The gaseous hydrocarbon acetylene, C2H2, used in welders torches, releases 1300 kJ when

What is a mole?

What is Avogadros number?

Calculate each of the following: a. number of C atoms in 0.500 mole of C b. number of SO2 molecules in 1.28 moles of SO2 c. moles of Fe in 5.22 * 1022 atoms of Fe d. moles of C2H6O in 8.50 * 1024 molecules of C2H6O

Calculate each of the following: a. number of \(\mathrm{Li}\) atoms in 4.5 moles of \(\mathrm{Li}\) b. number of \(\mathrm{CO}_{2}\) molecules in 0.0180 mole of \(\mathrm{CO}_{2}\) c. moles of \(\mathrm{Cu}\) in \(7.8 \times 10^{21}\) atoms of \(\mathrm{Cu}\) d. moles of \(\mathrm{C}_{2} \mathrm{H}_{6}\) in \(3.75 \times 10^{23}\) molecules of \(\mathrm{C}_{2} \mathrm{H}_{6}\)

Calculate each of the following quantities in 2.00 moles of \(\mathrm{H}_{3} \mathrm{PO}_{4}\): a. moles of \(\mathrm{H}\) b. moles of \(\mathrm{0}\) c. atoms of \(P\) d. atoms of \(\mathrm{O}\)

Calculate each of the following quantities in 0.185 mole of \(\mathrm{C}_{6} \mathrm{H}_{14} \mathrm{O}:\) a. moles of \(\mathrm{C}\) b. moles of \(\mathrm{O}\) c. atoms of \(\mathrm{H}\) d. atoms of \(\mathrm{C}\)

Quinine, C20H24N2O2, is a component of tonic water and bitter lemon. a. How many moles of H are in 1.0 mole of quinine? b. How many moles of C are in 5.0 moles of quinine? c. How many moles of N are in 0.020 mole of quinine?

Aluminum sulfate, \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\), is used in some antiperspirants. a. How many moles of S are present in 3.0 moles of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\)? b. How many moles of aluminum ions \(\left(\mathrm{Al}^{3+}\right)\) are present in 0.40 mole of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\)? c. How many moles of sulfate ions \(\left(\mathrm{SO}_{4}{ }^{2-}\right)\) are present in 1.5 moles of \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\)?

Calculate the molar mass for each of the following: a. KC4H5O6 1cream of tartar2 b. Fe2O3 1rust2 c. C19H20FNO3 1Paxil, an antidepressant2 d. Al21SO423 1antiperspirant2 e. Mg1OH22 1antacid2

Calculate the molar mass for each of the following: a. \(\mathrm{FeSO}_{4}\) (iron supplement) b. \(\mathrm{Al}_{2} \mathrm{O}_{3}\) (absorbent and abrasive) c. \(\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{NO}_{3} \mathrm{~S}\) (saccharin) d. \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}\) (rubbing alcohol) e. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{CO}_{3}\) (baking powder)

Calculate the molar mass for each of the following: a. Cl2 b. C3H6O3 c. Mg31PO422 d. AlF3 e. C2H4Cl2

Calculate the molar mass for each of the following: a. O2 b. KH2PO4 c. Fe1ClO423 d. C4H8O4 e. Ga21CO323

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

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

Calculate the number of grams in 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

Calculate the number of grams in each of the following: a. 2.0 moles of MgCl2 b. 3.5 moles of C6H6 c. 5.00 moles of C2H6O d. 0.488 mole of C3H6O3

a. The compound \(\mathrm{MgSO}_{4},\), Epsom salts, is used to soothe sore feet and muscles. 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 \(CO_2\). How many grams of \(CO_2\) are in the bottle?

a. Cyclopropane, \(\mathrm{C}_{3} \mathrm{H}_{6}\), is an anesthetic given by inhalation. How many grams are in 0.25 mole of cyclopropane? b. The sedative Demerol hydrochloride has the formula \(\mathrm{C}_{15} \mathrm{H}_{22} \mathrm{ClNO}_{2}\). How many grams are in 0.025 mole of Demerol hydrochloride?

