Chemistry, Pearson Ch. 11 Test A.
Chapter Test A
A. Matching
Match each description in Column B with the correct term in Column A. Write the letter of the correct description on the line.
Column A
1. coefficient → E.
2. spectator ion → G.
3. combustion reaction → J.
4. reactant → B.
5. skeleton equation → A.
6. balanced equation → H.
7. activity series → C.
8. product → F.
9. decomposition reaction → D.
10. single-replacement reaction → I.
Column B
a. a chemical equation that does not indicate relative amounts of reactants and products
b. a starting substance in a chemical reaction
c. a list of metals in order of decreasing reactivity
d. a reaction in which a single compound is broken down into simpler substances
e. a whole number that appears before a formula in an equation
f. a new substance formed in a chemical reaction
g. a particle not directly involved in a chemical reaction
h. an equation in which each side has the same number of atoms of each element
i. a reaction in which the atoms of one element replace the atoms of a second element
j. a reaction in which oxygen reacts with another substance, often producing heat or light
B. Multiple Choice
Choose the best answer and write its letter on the line.
11. The symbol D in a chemical equation means:
a. heat is supplied to the reaction.
b. a catalyst is needed.
c. yields.
d. precipitate.
12. A catalyst is:
a. a solid product of a reaction.
b. one of the reactants in a single-replacement reaction.
c. not used up in a reaction.
d. the product of a combustion reaction.
13. When the equation Fe + O2®Fe2O3 is balanced, the coefficient for O2 is:
a. 4 c. 2
b. 3 d. 1
14. The reaction in question 13 is an example of a(n):
a. aqueous reaction. c. combination reaction.
b. single-replacement reaction. d. decomposition reaction.
15. The equation H3PO4 + 3KOH ®K3PO4 + 3H2O is an example of which type of reaction?
a. double-replacement c. decomposition
b. combination d. single-replacement
16. In a double-replacement reaction:
a. the reactants are usually a metal and a nonmetal.
b. the reactants are generally two ionic compounds in aqueous solution.
c. one of the reactants is often water.
d. energy in the form of heat or light is always produced.
17. In order for the reaction 2Al(s) + 6HCl(aq) ®2AlCl3(aq) + 3H2(g) to occur, which of the following must be true?
a. Al must be above Cl on the activity series.
b. Al must be above H on the activity series.
c. Heat must be supplied for the reaction.
d. AlCl3 must be a precipitate.
18. In a double-replacement reaction:
a. one of the products is always a gas.
b. one of the products must be an element.
c. positive ions are exchanged between two compounds.
d. all of the above
19. When the following equation is balanced, the coefficient in front of HCl is:
Ba(s) + HCl(aq) ®BaCl2(aq) + H2(g)
a. 6 c. 1
b. 3 d. 2
20. The equation in question 19 is an example of which type of reaction?
a. combustion c. decomposition
b. single-replacement d. double-replacement
21. This symbol f indicates:
a. that heat must be applied.
b. an incomplete combustion reaction.
c. that a gas is formed by the reaction.
d. that the reaction is reversible.
22. Which of the following statements is incorrect?
a. Complete combustion has occurred when all the carbon in the product is in the form of carbon dioxide.
b. A single reactant is the identifying characteristic of a decomposition reaction.
c. The only way to determine the products of a reaction is to perform the reaction.
d. All chemical reactions can be classified as one of four general types.
23. A chemical formula written above or below the yield sign indicates:
a. that a gas is formed.
b. that the substance is used as a catalyst.
c. that heat must be supplied.
d. a reversible reaction.
24. The equation 2C3H7OH(g) + 9O2(g) ®6CO2(g) + 8H2O(g) is an example of which type of reaction?
a. combustion c. double-replacement
b. combination d. decomposition
25. A double-replacement reaction takes place when aqueous K2SO4 reacts with aqueous Pb(NO3)2. You would expect one of the products of this reaction to be:
a. K2S. c. PbSO4.
b. NaPb. d. CNO3.
C. Problems
Solve the following problems in the space provided. Show your work.
26. Balance the following equations:
a. Ca(s) + H3PO4(aq) ®Ca3(PO4)2(s) + H2(g)
3Ca(s) + 2H3PO4(aq)
→ Ca3(PO4)2(s) + 3H2(g)
b. KBrO3(s) ®KBr(s) + O2(g)
2KBrO3(s) → 2KBr(s) + 3O2(g)
c. (NH4)2CO3(aq) + NaOH(aq) ®Na2CO3(aq) + NH3(g) + H2O(l)
(NH4)2CO3(aq) + 2NaOH(aq)
→ Na2CO3(aq) + 2NH3(g) + 2H2O(l)
27. For each equation in question 26, identify the type of reaction.
a. Single-replacement
b. Decomposition
c. Double-replacement
28. Balance the following equations. Indicate whether combustion is complete or incomplete.
a. C5H10(g) + O2(g) ®CO(g) + H2O(g)
C5H10(g) + 5O2(g) → 5CO(g) + 5H2O(g) (incomplete)
b. C3H7OH(l) + O2(g) ®CO2(g) + H2O(g)
2C3H7OH(l) + 9O2(g)y6CO2(g) + 8H2O(g) (complete)
29. Complete and balance the following equations. Then write each as a net ionic equation.
a. K3PO4(aq) + MgCl2(aq) →
2K3PO4(aq) + 3MgCl2(aq)
→ Mg3(PO4)2(s) 6KCl(aq)
net: 3Mg2^+(aq) + 2PO4 ^3-(aq)
→ Mg3(PO4)2(s)
b. Fe(NO3)3(aq) + Na2CO3(aq) →
2Fe(NO3)3(aq) + 3Na2CO3(aq)
→ Fe2(CO3)3(s) + 6NaNO3(aq)
net: 2Fe^3+(aq) + 3CO3 ^2-(aq)
→ Fe2(CO3)3(s)
D. Essay
Write a short essay for the following.
30. What determines whether one metal will replace another metal from a compound in a single-replacement reaction?
Whether one metal will replace another is determined by the relative reactivity of the two metals. The activity series of metals lists metals in order of decreasing reactivity. A metal will replace any metal found below it in the activity series.