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Final Prep Chap 8&9
(DO NOT WRITE ON THIS TEST)
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. After the correct formula for a reactant in an equation has been written, the
a. subscripts are adjusted to balance the equation.
b. formula should not be changed.
c. same formula must appear as the product.
d. symbols in the formula must not appear on the product side of the equation.
____
2. A chemical formula written over the arrow in a chemical equation signifies
a. a byproduct.
c. a catalyst for the reaction.
b. the formation of a gas.
d. an impurity.
____
3. Which coefficients correctly balance the formula equation CaO + H 2 O → Ca(OH) 2 ?
a. 2, 1, 2
c. 1, 2, 1
b. 1, 2, 3
d. 1, 1, 1
____
4. In what kind of reaction does a single compound produce two or more simpler substances?
a. decomposition reaction
c. single-replacement reaction
b. synthesis reaction
d. ionic reaction
____
5. The equation A + BX → AX + B is the general equation for a
a. double-replacement reaction.
c. single-replacement reaction.
b. decomposition reaction.
d. combustion reaction.
____
6. In what kind of reaction do the ions of two compounds exchange places in aqueous solution to form two new
compounds?
a. synthesis reaction
c. decomposition reaction
b. double-replacement reaction
d. combustion reaction
____
7. The reaction 2Mg(s) + O 2 (g) → 2MgO(s) is a
a. synthesis reaction.
c. single-replacement reaction.
b. decomposition reaction.
d. double-replacement reaction.
____
8. In one type of synthesis reaction, an element combines with oxygen to yield a(n)
a. acid.
c. oxide.
b. hydroxide.
d. metal.
____
9. When heated, a metal carbonate decomposes into a metal oxide and
a. carbon.
c. oxygen.
b. carbon dioxide.
d. hydrogen.
____ 10. The formulas for the products of the reaction between sodium hydroxide and sulfuric acid are
a. Na 2 SO 4 and H 2 O.
c. SI 4 and Na 2 O.
b. NaSO 4 and H 2 O.
d. S + O 2 and Na.
____ 11. Predict what happens when nickel is added to a solution of potassium chloride.
a. No reaction occurs.
c. Potassium nickel chloride forms.
b. Nickel chloride forms.
d. Hydrochloric acid forms.
____ 12. Which reaction can be predicted from the activity series?
a. 2Cl → Cl 2
c. 2HCl + 2Na → 2NaCl + H 2
b. HCl + NaOH → NaCl + H 2 O
d. Cl 2 → 2Cl
____ 13. In the chemical reaction wA + xB → yC + zD, a comparison of the number of moles of A to the number of
moles of C would be a(n)
a. mass ratio.
c. electron ratio.
b. mole ratio.
d. energy proportion.
____ 14. For the reaction N 2 + 3H 2 → 2NH 3 , how many moles of nitrogen are required to produce 18 mol of
ammonia?
(SHOW YOUR WORK)
a. 9.0 mol
c. 27 mol
b. 18 mol
d. 36 mol
Element
Bromine
Calcium
Carbon
Chlorine
Cobalt
Symbol
Br
Ca
C
Cl
Co
Copper
Fluorine
Cu
F
Hydrogen
H
Iodine
Iron
Lead
Magnesium
Mercury
Nitrogen
I
Fe
Pb
Mg
Hg
N
Oxygen
Potassium
Sodium
O
K
Na
Sulfur
S
Atomic mass
79.904
40.078
12.011
35.4527
58.933
20
63.546
18.998
4032
1.007
94
126.904
55.847
207.2
24.3050
200.59
14.006
74
15.9994
39.0983
22.989
768
32.066
____ 15. For the reaction 3Fe + 4H 2 O → Fe 3 O 4 + 4H 2 , how many moles of iron oxide are produced from 500 g of
iron?
(SHOW YOUR WORK)
a. 1 mol
c. 9 mol
b. 3 mol
d. 12 mol
____ 16. For the reaction SO 3 + H 2 O → H 2 SO 4 , how many grams of sulfuric acid can be produced from 200. g of
sulfur trioxide and 100. g of water?