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

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. 100.0 g of O2

Calculate the number of moles in 25.0 g of each of the following: a. Ne b. O2 c. Al1OH23 d. Ga2S3

Calculate the number of moles in 4.00 g of each of the following: a. He b. SnO2 c. Cr1OH23 d. Ca3N2

How many moles of S are in each of the following quantities? a. 25 g of S b. 125 g of SO2 c. 2.0 moles of Al2S3

How many moles of C are in each of the following quantities? a. 75 g of C b. 0.25 mole of C2H6 c. 88 g of CO2

Dinitrogen oxide 1or nitrous oxide2, N2O, also known as laughing gas, is widely used as an anesthetic in dentistry. a. How many grams of the compound are in 1.50 moles of N2O? b. How many moles of the compound are in 34.0 g of N2O? c. How many grams of N are in 34.0 g of N2O?

Allyl sulfide, C6H10S, is the substance that gives garlic, onions, and leeks their characteristic odor. Some studies indicate that garlic may be beneficial for the heart and in lowering cholesterol. a. How many moles of H are in 0.75 mole of C6H10S? b. How many moles of S are in 23.2 g of C6H10S? c. How many grams of C are in 44.0 g of C6H10S?

Determine whether each of the following chemical equations is balanced or not balanced: a. S1s2 + O21g2 h SO31g2 b. 2Al1s2 + 3Cl21g2 h 2AlCl31s2 c. H21g2 + O21g2 h H2O1g2 d. C3H81g2 + 5O21g2 h 3CO21g2 + 4H2O1g2

Determine whether each of the following chemical equations is balanced or not balanced: a. PCl31s2 + Cl21g2 h PCl51s2 b. CO1g2 + 2H21g2 h CH3OH1g2 c. 2KClO31s2 h 2KCl1s2 + O21g2 d. Mg1s2 + N21g2 h Mg3N21s2

Balance each of the following chemical equations: a. N21g2 + O21g2 h NO1g2 b. HgO1s2 h Hg1l2 + O21g2 c. Fe1s2 + O21g2 h Fe2O31s2 d. Na1s2 + Cl21g2 h NaCl1s2

Balance each of the following chemical equations: a. \(\mathrm{Ca}(s)+\mathrm{Br}_2(l) \longrightarrow \mathrm{CaBr}_2(s)\) b. \(\mathrm{P}_4(s)+\mathrm{O}_2(g) \longrightarrow \mathrm{P}_4 \mathrm{O}_{10}(s)\) c. \(\mathrm{Sb}_2 \mathrm{~S}_3(s)+\mathrm{HCl}(a q) \longrightarrow \mathrm{SbCl}_3(s)+\mathrm{H}_2 \mathrm{~S}(g)\) d. \(\mathrm{Fe}_2 \mathrm{O}_3(s)+\mathrm{C}(s) \longrightarrow \mathrm{Fe}(s)+\mathrm{CO}(g)\)

Balance each of the following chemical equations: a. Mg1s2 + AgNO31aq2 h Mg1NO3221aq2 + Ag1s2 b. Al1s2 + CuSO41aq2 h Al21SO4231aq2 + Cu1s2 c. Pb1NO3221aq2 + NaCl1aq2 h PbCl21s2 + NaNO31aq2 d. Al1s2 + HCl1aq2 h AlCl31aq2 + H21g2

Balance each of the following chemical equations: a. Zn1s2 + HNO31aq2 h Zn1NO3221aq2 + H21g2 b. Al1s2 + H2SO41aq2 h Al21SO4231aq2 + H21g2 c. K2SO41aq2 + BaCl21aq2 h KCl1aq2 + BaSO41s2 d. CaCO31s2 h CaO1s2 + CO21g2

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction: a. \(2 \mathrm{Al}_{2} \mathrm{O}_{3}(s) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{Al}(s)+3 \mathrm{O}_{2}(g)\) b. \(\mathrm{Br}_{2}(g)+\mathrm{BaI}_{2}(s) \longrightarrow \mathrm{BaBr}_{2}(s)+\mathrm{I}_{2}(g)\) c. \(2 \mathrm{C}_{2} \mathrm{H}_{2}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)\) d. \(\mathrm{BaCl}_{2}(a q)+\mathrm{K}_{2} \mathrm{CO}_{3}(a q) \longrightarrow \mathrm{BaCO}_{3}(s)+2 \mathrm{KCl}(a q)\) e. \(\mathrm{Pb}(s)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{PbO}_{2}(s)\)

