Matching
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Match each item with the correct statement below. a. | molar volume | b. | molar mass | c. | atomic
mass |
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1.
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the number of grams of an element that is numerically equal to the atomic mass
of the element in amu
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2.
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the mass of a mole of any element or compound
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3.
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the volume occupied by a mole of any gas at STP
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Match each item with the correct statement below. a. | representative particle | c. | empirical
formula | b. | mole | d. | percent composition |
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4.
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the percent by mass of each element in a compound
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5.
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an atom, an ion, or a molecule, depending upon the way a substance commonly
exists
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6.
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the SI unit used to measure amount of substance
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7.
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the smallest whole number ratio of the atoms in a compound
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8.
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What is the sum of the atomic masses of all the atoms in a formula for a
compound?
a. | molecular mass | b. | formula mass | c. | atomic mass | d. | actual
mass |
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9.
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The volume of one mole of a substance is 22.4 L at STP for all ____.
a. | gases | b. | liquids | c. | solids | d. | compounds |
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10.
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The formula for carbon dioxide, CO2, can represent
a. | one molecule of carbon dioxide. | b. | 1 mol of carbon dioxide
molecules. | c. | the combination of 1 atom of carbon and 2 atoms of oxygen. | d. | all of the
above. |
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11.
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What is the formula mass of ethyl alcohol, C2H5OH?
a. | 30.33 amu | b. | 33.27 amu | c. | 45.06 amu | d. | 46.08
amu |
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12.
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Using 1 mole He = 6.02 × 1023 atoms =
4.0 grams = 22.4 L at
STP
A
B
C D
What is
the number of moles in 500 L of He gas at STP?
a. | 0.05 mol | b. | 0.2 mol | c. | 22 mol | d. | 90
mol |
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13.
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The molar mass of NO2 is 46.01 g/mol. How many moles of
NO2 are present in 114.95 g?
a. | 0.4003 mol | b. | 1.000 mol | c. | 2.498 mol | d. | 114.95
mol |
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14.
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The molar mass of CS2 is 76.15 g/mol. How many grams of
CS2 are present in 10.00 mol?
a. | 0.13 g | b. | 7.615 g | c. | 10.00 g | d. | 761.5
g |
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15.
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Calculate the number of molecules in 4.0 mol H2O.
a. | 0.60 ´ 1023 molecules | c. | 2.4 ´ 10–23 molecules | b. | 2.4 ´ 1024 molecules | d. | 2.4 ´
1023 molecules |
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16.
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The molar mass of H2O is 18.02 g/mol. How many grams of
H2O are present in 0.20 mol?
a. | 0.2 g | b. | 3.6 g | c. | 35.9 g | d. | 89.9
g |
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17.
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What is the volume, in Liters, of 0.500 mol of CO2?
a. | 11. 2 L | b. | 22.4 L | c. | 56.0 L | d. | 44
L |
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18.
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The percentage composition of sulfur in SO2 is about 50%. What is the
percentage of oxygen in this compound?
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19.
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What is the percentage composition by mass of CO2?
a. | 50% C, 50% O | c. | 33.3% C, 67.7% O | b. | 12% C, 88% O | d. | 27.3% C, 72.7%
O |
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20.
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What is the empirical formula for a compound that is 43.6% phosphorus and 56.4%
oxygen?
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21.
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A compound contains 64 g of O and 8 g of H. What is the empirical formula for
this compound?
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22.
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A molecular compound has the empirical formula XY3. Which of the
following is a possible molecular formula?
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23.
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What is the empirical formula for a compound that is 31.9% potassium, 28.9%
chlorine, and 39.2% oxygen?
a. | KClO2 | b. | KClO3 | c. | K2Cl2O3 | d. | K2Cl2O5 |
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24.
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A compound's empirical formula is N2O5. If the
formula mass is 108 amu, what is the molecular formula?
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25.
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A compound's empirical formula is CH. If the formula mass is 52 amu, what
is the molecular formula?
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