Complete and balance the equations for the following single-displacement reactions: a

List four observations that indicate that a chemical reaction may be taking place.

List the three requirements for a correctly written chemical equation.

a. What is meant by the term coefficient in relation to a chemical equation? / b. How does the presence of a coefficient affect the number of atoms of each type in the for- mula that the coefficient precedes?

Give an example of a word equation, a formula equation, and a chemical equation.

What quantitative information is revealed by a chemical equation?

What limitations are associated with the use of both word and formula equations?

Define each of the following terms: a. aqueous solution b. catalyst c. reversible reaction

Write formulas for each of the following compounds: a. potassium hydroxide b. calcium nitrate c. sodium carbonate d. carbon tetrachloride e. magnesium bromide

What four guidelines are useful in balancing an equation?

How many atoms of each type are represented in each of the following? a. 3N2 f. 5Fe(NO3)2 b. 2H20 g. 4Mg3(PO4)2 c. 4HNO3 h. 2(NH4)2SO4 d. 2Ca(OH)2 i. 6Al(SeO)3 e. 3Ba(C103)2 j. 4C3H8

Write the chemical equation that relates to each of the following word equations. Include symbols for physical states in the equation. a. solid zinc sulfide + oxygen gas -* solid zinc oxide + sulfur dioxide gas b. aqueous hydrochloric acid + aqueous barium hydroxide -+ aqueous barium chloride + water c. aqueous nitric acid + aqueous calcium hydroxide -* aqueous calcium nitrate + water

Translate each of the following chemical equations into a sentence. a. 2ZnS(s) + 302(g) -. 2ZnO(s) + 2S02(9) b. CaH2(s) + 2H20(0 -* Ca(OH)2(aq) + 2H2(g) c. AgNO3(aq) + KI(aq) -p AgI(s) + KNO3(aq)

Balance each of the following: a. H2 +C12 HCl b. Al+Fe203 *A1203 +Fe c. Pb(CH3COO)2+ H2S -p PbS + CH3COOH

Identif and correct each error in the following equations, 4nd then balance each equation. a. Li+02 *Li02 / b. H2+ C12-* H2C12 / C- MgCO3-f M902+ CO2 d. NaI-Cl2 ---- NaCl +I

Write chemical equations for each of the following sentences: a. Aluminum reacts with oxygen to produce aluminum oxide. b. Phosphoric acid, H3PO4, is produced through the reaction between tetraphosphorus decoxide and water. c. Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide.

Carbon tetrachloride is used as an intermediate chemical in the manufacture of other chemicals. It is prepared in liquid form by reacting chlorine gas with methane gas. Hydrogen chloride gas is also formed in this reaction. Write the balanced chemical equation for the production of carbon tetrachloride. (Hint: See Sample Problems C and D.)

For each of the following synthesis reactions, identify the missing reactant(s) or product(s), and then balance the resulting equation. a.Mg+ *MgO b. + 02 * Fe203 c. d. Ca+

Define and give general equations for the five basic types of chemical reactions introduced in Chapter 8.

How are most decomposition reactions initiated?

A substance is decomposed by an electric current. What is the name of this type of reaction?

a. In what environment do many singledisplacement reactions commonly occur? b. In general, how do single-displacement reactions compare with synthesis and decomp9sition reactions in terms of the amount of energy involved?

Complete each of the following synthesis reactions by writing both a word equation and a chemical equation. a. sodium + oxygen b. magnesium + fluorine

Complete and balance the equations for the following decomposition reactions: a. HgO -- b. H20(1) electricity > c. Ag20 --* d. CuC12 electricity

Complete and balance the equations for the following single-displacement reactions: a. Zn + Pb(NO3)2 b. Al + Hg(CH3COO)2 c. Al + NiSO4 d. Na+H20*

Complete and balance the equations for the following double-displacement reactions: a. AgNO3(aq) + NaC1(aq) b. Mg(NO3)2(aq) + KOH(aq) c. LiOH(aq) + Fe(NO3)3(aq)

Complete and balance the equations for the following combustion reactions: a. CH4 +02 l. b. C3H+02 * c. C5H12 +02

Write and balance each of the following equations, and then identify each by type. a. hydrogen + iodine * hydrogen iodide b. lithium + hydrochloric acid * lithium chloride + hydrogen c. sodium carbonate sodium oxide + carbon dioxide d. mercury(II) oxide --- mercury + oxygen e. magnesium hydroxide -~ magnesium oxide + water

Identify the compound that could undergo decomposition to produce the following products, and then balance the final equation. a. magnesium oxide and water b. lead(II) oxide and water c. lithium chloride and oxygen d. barium chloride and oxygen e. nickel chloride and oxygen

In each of the following combustion reactions, identify the missing reactant(s), product(s), or both, and then balance the resulting equation. a. C3H8 + - ____ +H0 b. +802 *5CO2 +6H20 c. C2H50H+ * +

Complete and balance the equations for the following reactiops, and then identify each by type. a. zinc + sulfur b. silver nitrate + potassium iodide c. tQluene, C7H8 toxygen d. nonane, C9H20 + oxygen

a. What is meant by the activity of an element? b. How does this description differ for metals and nonmetals?

a. What is an activity series of elements? b. What is the basis for the ordering of the elements in the activity series?

a. What chemical principle is the basis for the activity series of metals? b. What is the significance of the distance between two metals in the activity series?