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction: a. \(\mathrm{H}_{2}(g)+\mathrm{Br}_{2}(g) \longrightarrow 2 \mathrm{HBr}(g)\) b. \(\operatorname{AgNO}_{3}(a q)+\mathrm{NaCl}(a q) \longrightarrow \operatorname{AgCl}(s)+\mathrm{NaNO}_{3}(a q)\) c. \(2 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)\) d. \(\mathrm{Zn}(s)+\mathrm{CuCl}_{2}(a q) \rightarrow \mathrm{Cu}(s)+\mathrm{ZnCl}_{2}(a q)\) e. \(\mathrm{C}_{5} \mathrm{H}_{8}(g)+7 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 5 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)\)

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction: a. 4Fe1s2 + 3O21g2 h 2Fe2O31s2 b. Mg1s2 + 2AgNO31aq2 h Mg1NO3221aq2 + 2Ag1s2 c. CuCO31s2 h CuO1s2 + CO21g2 d. Al21SO4231aq2 + 6KOH1aq2 h 2Al1OH231s2 + 3K2SO41aq2 e. C4H81g2 + 6O21g2 h 4CO21g2 + 4H2O1g2

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction: a. \(\mathrm{CuO}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{CuCl}_2(a q)+\mathrm{H}_2 \mathrm{O}(l)\) b. \(2 \mathrm{Al}(s)+3 \mathrm{Br}_2(g) \longrightarrow 2 \mathrm{AlBr}_3(s)\) c. \(2 \mathrm{C}_2 \mathrm{H}_2(g)+5 \mathrm{O}_2(g) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{CO}_2(g)+2 \mathrm{H}_2 \mathrm{O}(g)\) d. \(\mathrm{Fe}_2 \mathrm{O}_3(s)+3 \mathrm{C}(s) \longrightarrow 2 \mathrm{Fe}(s)+3 \mathrm{CO}(g)\) e. \(\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6(a q) \longrightarrow 2 \mathrm{C}_2 \mathrm{H}_6 \mathrm{O}(a q)+2 \mathrm{CO}_2(g)\)

Using Table 7.5, predict the products that would result from each of the following reactions and balance: a. combination: \(\mathrm{Mg}(s)+\mathrm{Cl}_{2}(g) \longrightarrow\) b. decomposition: \(\mathrm{HBr}(g) \longrightarrow\) c. single replacement: \(\mathrm{Mg}(s)+\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow\) d. double replacement: \(\mathrm{K}_{2} \mathrm{~S}(a q)+\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow\) e. combustion: \(\mathrm{C}_{2} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow}\)

Using Table 7.5, predict the products that would result from each of the following reactions and balance: a. combination: \(\mathrm{Ca}(s)+\mathrm{O}_{2}(g) \longrightarrow\) b. combustion: \(\mathrm{C}_{6} \mathrm{H}_{6}(g)+\mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow}\) c. decomposition: \(\mathrm{PbO}_{2}(s) \stackrel{\Delta}{\longrightarrow}\) d. single replacement: \(\mathrm{KI}(s)+\mathrm{Cl}_{2}(g) \longrightarrow\) e. double replacement: \(\mathrm{CuCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{~S}(a q) \longrightarrow\)

Identify each of the following as an oxidation or a reduction: a. \(\mathrm{Na}^{+}(a q)+e^{-} \longrightarrow \mathrm{Na}(s)\) b. \(\mathrm{Ni}(s) \longrightarrow \mathrm{Ni}^{2+}(a q)+2 e^{-}\) c. \(\mathrm{Cr}^{3+}(a q)+3 e^{-} \stackrel{ }{\longrightarrow} \mathrm{Cr}(s)\) d. \(2 \mathrm{H}^{+}(a q)+2 e^{-} \longrightarrow \mathrm{H}_{2}(g)\)

Identify each of the following as an oxidation or a reduction: a. O21g2 + 4 e- h 2O2-1aq2 b. Ag1s2 h Ag+1aq2 + ec. Fe3+1aq2 + e- h Fe2+1aq2 d. 2Br -1aq2 h Br21l2 + 2 e

In each of the following reactions, identify the reactant that is oxidized and the reactant that is reduced: a. Zn1s2 + Cl21g2 h ZnCl21s2 b. Cl21g2 + 2NaBr1aq2 h 2NaCl1aq2 + Br21l2 c. 2PbO1s2 h 2Pb1s2 + O21g2 d. 2Fe3+1aq2 + Sn2+1aq2 h 2Fe2+1aq2 + Sn4+1aq2

