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Chapter 11: The Mole

Practice Test
  1.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   6.0 × 1011 g  
  b.   5.3 × 10-11 g  
  c.   1.9 × 1013 g  
  d.   2.7 × 10-11 g  
  2.A 4.628-g sample of an iron oxide was found to contain 3.348 g of iron and 1.280 g of oxygen. What is the simplest formula for this compound?  
  a.   FeO2  
  b.   Fe2O3  
  c.   Fe3O4  
  d.   FeO  
  3.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   58.5 g  
  b.   29.2 g  
  c.   31.7 g  
  d.   40.3 g  
  4.What is the SI base unit used to measure the amount of a substance?  
  a.   mole  
  b.   kilogram  
  c.   meter  
  d.   kelvin  
  5.An empirical formula mass is found to be 17 g/mol. The molar mass is found to be 34 g/mol. What is the number of empirical formula units in this molar mass?  
  a.   0.5 unit  
  b.   17 units  
  c.   1 unit  
  d.   2 units  
  6.What is the molar mass of H2CrO4?  
  a.   2 g  
  b.   118 g  
  c.   64 g  
  d.   52 g  
  7.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
  a.   Avogadro’s number  
  b.   empirical formula  
  c.   percent composition  
  d.   mole ratio  
  8.How is one gram defined?  
  a.   one mole of amu  
  b.   one mole of protons  
  c.   0.1 mole of amu  
  d.   10 moles of amu  
  9.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
  a.   1.0 mol  
  b.   4.0 mol  
  c.   0.5 mol  
  d.   2.0 mol  
  10.What is the percent composition of carbon dioxide CO(2)?  
  a.   33% C and 66% O  
  b.   27% C and 73% O  
  c.   73% C and 27% O  
  d.   50% C and 50% O  
  11.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.4 kg  
  b.   0.5 kg  
  c.   0.05 kg  
  d.   0.2 kg  
  12.A compound contains sulfur, oxygen, and chlorine. Analysis of a sample showed that it contained by mass 26.95% sulfur and 59.61% chlorine. What is the simplest formula for this compound?  
  a.   SOCl2.  
  b.   SOCl  
  c.   SO2Cl  
  d.   SO2Cl2.  
  13.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   aqueous  
  b.   an anhydrate  
  c.   a hydrate  
  d.   waterlogged  
  14.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   3.24 × 1023 atoms  
  b.   5.54 × 1020 atoms  
  c.   3.92 × 1019 atoms  
  d.   1.05 × 1018 atoms  
  15.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   mono-  
  c.   di-  
  16.How many moles of C3H8 are present in 451 g C3H8?  
  a.   10.2 mol  
  b.   1.44 mol  
  c.   3.84 mol  
  d.   0.879 mol  
  17.How can the actual molecular formula be determined?  
  a.   from the molar mass multiplied by the mass of the empirical formula  
  b.   from the molar mass divided by the mass of the empirical formula  
  c.   from the molar mass alone  
  d.   from the empirical formula alone  
  18.A sample of a compound is found to contain 0.404 grams of Fe and 0.174 grams of O. What is the empirical formula for this compound?  
  a.   Fe2O3  
  b.   FeO2  
  c.   Fe3O4  
  d.   FeO  
  19.Analysis of a covalent compound showed that it contained 14.4% hydrogen and 85.6% carbon by mass. What is the empirical formula for this compound?  
  a.   CH  
  b.   CH2  
  c.   C2 H3  
  d.   CH2  
  20.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   6.0 mol  
  b.   8.0 mol  
  c.   3.0 mol  
  d.   2.0 mol  

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