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Chapter 11: The Mole

Practice Test
  1.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.05 kg  
  b.   0.5 kg  
  c.   0.2 kg  
  d.   0.4 kg  
  2.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  
  3.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  
  4.What is the mass of one mole of carbon-12 atoms?  
  a.   6 grams  
  b.   6 amu  
  c.   12 grams  
  d.   12 amu  
  5.How is one gram defined?  
  a.   one mole of amu  
  b.   10 moles of amu  
  c.   0.1 mole of amu  
  d.   one mole of protons  
  6.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.   2 units  
  c.   0.5 unit  
  d.   17 units  
  7.How many moles of atoms are present in one mole of water?  
  a.   2 mol  
  b.   6 mol  
  c.   1 mol  
  d.   3 mol  
  8.What is the molar mass of H2CrO4?  
  a.   2 g  
  b.   52 g  
  c.   118 g  
  d.   64 g  
  9.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  
  10.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   di-  
  b.   mono-  
  c.   tri-  
  11.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
  a.   1.0 mol  
  b.   0.5 mol  
  c.   4.0 mol  
  d.   2.0 mol  
  12.How can the actual molecular formula be determined?  
  a.   from the molar mass alone  
  b.   from the molar mass divided by the mass of the empirical formula  
  c.   from the molar mass multiplied by the mass of the empirical formula  
  d.   from the empirical formula alone  
  13.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
  a.   mole ratio  
  b.   empirical formula  
  c.   Avogadro’s number  
  d.   percent composition  
  14.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.   FeO  
  c.   FeO2  
  d.   Fe3O4  
  15.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.77 × 1022  
  b.   6.02 × 1023  
  c.   1.20 × 1024  
  d.   34  
  16.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   29.2 g  
  b.   40.3 g  
  c.   31.7 g  
  d.   58.5 g  
  17.What is the percent composition of carbon dioxide CO(2)?  
  a.   27% C and 73% O  
  b.   73% C and 27% O  
  c.   50% C and 50% O  
  d.   33% C and 66% O  
  18.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   3.0 mol  
  b.   8.0 mol  
  c.   6.0 mol  
  d.   2.0 mol  
  19.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   3.92 × 1019 atoms  
  b.   3.24 × 1023 atoms  
  c.   1.05 × 1018 atoms  
  d.   5.54 × 1020 atoms  
  20.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   5.3 × 10-11 g  
  b.   6.0 × 1011 g  
  c.   1.9 × 1013 g  
  d.   2.7 × 10-11 g  

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