In each of the following reactions, identify the reactant that is oxidized and the reactant that is reduced: a. \(2 \mathrm{Li}(s)+\mathrm{F}_{2}(g) \longrightarrow 2 \mathrm{LiF}(s)\) b. \(\mathrm{Cl}_{2}(g)+2 \mathrm{KI}(a q) \longrightarrow 2 \mathrm{KCl}(a q)+\mathrm{I}_{2}(s)\) c. \(2 \mathrm{Al}(s)+3 \mathrm{Sn}^{2+}(a q) \longrightarrow 2 \mathrm{Al}^{3+}(a q)+3 \mathrm{Sn}(s)\) d. \(\mathrm{Fe}(s)+\mathrm{CuSO}_{4}(a q) \longrightarrow \mathrm{FeSO}_{4}(a q)+\mathrm{Cu}(s)\)

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

Chlorine (\(\mathrm{Cl}_{2}\)) is a strong germicide used to disinfect drinking water and to kill microbes in swimming pools. If the product is \(\mathrm{Cl}^{-}\), was the elemental chlorine oxidized or reduced?

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? C18H32O2 + 2H2 h C18H36O2

In one of the reactions in the citric acid cycle, which provides energy, succinic acid is converted to fumaric acid. C4H6O4 h C4H4O4 + 2H Succinic acid Fumaric acid The reaction is accompanied by a coenzyme, flavin adenine dinucleotide 1FAD2. FAD + 2H h FADH2 a. Is succinic acid oxidized or reduced? b. Is FAD oxidized or reduced? c. Why would the two reactions occur together?

Write all the molemole factors for each of the following chemical equations: a. 2SO21g2 + O21g2 h 2SO31g2 b. 4P1s2 + 5O21g2 h 2P2O51s2

Write all the molemole factors for each of the following chemical equations: a. 2Al1s2 + 3Cl21g2 h 2AlCl31s2 b. 4HCl1g2 + O21g2 h 2Cl21g2 + 2H2O1g2

The chemical reaction of hydrogen with oxygen produces water. 2H21g2 + O21g2 h 2H2O1g2 a. How many moles of O2 are required to react with 2.0 moles of H2? b. How many moles of H2 are needed to react with 5.0 moles of O2? c. How many moles of H2O form when 2.5 moles of O2 reacts?

Ammonia is produced by the chemical reaction of hydrogen and nitrogen. N21g2 + 3H21g2 h 2NH31g2 Ammonia a. How many moles of H2 are needed to react with 1.0 mole of N2? b. How many moles of N2 reacted if 0.60 mole of NH3 is produced? c. How many moles of NH3 are produced when 1.4 moles of H2 reacts?

Carbon disulfide and carbon monoxide are produced when carbon is heated with sulfur dioxide. \(5 \mathrm{C}(s)+2 \mathrm{SO}_{2}(g) \stackrel{\Delta}{\longrightarrow} \mathrm{CS}_{2}(l)+4 \mathrm{CO}(g)\) a. How many moles of C are needed to react with 0.500 mole of \(SO_2\)? b. How many moles of CO are produced when 1.2 moles of C reacts? c. How many moles of \(SO_2\) are needed to produce 0.50 mole of \(CS_2\)? d. How many moles of \(CS_2\) are produced when 2.5 moles of C reacts?

In the acetylene torch, acetylene gas \(\left(\mathrm{C}_2 \mathrm{H}_2\right)\) burns in oxygen to produce carbon dioxide and water. \(2 \mathrm{C}_2 \mathrm{H}_2(g)+5 \mathrm{O}_2(g) \stackrel{\Delta}{\longrightarrow} 4 \mathrm{CO}_2(g)+2 \mathrm{H}_2 \mathrm{O}(g)\) a. How many moles of \(\mathrm{O}_2\) are needed to react with 2.00 moles of \(\mathrm{C}_2 \mathrm{H}_2\)? b. How many moles of \(\mathrm{CO}_2\) are produced when 3.5 moles of \(\mathrm{C}_2 \mathrm{H}_2\) reacts? c. How many moles of \(\mathrm{C}_2 \mathrm{H}_2\) are needed to produce \(0.50\) mole of \(\mathrm{H}_2 \mathrm{O}\)? d. How many moles of \(\mathrm{CO}_2\) are produced from 0.100 mole of \(\mathrm{O}_2\)?

Sodium reacts with oxygen to produce sodium oxide. 4Na1s2 + O21g2 h 2Na2O1s2 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 needed for the reaction? c. How many grams of O2 are needed in a reaction that produces 75.0 g of Na2O?

