Multiple Choice
Identify the
choice that best completes the statement or answers the question.
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1.
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What is the formula for the compound formed by lead(II) ions and chromate
ions?
a. | PbCrO4 | c. | Pb2(CrO4)3 | b. | Pb2CrO4 | d. | Pb(CrO4)2 |
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2.
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What is the formula for tin(IV) chromate?
a. | Sn(CrO4)4 | c. | Sn2(CrO4)4 | b. | Sn2(CrO4)2 | d. | Sn(CrO4)2 |
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3.
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Name the compound Zn3(PO4)2.
a. | zinc potassium oxide | c. | zinc phosphate | b. | trizinc polyoxide | d. | zinc phosphite |
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4.
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Name the compound KClO3.
a. | potassium chloride | c. | potassium chlorate | b. | potassium trioxychlorite | d. | hypochlorite |
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5.
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What is the name of Sn3(PO4)4 under the Stock
system of nomenclature?
a. | stannous phosphate | c. | tin(III) phosphate | b. | tin(IV) phosphate | d. | tin(II)
phosphate |
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6.
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Using the Stock system, name the compound PbO.
a. | plumbous oxide | c. | potassium oxide | b. | lead oxide | d. | lead(II) oxide |
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7.
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Name the compound SiO2.
a. | silver oxide | c. | silicon dioxide | b. | silicon oxide | d. | monosilicon
dioxide |
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8.
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Name the compound SO3.
a. | sulfur trioxide | c. | selenium trioxide | b. | silver trioxide | d. | sodium trioxide |
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9.
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If 245 J is required to change the temperature of 14.4 g of chromium by 38.0 K,
what is the specific heat capacity of chromium?
a. | 0.448 J/g×K | b. | 2.23 J/g×K | c. | 4.18 J/g×K | d. | 4.68 J/g×K | e. | 92.8 J/g×K |
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10.
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Calculate the energy in the form of heat (in kJ) required to change 50.0 g ice
at –15.0 °C to liquid at 65.0 °C. (Heat of fusion = 333 J/g; heat of vaporization = 2256 J/g; specific
heat capacities: ice = 2.06 J/g×K, liquid water = 4.184 J/g×K)
a. | 15.5 kJ | b. | 16.7 kJ | c. | 31.8
kJ | d. | 128 kJ | e. | 145 kJ |
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11.
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What is the H3O+ concentration in 5.8 ´ 10–4 M KOH(aq) at 25 °C?
(Kw = 1.0 ´ 10–14)
a. | 5.8 ´ 10–18 M | b. | 1.7 ´ 10–11 M | c. | 5.8 ´
10–4 M | d. | 11 M | e. | 5.8 ´ 1010 M |
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12.
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What is the pH of 4.4 ´ 10–4 M
KOH(aq) at 25 °C? (Kw = 1.0 ´ 10–14)
a. | –3.36 | b. | 3.36 | c. | 6.27 | d. | 7.73 | e. | 10.64 |
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13.
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What units are used to measure heat?
a. | joules/mole or kilojoules/mole | c. | joules or
kilojoules | b. | kelvins or degrees Celsius | d. | None of the above |
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14.
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A 4.0 g sample of iron was heated from 0ºC to 20.ºC. It absorbed 35.2
J of energy as heat. What is the specific heat of this piece of iron?
a. | 2816 J/g·ºC | c. | 2.27 J/g | b. | 2.27 J/g·ºC | d. | 0.44
J/g·ºC |
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15.
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Which of the following is a measure of the disorder in a system?
a. | entropy | c. | free energy | b. | enthalpy | d. | temperature |
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16.
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In the reaction 2H2 + O2 ®
2H2O, what is the mole ratio of oxygen to water?
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17.
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For the reaction 2H2 + O2®
2H2O, how many moles of water can be produced from 6.0 mol of oxygen?
a. | 2.0 mol | c. | 12 mol | b. | 6.0 mol | d. | 18 mol |
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| Element | Symbol | Atomic mass | | Bromine | Br | 79.904 | | Calcium | Ca | 40.078 | | Carbon | C | 12.011 | | Chlorine | Cl | 35.4527 | | Cobalt | Co | 58.933 20 | | Copper | Cu | 63.546 | | Fluorine | F | 18.998 4032 | | Hydrogen | H | 1.007 94 | | Iodine | I | 126.904 | | Iron | Fe | 55.847 | | Lead | Pb | 207.2 | | Magnesium | Mg | 24.3050 | | Mercury | Hg | 200.59 | | Nitrogen | N | 14.006 74 | | Oxygen | O | 15.9994 | | Potassium | K | 39.0983 | | Sodium | Na | 22.989 768 | | Sulfur | S | 32.066 | | | |
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18.
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For the reaction SO3 + H2O ® H2SO4, how many grams of sulfur trioxide are
required to produce 4.00 mol of sulfuric acid?
a. | 80.0 g | c. | 240. g | b. | 160. g | d. | 320. g |
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19.
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What is the formula for nitrogen monoxide?
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20.
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What is the formula for sulfur dichloride?
a. | NaCl2 | c. | S2Cl | b. | SCl2 | d. | S2Cl2 |
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21.
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If 50.0 g of ethanol, CH3CH2OH, at 20.0 °C absorbs 1.45 kJ of heat, what is the final temperature of the ethanol?
The specific heat capacity of ethanol is 2.44 J/g×K.
a. | 8.1 °C | b. | 21.2 °C | c. | 31.9 °C | d. | 47.7 °C | e. | 90.8 °C |
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22.
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What is the pH of 2.75 M HCl(aq) at 25 °C?
(Kw = 1.0 ´ 10–14)
a. | –0.439 | b. | 0.439 | c. | 1.012 | d. | 2.75 | e. | 3.636 |
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23.
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What is the product of H3O+ and OH–
concentrations in water?
a. | 10–28 | c. | 10–7 | b. | 10–14 | d. | 55.4 |
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24.
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Which expression represents the concentration of OH– in
solution?
a. | 10–14 – [H3O+] | c. | 10–14 ¸
[H3O+] | b. | 10–14 ´ [H3O+] | d. | [OH–] ¸ 10–14 |
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25.
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A water solution whose pH is 4
a. | is always neutral. | c. | is always acidic. | b. | is always basic. | d. | might be neutral, basic, or
acidic. |
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26.
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What is the pH of a 10–5 M KOH solution?
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27.
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What is the hydronium ion concentration of a solution whose pH is 7.30?
a. | 1.4 ´ 10–11 M | c. | 5.0 ´ 10–8 M | b. | 3.8 ´
10–8 M | d. | 7.1
´ 10–6 M |
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28.
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In an acid-base titration,
a. | base is always added to acid. | b. | acid is always added to
base. | c. | base is added to acid or acid is added to base. | d. | None of the
above |
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29.
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What is the molarity of an HCl solution if 50.0 mL is neutralized in a titration
by 40.0 mL of 0.400 M NaOH?
a. | 0.200 M | c. | 0.320 M | b. | 0.280 M | d. | 0.500 M |
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30.
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What is the molarity of an NaOH solution if 4.37 mL is titrated by 11.1 mL of
0.0904 M HNO3?
a. | 0.230 M | c. | 0.460 M | b. | 0.355 M | d. | 0.620 M |
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