Chapter 10 Review

A. MULTIPLE CHOICE

1. In the reaction

2C8H18(l) + 2502(g)    =>     16CO2(g) + 18H20(l)

the ratio of the volumes of gaseous products to gaseous reactants is

a. 16 : 25

b. 25 : 16

c. 27 : 34

d. 34 : 27

2. The molar volume of a gas at STP is 22.4 dm3. This volume is closest to the volume of a(n)

a. indoor sports arena.

b. classroom.

c. computer monitor.

d. coffee cup.

3. In the reaction

2CO(g)  +  O2(g=>  2CO2(g)

the volume of CO2 (at STP) produced when 10.0 dm3 of CO is completely reacted is

a. 5.0 dm3.

b. 10.0 dm3.

c. 20.0 dm3.

d. 224.0 dm3.

4. In the reaction

Ca  +  2HCL  =>  Ca Cl2  +  H2

the volume of hydrogen (at STP) formed by reacting 0.05 mol of Ca is

a. 112.0 dm3

b. 22.4 dm3

c. 2.24 dm3

d. 1.12 dm3

5. In the reaction

2C2H6  +  702  =>  4CO2  +  6H2O

the ratio of moles of C2H6 to moles of H2O is

a. 2 : 7

b. 1 : 2

c. 1 : 3

d. 3 : 1

6. Which of the following quantities is conserved in a balanced chemical equation?

a. moles

b. molecules

c. atoms

d. volume

7. To change from moles of the substance sought to mass of the substance sought,

a. divide moles of substance sought by Avogadro’s number.

b. divide moles of substance sought by its molar mass.

c. multiply moles of substance sought by Avogadro’s number.

d. multiply moles of substance sought by its molar mass.

8. To change from moles of the substance given to moles of the substance sought one uses the

a. ratio of molar masses of the two substances.

b. balanced equation coefficients for the substances.

c. subscripts in the formulas for the substances.

d. all of the above.

9. The coefficients in a balanced formula equation give information about the reactants and products that can be used to compare the

a. numbers of particles involved.

b. numbers of moles involved.

c. volumes involved.

d. all of the above.

10. According to Avogadro’s hypothesis, equal volumes of all gases at the same temperature and pressure have the same

a. mass.

b. number of particles.

c. density.

d. none of the above.

B. PROBLEMS

11. For the reaction

4H2O  +  3Fe  =>  FeO4  +  4H2

how many grams of iron oxide (Fe3O4) will be produced if 112 g of iron (Fe) reacts completely with water?

12. For the reaction

Zn  +  2HCL  =>  Zn Cl2  +  H2

what volume of hydrogen gas (H2) at STP will be produced if 130 g of Zn reacts completely with hydrochloric acid (HCL)?

13. For the reaction

H2  +  Br2  =>  2HBr

how many moles of hydrogen bromide (HBr) will be formed if 5.6 dm3 of hydrogen gas (H2) reacts completely with bromine (Br2)?

14. Referring to the reaction

2CuCl(aq)  +  H2S(g=>  Cu2S(s)  +  2HCl(aq)

what amount of Cu2S is formed when 4.95g of CuCl reacts completely with hydrogen sulfide gas?

15. Referring to the reaction

2Na  +  2H2=>  2NaOH  +  H2

how many particles of hydrogen are formed as a result of adding 4.6 g of sodium to water?

C. ESSAY QUESTION

16. Give two reasons why mathematics is important in chemistry.

A. MULTIPLE CHOICE

17. It is possible to cause a reversible reaction to produce more of the products by

a. limiting both of the reactants.

b. limiting one of the reactants.

c. decreasing the concentration of one of the reactants.

d. increasing the concentration of one of the reactants.

18. For the reaction, N2  +  3H2  =>   2NH3, if 3.0 mol of N2 and 2.0 mol of H2 are mixed, the limiting reactant will be

a. N2.

b. H2.

c. NH3.

d. all of the above.

B. PROBLEMS

19. For the reaction CaO  +  H2=>  Ca(OH)2, if 4.0 g of CaO and 7.0 g of H2O are available, what is the limiting reactant and what amount of Ca(OH)2 can be formed?

20. For the reaction 2Na  +  Cl2  =>  2NaCl, how many grams of NaCl could be produced from 23.0 g of Na and 22.4 dm3 of Cl2 (STP)?

21. For the reaction CS2  +  3O2  =>  CO2  +  2SO2, how many dm3 of SO2 can be formed from 152 g of CS2 and 48 g of O2? Identify the limiting reactant.

C. ESSAY QUESTION

22. What are two possible reasons for adding an excess of one of the reactants in a chemical reaction?

If you have any questions, please email Ms. Cummings