Nitrogen gas reacts with hydrogen gas to produce ammonia. \(\mathrm{N}_2(g)+3 \mathrm{H}_2(g) \longrightarrow 2 \mathrm{NH}_3(g)\) a. If you have \(3.64 \mathrm{~g}\) of \(\mathrm{H}_2\), how many grams of \(\mathrm{NH}_3\) can be produced? b. How many grams of \(\mathrm{H}_2\) are needed to react with \(2.80 \mathrm{~g}\) of \(\mathrm{N}_2\)? c. How many grams of \(\mathrm{NH}_3\) can be produced from \(12.0 \mathrm{~g}\) of \(\mathrm{H}_2\)?

Ammonia and oxygen react to form nitrogen and water. 4NH31g2 + 3O21g2 h 2N21g2 + 6H2O1g2 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 H2O are formed from the reaction of 34.0 g of NH3?

Iron1III2 oxide reacts with carbon to give iron and carbon monoxide. Fe2O31s2 + 3C1s2 h 2Fe1s2 + 3CO1g2 a. How many grams of C are required to react with 16.5 g of Fe2O3? 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 Fe2O3 reacts?

Nitrogen dioxide and water react to produce nitric acid, HNO3, and nitrogen oxide. 3NO21g2 + H2O1l2 h 2HNO31aq2 + NO1g2 a. How many grams of H2O are needed to react with 28.0 g of NO2? b. How many grams of NO are produced from 15.8 g of NO2? c. How many grams of HNO3 are produced from 8.25 g of NO2?

Calcium cyanamide reacts with water to form calcium carbonate and ammonia. CaCN21s2 + 3H2O1l2 h CaCO31s2 + 2NH31g2 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?

When solid lead1II2 sulfide ore burns in oxygen gas, the products are solid lead1II2 oxide and sulfur dioxide gas. a. Write the balanced chemical equation for the reaction. b. How many grams of oxygen are required to react with 30.0 g of lead1II2 sulfide?

When the gases dihydrogen sulfide and oxygen react, they form the gases sulfur dioxide and water vapor. a. Write the balanced chemical equation for the reaction. b. How many grams of oxygen are needed 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 needed to produce 55.8 g of water vapor?

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

a. What is measured by the heat of reaction? b. How does the heat of reaction differ in exothermic and endothermic reactions?

Classify each of the following as an exothermic or endothermic reaction: 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.

Classify each of the following as an exothermic or endothermic reaction: 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.

Classify each of the following as an exothermic or endothermic reaction: a. CH41g2 + 2O21g2 h CO21g2 + 2H2O1g2 + 802 kJ b. Ca1OH221s2 + 65.3 kJ h CaO1s2 + H2O1l2 c. 2Al1s2 + Fe2O31s2 h Al2O31s2 + 2Fe1s2 + 850 kJ

Classify each of the following as an exothermic or endothermic reaction: a. \(\mathrm{C}_{3} \mathrm{H}_{8}(g)+5 \mathrm{O}_{2}(g) \stackrel{\Delta}{\longrightarrow} 3 \mathrm{CO}_{2}(g)+4 \mathrm{H}_{2} \mathrm{O}(g)+2220 \mathrm{~kJ}\) b. \(2 \mathrm{Na}(s)+\mathrm{Cl}_{2}(g) \longrightarrow 2 \mathrm{NaCl}(s)+819 \mathrm{~kJ}\) c. \(\mathrm{PCl}_{5}(g)+67 \mathrm{~kJ} \longrightarrow \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g)\)

a. What is meant by the rate of a reaction? b. Why does bread grow mold more quickly at room temperature than in the refrigerator?

a. How does a catalyst affect the activation energy? b. Why is pure oxygen used in respiratory distress?

