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Chapter 11: The Mole

Practice Test
  1.How many particles are present in one mole of particles?  
  a.   6.02 × 1023  
  b.   3.0 × 108  
  c.   1  
  d.   12  
  2.How many moles of atoms are present in one mole of water?  
  a.   2 mol  
  b.   1 mol  
  c.   6 mol  
  d.   3 mol  
  3.What is the molar mass of H2CrO4?  
  a.   64 g  
  b.   52 g  
  c.   2 g  
  d.   118 g  
  4.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   34  
  b.   6.02 × 1023  
  c.   1.20 × 1024  
  d.   1.77 × 1022  
  5.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   1.05 × 1018 atoms  
  b.   5.54 × 1020 atoms  
  c.   3.24 × 1023 atoms  
  d.   3.92 × 1019 atoms  
  6.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   58.5 g  
  b.   31.7 g  
  c.   40.3 g  
  d.   29.2 g  
  7.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.   empirical formula  
  d.   mole ratio  
  8.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.   17 units  
  b.   2 units  
  c.   0.5 unit  
  d.   1 unit  
  9.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.   SO2Cl2.  
  c.   SOCl2.  
  d.   SO2Cl  
  10.How many moles of C3H8 are present in 451 g C3H8?  
  a.   0.879 mol  
  b.   3.84 mol  
  c.   1.44 mol  
  d.   10.2 mol  
  11.What is the SI base unit used to measure the amount of a substance?  
  a.   kilogram  
  b.   kelvin  
  c.   mole  
  d.   meter  
  12.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   aqueous  
  b.   a hydrate  
  c.   an anhydrate  
  d.   waterlogged  
  13.What is the mass of one mole of carbon-12 atoms?  
  a.   12 amu  
  b.   12 grams  
  c.   6 amu  
  d.   6 grams  
  14.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   5.3 × 10-11 g  
  b.   2.7 × 10-11 g  
  c.   6.0 × 1011 g  
  d.   1.9 × 1013 g  
  15.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.   Fe3O4  
  b.   FeO  
  c.   FeO2  
  d.   Fe2O3  
  16.How is one gram defined?  
  a.   one mole of protons  
  b.   one mole of amu  
  c.   0.1 mole of amu  
  d.   10 moles of amu  
  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 alone  
  c.   from the empirical formula alone  
  d.   from the molar mass divided by the mass of the empirical formula  
  18.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  
  19.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.   Fe2O3  
  c.   FeO  
  d.   Fe3O4  
  20.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.   CH  
  d.   CH2  

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