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Chapter 11: The Mole

Practice Test
  1.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.   1 unit  
  b.   0.5 unit  
  c.   2 units  
  d.   17 units  
  2.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.20 × 1024  
  b.   34  
  c.   6.02 × 1023  
  d.   1.77 × 1022  
  3.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   2.7 × 10-11 g  
  b.   5.3 × 10-11 g  
  c.   1.9 × 1013 g  
  d.   6.0 × 1011 g  
  4.How many moles of atoms are present in one mole of water?  
  a.   3 mol  
  b.   1 mol  
  c.   6 mol  
  d.   2 mol  
  5.How many moles of C3H8 are present in 451 g C3H8?  
  a.   1.44 mol  
  b.   10.2 mol  
  c.   3.84 mol  
  d.   0.879 mol  
  6.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.   FeO2  
  b.   FeO  
  c.   Fe3O4  
  d.   Fe2O3  
  7.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   3.0 mol  
  b.   6.0 mol  
  c.   2.0 mol  
  d.   8.0 mol  
  8.What is the mass of one mole of carbon-12 atoms?  
  a.   12 grams  
  b.   12 amu  
  c.   6 amu  
  d.   6 grams  
  9.How is one gram defined?  
  a.   one mole of protons  
  b.   10 moles of amu  
  c.   one mole of amu  
  d.   0.1 mole of amu  
  10.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   di-  
  c.   mono-  
  11.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.   FeO  
  b.   FeO2  
  c.   Fe2O3  
  d.   Fe3O4  
  12.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   31.7 g  
  b.   40.3 g  
  c.   29.2 g  
  d.   58.5 g  
  13.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   a hydrate  
  b.   an anhydrate  
  c.   waterlogged  
  d.   aqueous  
  14.How many particles are present in one mole of particles?  
  a.   3.0 × 108  
  b.   12  
  c.   1  
  d.   6.02 × 1023  
  15.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
  a.   percent composition  
  b.   Avogadro’s number  
  c.   mole ratio  
  d.   empirical formula  
  16.What is the percent composition of carbon dioxide CO(2)?  
  a.   27% C and 73% O  
  b.   50% C and 50% O  
  c.   33% C and 66% O  
  d.   73% C and 27% O  
  17.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.   CH2  
  b.   C2 H3  
  c.   CH2  
  d.   CH  
  18.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.5 kg  
  b.   0.2 kg  
  c.   0.05 kg  
  d.   0.4 kg  
  19.How can the actual molecular formula be determined?  
  a.   from the molar mass divided by the mass of the empirical formula  
  b.   from the molar mass alone  
  c.   from the molar mass multiplied by the mass of the empirical formula  
  d.   from the empirical formula alone  
  20.What is the molar mass of H2CrO4?  
  a.   52 g  
  b.   2 g  
  c.   118 g  
  d.   64 g  

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