How would each of the following change the rate of the reaction shown here? \(2\mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{SO}_{3}(g)\) a. adding some \(\mathrm{SO}_{2}(g)\) b. increasing the temperature c. adding a catalyst d. removing some \(\mathrm{O}_{2}(g)\)

How would each of the following change the rate of the reaction shown here? \(2 \mathrm{NO}(g)+2 \mathrm{H}_{2}(g) \longrightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)\) a. adding some NO(g) b. lowering the temperature c. removing some \(\mathrm{H}_{2}(g)\) d. adding a catalyst

Using the models of the molecules 1black = C, white = H, yellow = S, green = Cl2, determine each of the following for models of compounds 1 and 2: 17.1, 7.22 1. 2. a. molecular formula b. molar mass c. number of moles in 10.0 g

Using the models of the molecules 1black = C, white = H, yellow = S, red = O2, determine each of the following for models of compounds 1 and 2: 17.1, 7.22 1. 2. a. molecular formula b. molar mass c. number of moles in 10.0 g

A dandruff shampoo contains dipyrithione, C10H8N2O2S2, which acts as an antibacterial and antifungal agent. 17.1, 7.22 a. What is the molar mass of dipyrithione? b. How many moles of dipyrithione are in 25.0 g? c. How many moles of C are in 25.0 g of dipyrithione? d. How many moles of dipyrithione contain 8.2 * 1024 atoms of N?

Ibuprofen, an anti-inflammatory, has the formula C13H18O2. 17.1, 7.22 a. What is the molar mass of ibuprofen? b. How many grams of ibuprofen are in 0.525 mole? c. How many moles of C are in 12.0 g of ibuprofen? d. How many moles of ibuprofen contain 1.22 * 1023 atoms of C?

Balance each of the following by adding coefficients, and identify the type of reaction for each: 17.3, 7.42 a. + b. +

Balance each of the following by adding coefficients, and identify the type of reaction for each: 17.3, 7.42 a. + + +

If red spheres represent oxygen atoms, blue spheres represent nitrogen atoms, and all the molecules are gases, 17.3, 7.42 Reactants Products a. write the formula for each of the reactants and products. b. write a balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

If purple spheres represent iodine atoms, white spheres represent hydrogen atoms, and all the molecules are gases, 17.3, 7.42 Reactants Products a. write the formula for each of the reactants and products. b. write a balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

If blue spheres represent nitrogen atoms, purple spheres represent iodine atoms, the reacting molecules are solid, and the products are gases, 17.3, 7.42 Reactants Products a. write the formula for each of the reactants and products. b. write a balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

If green spheres represent chlorine atoms, yellow-green spheres represent fluorine atoms, white spheres represent hydrogen atoms, and all the molecules are gases, 17.3, 7.42 Reactants Products a. write the formula for each of the reactants and products. b. write a balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

If green spheres represent chlorine atoms, red spheres represent oxygen atoms, and all the molecules are gases, 17.3, 7.42 Reactants Products a. write the formula for each of the reactants and products. b. write a balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

If blue spheres represent nitrogen atoms, purple spheres represent iodine atoms, the reacting molecules are gases, and the products are solid, (7.3, 7.4) Reactants Products a. write the formula for each of the reactants and products. b. write a balanced equation for the reaction. c. indicate the type of reaction as combination, decomposition, single replacement, double replacement, or combustion.

Calculate the molar mass for each of the following: 17.22 a. ZnSO4, zinc sulfate, zinc supplement b. Ca1IO322, calcium iodate, iodine source in table salt c. C5H8NNaO4, monosodium glutamate, flavor enhancer d. C6H12O2, isoamyl formate, used to make artificial fruit syrups

Calculate the molar mass for each of the following: 17.22 a. MgCO3, magnesium carbonate, used in antacids b. Au1OH23, gold1III2 hydroxide, used in gold plating c. C18H34O2, oleic acid, from olive oil d. C21H26O5, prednisone, anti-inflammatory

How many grams are in 0.150 mole of each of the following? 17.22 a. K b. Cl2 c. Na2CO3

How many grams are in 2.25 moles of each of the following? 17.22 a. N2 b. NaBr c. C6H14

How many moles are in 25.0 g of each of the following compounds? 17.22 a. CO2 b. Al2O3 c. MgCl2

How many moles are in 4.00 g of each of the following compounds? 17.22 a. NH3 b. Ca1NO322 c. SO3

Identify the type of reaction for each of the following as combination, decomposition, single replacement, double replacement, or combustion: (7.4) a. A metal and a nonmetal form an ionic compound. b. A compound of hydrogen and carbon reacts with oxygen to produce carbon dioxide and water. c. Heating calcium carbonate produces calcium oxide and carbon dioxide. d. Zinc replaces copper in \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\).