(SHOW YOUR WORK)
a. 100. g
c. 245 g
b. 200. g
d. 285 g
____ 17. In the reaction A + B → C + D, if the quantity of B is insufficient to react with all of A,
a. A is the limiting reactant.
c. there is no limiting reactant.
b. B is the limiting reactant.
d. no product can be formed.
____ 18. What is the maximum possible amount of product obtained in a chemical reaction?
a. theoretical yield
c. mole ratio
b. percent yield
d. actual yield
____ 19. A chemist interested in the efficiency of a chemical reaction would calculate the
a. mole ratio.
c. percent yield.
b. energy released.
d. rate of reaction.
____ 20. A chemical reaction has NOT occurred if the products have
a. the same mass as the reactants.
b. less total bond energy than the reactants.
c. more total bond energy than the reactants.
d. the same chemical properties as the reactants.
____ 21. To balance a chemical equation, it may be necessary to adjust the
a. coefficients.
c. formulas of the products.
b. subscripts.
d. number of products.
____ 22. Which equation is NOT balanced?
a. 2H 2 + O 2 → 2H 2 O
b. 4H 2 + 2O 2 → 4H 2 O
c. H 2 + H 2 + O 2 → H 2 O + H 2 O
d. 2H 2 + O 2 → H 2 O
____ 23. An active metal and a halogen react to form a(n)
a. salt.
c. acid.
b. hydroxide.
d. oxide.
____ 24. In the equation 2Al(s) + 3Fe(NO 3 ) 2 (aq) → 3Fe(s) + 2Al(NO 3 ) 3 (aq), iron has been replaced by
a. nitrate.
c. aluminum.
b. water.
d. nitrogen.
____ 25. If a certain metal is placed in an ionic solution containing another metal and no reaction occurs, then the metal
originally in the solution is
a. a halogen.
c. not on the activity series.
b. higher on the activity series.
d. unreactive.
____ 26. A balanced chemical equation allows one to determine the
a. mole ratio of any two substances in the reaction.
b. energy released in the reaction.
c. electron configuration of all elements in the reaction.
d. mechanism involved in the reaction.
____ 27. The coefficients in a chemical equation represent the
a. masses, in grams, of all reactants and products.
b. relative numbers of moles of reactants and products.
c. number of atoms in each compound in a reaction.
d. number of valence electrons involved in the reaction.
____ 28. To determine the limiting reactant in a chemical reaction involving known masses of A and B, one could first
calculate
a. the mass of 100 mol of A and B.
b. the masses of all products.
c. the bond energies of A and B.
d. the number of moles of B and the number of moles of A available.
____ 29. What is the ratio of the actual yield to the theoretical yield, multiplied by 100%?
a. mole ratio
c. Avogadro yield
b. percent yield
d. excess yield
Problem
(SHOW YOUR WORK)
Element
Bromine
Calcium
Carbon
Chlorine
Cobalt
Symbol
Br
Ca
C
Cl
Co
Copper
Fluorine
Cu
F
Hydrogen
H
Iodine
Iron
Lead
Magnesium
Mercury
Nitrogen
I
Fe
Pb
Mg
Hg
N
Oxygen
Potassium
Sodium
O
K
Na
Sulfur
S
Atomic mass
79.904
40.078
12.011
35.4527
58.933
20
63.546
18.998
4032
1.007
94
126.904
55.847
207.2
24.3050
200.59
14.006
74
15.9994
39.0983
22.989
768
32.066
30. What mass in grams of hydrogen gas is produced if 20.0 mol of Zn are added to excess hydrochloric acid
according to the equation Zn(s) +2HCl(aq) → ZnCl 2 (aq) + H 2 ( )?
final Prep
Answer Section
MULTIPLE CHOICE
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B
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D
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C
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B
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PROBLEM
30. ANS:
40.4 g H 2
PTS: 1
DIF: III
OBJ: 9-3.2
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8-1.2
8-1.3
8-1.4
8-2.1
8-2.1
8-2.1
8-2.2
8-2.3
8-2.3
8-2.5
8-3.2
8-3.2
9-1.2
9-2.1
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9-3.1
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8-1.1
8-1.2
8-1.4
8-2.3
8-2.4
8-3.1
9-1.2
9-1.2
9-3.1
9-3.3