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Chapter 11: The Mole

Practice Test
  1.What is the mass of 5.0 × 1021 molecules of water?  
  a.   6.02 x 1023 g  
  b.   8.3 x 10-3 g  
  c.   0.15 g  
  d.   5.0 g  
  2.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   34  
  b.   6.02 × 1023  
  c.   1.77 × 1022  
  d.   1.20 × 1024  
  3.How many moles of atoms are present in one mole of water?  
  a.   6 mol  
  b.   3 mol  
  c.   2 mol  
  d.   1 mol  
  4.What is the molar mass of H2CrO4?  
  a.   52 g  
  b.   2 g  
  c.   64 g  
  d.   118 g  
  5.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 empirical formula alone  
  d.   from the molar mass multiplied by the mass of the empirical formula  
  6.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.   Fe2O3  
  b.   FeO  
  c.   FeO2  
  d.   Fe3O4  
  7.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.   17 units  
  c.   2 units  
  d.   0.5 unit  
  8.What is the percent composition of carbon dioxide CO(2)?  
  a.   27% C and 73% O  
  b.   33% C and 66% O  
  c.   73% C and 27% O  
  d.   50% C and 50% O  
  9.How many particles are present in one mole of particles?  
  a.   1  
  b.   3.0 × 108  
  c.   6.02 × 1023  
  d.   12  
  10.What is the SI base unit used to measure the amount of a substance?  
  a.   meter  
  b.   kelvin  
  c.   mole  
  d.   kilogram  
  11.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   a hydrate  
  b.   aqueous  
  c.   an anhydrate  
  d.   waterlogged  
  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.   SOCl  
  b.   SOCl2.  
  c.   SO2Cl  
  d.   SO2Cl2.  
  13.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   5.3 × 10-11 g  
  b.   1.9 × 1013 g  
  c.   2.7 × 10-11 g  
  d.   6.0 × 1011 g  
  14.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.4 kg  
  b.   0.2 kg  
  c.   0.05 kg  
  d.   0.5 kg  
  15.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.   C2 H3  
  b.   CH2  
  c.   CH  
  d.   CH2  
  16.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   40.3 g  
  b.   58.5 g  
  c.   29.2 g  
  d.   31.7 g  
  17.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   mono-  
  b.   di-  
  c.   tri-  
  18.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
  a.   empirical formula  
  b.   Avogadro’s number  
  c.   percent composition  
  d.   mole ratio  
  19.How many moles of C3H8 are present in 451 g C3H8?  
  a.   10.2 mol  
  b.   3.84 mol  
  c.   0.879 mol  
  d.   1.44 mol  
  20.How is one gram defined?  
  a.   10 moles of amu  
  b.   one mole of amu  
  c.   one mole of protons  
  d.   0.1 mole of amu  

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