Identify the type of reaction for each of the following as combination, decomposition, single replacement, double replacement, or combustion: (7.4) a. A compound breaks apart into its elements. b. Copper and bromine form copper(II) bromide. c. Iron(II) sulfite breaks down to iron(II) oxide and sulfur dioxide. d. Silver ion from \(AgNO_3\)(aq) forms a solid with bromide ion from KBr(aq).

Balance each of the following chemical equations, and identify the type of reaction: 17.3, 7.42 a. NH31g2 + HCl1g2 h NH4Cl1s2 b. C4H81g2 + O21g2 h CO21g2 + H2O1g2 c. Sb1s2 + Cl21g2 h SbCl31s2 d. NI31s2 h N21g2 + I21g2 e. KBr1aq2 + Cl21aq2 h KCl1aq2 + Br21l2 f. Fe1s2 + H2SO41aq2 h Fe21SO4231aq2 + H21g2 g. Al21SO4231aq2 + NaOH1aq2 h Na2SO41aq2 + Al1OH231s2

Balance each of the following chemical equations, and identify the type of reaction: 17.3, 7.42 a. Si3N41s2 h Si1s2 + N21g2 b. Mg1s2 + N21g2 h Mg3N21s2 c. Al1s2 + H3PO41aq2 h AlPO41aq2 + H21g2 d. C3H41g2 + O21g2 h CO21g2 + H2O1g2 e. Cr2O31s2 + H21g2 h Cr1s2 + H2O1g2 f. Al1s2 + Cl21g2 h AlCl31s2 g. MgCl21aq2 + AgNO31aq2 h Mg1NO3221aq2 + AgCl1s2

Predict the products and write a balanced equation for each of the following: (7.3, 7.4) a. single replacement: \(\mathrm{Zn}(s)+\mathrm{HCl}(a q) \longrightarrow\) ________ + ________ b. decomposition: \(\mathrm{BaCO}_{3}(s) \stackrel{\Delta}{\longrightarrow}\) ________ + ________ c. double replacement: \(\mathrm{NaOH}(a q)+\mathrm{HCl}(a q) \longrightarrow\) ________ + _________ d. combination: \(\mathrm{Al}(s)+\mathrm{F}_{2}(g) \longrightarrow\) ________

Predict the products and write a balanced equation for each of the following: (7.3, 7.4) a. decomposition: \(\operatorname{NaCl}(s) \stackrel{\text { Electricity }}{\longrightarrow}\) ______ + ______ b. combination: \(\mathrm{Ca}(s)+\mathrm{Br}_2(g) \longrightarrow\) ______ c. combustion: \(\mathrm{C}_2 \mathrm{H}_4(g)+\mathrm{O}_2(g) \stackrel{\Delta}{\longrightarrow}\) ______ + ______ d. double replacement: \(\mathrm{NiCl}_2(a q)+\mathrm{NaOH}(a q) \longrightarrow\) ______ + ______

Identify each of the following as an oxidation or a reduction reaction: 17.52 a. Zn2+1aq2 + 2 e- h Zn1s2 b. Al1s2 h Al 3+1aq2 + 3 ec. Pb1s2 h Pb2+1aq2 + 2 ed. Cl21g2 + 2 e- h 2Cl -1aq2

Write a balanced chemical equation for each of the following oxidation-reduction reactions: (7.3, 7.5) a. Sulfur reacts with molecular chlorine to form sulfur dichloride. b. Molecular chlorine and sodium bromide react to form molecular bromine and sodium chloride. c. Aluminum metal and iron(III) oxide react to produce aluminum oxide and elemental iron. d. Copper(II) oxide reacts with carbon to form elemental copper and carbon dioxide.

When ammonia 1NH32 reacts with fluorine, the products are dinitrogen tetrafluoride 1N2F42 and hydrogen fluoride 1HF2 17.3, 7.6, 7.72. a. Write the balanced chemical equation. b. How many moles of each reactant are needed to produce 4.00 moles of HF? c. How many grams of F2 are needed to react with 25.5 g of NH3? d. How many grams of N2F4 can be produced when 3.40 g of NH3 reacts?

When nitrogen dioxide 1NO22 from car exhaust combines with water in the air, it forms nitric acid 1HNO32, which causes acid rain, and nitrogen oxide. 17.3, 7.6, 7.72 a. Write the balanced chemical equation. b. How many moles of each product are produced from 0.250 mole of H2O? c. How many grams of HNO3 are produced when 60.0 g of NO2 completely reacts? d. How many grams of NO2 are needed to form 75.0 g of HNO3?

