al(s) + F2(g) ? ______

Problem 98AQP Predict the products and write a balanced equation for each of the following: (6.1, 6.2) a. b. combination: Ca(s) + Br2(g) ?______ c. combustion: d. double replacement: NiCl2(aq) + NaOH(aq) ?Ni(OH)2(s) + ______

Problem 100AQP For each of the following reactions, predict which reactant is oxidized and which reactant is reduced: (6.3) a. 2Ag(s) + 2H+(aq) ? 2Ag+(aq) + H2(g) b. Mg(s) + Cu2+(aq) ? Mg2+(aq) + Cu(s) c. 2Al(s) + 3Cu2+(aq) ? 2Al3+(aq) + 3Cu(s) d. Mg2+(aq) + Zn(s) ? Mg(s) + Zn2+(aq) e. Al3+(aq) + 3Na(s) ?Al(s) + 3Na+(aq) f. Ni2+(aq) + Mg(s) ? Mg2+(aq) + Ni(s)

Problem 99AQP For each of the following reactions, predict which reactant is oxidized and which reactant is reduced: (6.3) a. Cu(s) + 2H+(aq) ? Cu2+(aq) + H2(g) b. Ni2+(aq) + Fe(s) ? Fe2+(aq) + Ni(s) c. 2Ag(s) + Cu2+(aq) ? 2Ag+(aq) + Cu(s) d. 3Ni2+(aq) + 2Cr(s) ? 3Ni(s) + 2Cr3+(aq) e. Zn(s) + Cu2++(aq) ? Zn2+(aq) + Cu(s) f. Pb2++(aq) + Zn(s) ? Pb(s) + Zn2+(aq)

Problem 101AQP During heavy exercise and workouts, lactic acid, C3H6O3, accumulates in the muscles, where it can cause pain and soreness. (6.4, 6.5) In the ball-and-stick model of lactic acid, black spheres = C, white spheres = H, and red spheres = O. a. What is the molar mass of lactic acid? b. How many molecules are in 0.500 mole of lactic acid? c. How many atoms of C are in 1.50 moles of lactic acid? d. How many grams of lactic acid contain 4.5 × 1024 atoms of O?

Problem 104AQP Calculate the molar mass of each of the following: (6.5) a. Mg(HCO3)2, magnesium hydrogen carbonate b. Au(OH)3, gold(III) hydroxide, used in gold plating c. C18H34O2, oleic acid from olive oil

Problem 103AQP Calculate the molar mass of each of the following: (6.5) a. ZnSO4, zinc sulfate, zinc supplement b. Ca(IO3)2, calcium iodate, iodine source in table salt c. C5H8NNaO4, monosodium glutamate, flavor enhancer

Problem 102AQP Ibuprofen, the anti-inflammatory ingredient in Advil, has the formula C13H18O2. (6.4, 6.5) Ibuprofen is an anti-inflammatory drug. a. What is the molar mass of ibuprofen? b. How many molecules are in 0.200 mole of ibuprofen? c. How many atoms of H are in 0.100 mole of ibuprofen? d. How many grams of ibuprofen contain 7.4 × 1025 atoms of C?

Problem 105AQP How many grams are in 0.150 mole of each of the following? (6.5) a. K b. Cl2 c. Na2CO3

Problem 106AQP How many grams are in 2.25 moles of each of the following? (6.5) a. N2 b. NaBr c. C6H14

Problem 117CQ Pentane gas, C5H12, reacts with oxygen to produce carbon dioxide and water. (6.6, 6.7, 6.8) a. How many grams of pentane must react to produce 4.0 moles of water? b. How many grams of CO2 are produced from 32.0 g of oxygen and excess pentane? c. How many grams of CO2 are formed if 44.5 g of C5H12 is reacted with 108 g of O2?

Problem 119CQ When 12.8 g of Na and 10.2 g of Cl2 react, what is the mass, in grams, of NaCl that is produced? 2Na(s) + Cl2(g) ? 2NaCl(s)

Problem 57QP When the ore lead(II) sulfide burns in oxygen, the products are solid lead(II) oxide and sulfur dioxide gas. a. Write the balanced equation for the reaction. b. How many grams of oxygen are required to react with 29.9 g of lead(II) sulfide? c. How many grams of sulfur dioxide can be produced when 65.0 g of lead(II) sulfide reacts? d. How many grams of lead(II) sulfide are used to produce 128 g of lead(II) oxide?