Based on the activity series of metals and halo- 40. gens, which element within each pair is more likely to replace the other in a compound? a. K and Na e. Au and Ag b. Al and Ni f. Cl and I c. Bi and Cr g. Fe and Sr 41 d. Cl and F h. I and F

Using the activity series in Table 3 on page 286, predict whether each of the possible reactions listed below will occur. For the reactions that will occur, write the products and balance the equation. a. Ni(s) + CuCl2(aq) -p b. Zn(s) + Pb(NO3)2(aq) C- C12(9) + KI(aq) d. Cu(s) + FeSO4(aq) e. Ba(s)+H20(1)-4

Use the activity series to predict whether each of the following synthesis reactions will occur, 43. and write the chemical equations for those predicted to occur. a. Ca(s) + 02(g) -* b. Ni(s) + 02(g) -4 c. Au(s) + 02(g) -

Ammonia reacts with oxygen to yield nitrogen and water. 4NH3(9) + 302(g) -* 2N2(9) + 6H20(1) Given this chemical equation, as well as the number of moles of the reactant or product indicated below, determine the number of moles of all remaining reactants and products. a. 3.0 mol 02 c. 1.0 mol N2 b. 8.0 mol NH3 d. 0.40 mol H20

Complete the following synthesis reactions by writing both the word and chemical equation for each: a. potassium + chlorine b. hydrogen + iodine c. magnesium + oxygen

Use the activity series to predict which metalSn, Mn, or Ptwould be the best choice as a container for an acid.

Aqueous sodium hydroxide is produced commercially by the electrolysis of aqueous sodium chloride. Hydrogen and chlorine gases are also produced. Write the balanced chemical equation for the production of sodium hydroxide. Include the physical states of the reactants and products.

Balance each of the following: a. Ca(OH)2+ (NH4)2SO4-* CaSO4+ NH3+ H20 b. C2H6 +02 *CO2 +H20 C- Cu2S + 02* Cu20 + SO2 d. Al + H2SO4 - Al2(SO4)3+ H2

Use the activity series to predict whether each of the following reactions will occur, and write the balanced chemical equations for those predicted to occur. a. Al(s) + 02(g) b. Pb(s) + ZnC12(s)

Complete and balance the equations for the following reactions, and identify the type of reaction that each equation represents. a. (NH4)2S(aq) + ZnC12(aq) -* + ZnS(s) b. Al(s) + Pb(NO3)2(aq) c. Ba(s) + H20(1) d. C12(g) + KBr(aq) -4 e. NH3(9) + 02(g) -- N0(g) + H20(1) L H20(1) -4 H2(9) + 02(g)

Write and balance each of the following equations, and then identify each by type. a. copper + chlorine -9 copper(II) chloride b. calcium chlorate -* calcium chloride + oxygen C. lithium + water -* lithium hydroxide + hydrogen d. lead(II) carbonate -* lead(II) oxide + carbon dioxide

How many moles of HCl can be made from 6.15 mol H2and an excess of C12?

What product is missing in the following wrote in (a) and (b). equation? MgO + 2110 -p MgC12 + _____

Balance the following equations: a. Pb(NO3)2(aq) + NaOH(aq) - Pb(OH)2(s) + NaNO3(aq) b. C12H22011(l) + 02(g) -) CO2(9) + H20(l) C. Al(OH)3(s) + H2SO4(aq) _.... (SO4)3(aq) + H20(l)

Inferring Relationships Activity series are prepared by comparing single-displacement reactions between metals. Based on observations, the metals can be ranked by their ability to react. However, reactivity can be explained by the ease with which atoms of metals lose electrons. Using information from the activity series, identify the locations in the periodic table of the most reactive metals and the least reactive metals. Using your knowledge of electron configurations and periodic trends, infer possible explanations for the metals' reactivity and position in the periodic table.

Analyzing Results Formulate an activity series for the hypothetical elements A, J, Q, and Z by using the following reaction information: A + ZX -3 AX + z J + ZX no reaction 0+ AX + OX + A

Find the common-reactions section for Group 1 metals in the Elements Handbook. Use this information to answer the following: a. Write a balanced chemical equation for the formation of rubidium hydroxide from rubidum oxide. b. Write a balanced chemical equation for the formation of cesium iodide. c. Classify the reactions you wrote in (a) and (b). d. Write word equations for the reactions you wrote in (a) and (b).

Find the common-reactions section for Group 13 in the Elements Handbook. Use this information to answer the following: a. Write a balanced chemical equation for the formation of gallium bromide prepared from hydrobromic acid. b. Write a balanced chemical equation for the formation of gallium oxide. c. Classify the reactions you wrote in (a) and (b). d. Write word equations for the reactions you wrote in (a) and (b).

Trace the evolution of municipal water fluoridation. What advantages and disadvantages are associated with this practice?

Research how a soda-acid fire extinguisher works, and write the chemical equation for the reaction. Check your house and other structures for different types of fire extinguishers, and ask your local fire department to verify the effectiveness of each type of extinguisher.

Performance Assessment For one day, record situations that show evidence of a chemical change. Identify the reactants and the products, and determine whether there is proof of a chemical reaction. Classify each of the chemical reactions according to the common reaction types discussed in the chapter.