Pentane gas, C5H12, undergoes combustion with oxygen to produce carbon dioxide and water. 17.3, 7.6, 7.72 a. Write the balanced chemical equation. b. How many grams of C5H12 are needed to produce 72 g of water? c. How many grams of CO2 are produced from 32.0 g of O2?

Propane gas, \(\mathrm{C}_{3} \mathrm{H}_{8}\), reacts with oxygen to produce water and carbon dioxide. Propane has a density of 2.02 g/L at room temperature. (7.3, 7.6, 7.7) a. Write the balanced chemical equation. b. How many grams of \(H_2O\) form when 5.00 L of \(\mathrm{C}_{3} \mathrm{H}_{8}\) reacts? c. How many grams of \(CO_2\) are produced from 18.5 g of \(O_2\)? d. How many grams of \(H_2O\) can be produced from the reaction of 100. g of \(\mathrm{C}_{3} \mathrm{H}_{8}\)?

The equation for the formation of silicon tetrachloride from silicon and chlorine is 17.82 Si1s2 + 2Cl21g2 h SiCl41g2 + 157 kcal a. Is the formation of SiCl4 an endothermic or exothermic reaction? b. Is the energy of the product higher or lower than the energy of the reactants?

The equation for the formation of nitrogen oxide is 17.82 N21g2 + O21g2 + 90.2 kJ h 2NO1g2 a. Is the formation of NO an endothermic or exothermic reaction? b. Is the energy of the product higher or lower than the energy of the reactants?

At a winery, glucose 1C6H12O62 in grapes undergoes fermentation to produce ethanol 1C2H6O2 and carbon dioxide. 17.72 C6H12O6 h 2C2H6O + 2CO2 Glucose 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?

Gasohol is a fuel containing ethanol 1C2H6O2 that burns in oxygen 1O22 to give carbon dioxide and water. 17.3, 7.6, 7.72 a. Write the balanced chemical equation. 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 burn 125 g of C2H6O, how many grams of CO2 and H2O can be produced?

Consider the following unbalanced equation: 17.3, 7.4, 7.6, 7.72 Al1s2 + O21g2 h Al2O31s2 a. Write the balanced chemical equation. b. Identify the type of reaction. c. How many moles of O2 are needed to react with 4.50 moles of Al? d. How many grams of Al2O3 are produced when 50.2 g of Al reacts? e. When Al is reacted in a closed container with 8.00 g of O2, how many grams of Al2O3 can form?

A toothpaste contains 0.240% by mass sodium fluoride used to prevent dental caries and 0.30% by mass triclosan \(\mathrm{C}_{1} \mathrm{H}_{7} \mathrm{Cl}_{3} \mathrm{O}_{2}\), an antigingivitis agent. One tube contains 119 g of toothpaste. (7.1, 7.2) a. How many moles of NaF are in the tube of toothpaste? b. How many fluoride ions, \(\mathrm{F}^{-}\), are in the tube of toothpaste? c. How many grams of sodium ion, \(\mathrm{Na}^{+}\), are in 1.50 g of toothpaste? d. How many molecules of triclosan are in the tube of toothpaste?

During heavy exercise and workouts, lactic acid, C3H6O3, accumulates in the muscles where it can cause pain and soreness. 17.1, 7.22

Ammonium sulfate, 1NH422SO4, is used in fertilizers to provide nitrogen for the soil. 17.1, 7.22 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?

The gaseous hydrocarbon acetylene, C2H2, used in welders torches, releases 1300 kJ when 1 mole of C2H2 undergoes combustion. 17.1, 7.3, 7.6, 7.7, 7.82 a. Write a balanced equation for the reaction, including the heat of reaction. b. Is the reaction endothermic or exothermic? c. How many moles of H2O are produced when 2.00 moles of O2 reacts? d. How many grams of O2 are needed to react with 9.80 g of C2H2?

Methanol 1CH3OH2, which is used as a cooking fuel, burns with oxygen gas 1O22 to produce the gases carbon dioxide 1CO22 and water 1H2O2. The reaction produces 363 kJ of heat per mole of methanol. 17.1, 7.3, 7.6, 7.7, 7.82 a. Write a balanced equation for the reaction, including the heat of reaction. b. Is the reaction endothermic or exothermic? c. How many moles of O2 must react with 0.450 mole of CH3OH? d. How many grams of CO2 are produced when 78.0 g of CH3OH reacts?