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Chapter 11: The Mole

Practice Test
  1.How many particles are present in one mole of particles?  
  a.   3.0 × 108  
  b.   6.02 × 1023  
  c.   12  
  d.   1  
  2.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   8.0 mol  
  b.   2.0 mol  
  c.   6.0 mol  
  d.   3.0 mol  
  3.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   aqueous  
  b.   waterlogged  
  c.   an anhydrate  
  d.   a hydrate  
  4.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.   SO2Cl  
  d.   SOCl2.  
  5.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
  a.   mole ratio  
  b.   Avogadro’s number  
  c.   percent composition  
  d.   empirical formula  
  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.   0.5 unit  
  b.   1 unit  
  c.   2 units  
  d.   17 units  
  7.What is the mass of 5.0 × 1021 molecules of water?  
  a.   5.0 g  
  b.   8.3 x 10-3 g  
  c.   0.15 g  
  d.   6.02 x 1023 g  
  8.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   40.3 g  
  b.   29.2 g  
  c.   58.5 g  
  d.   31.7 g  
  9.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.   Fe3O4  
  c.   FeO  
  d.   FeO2  
  10.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  
  11.How many moles of atoms are present in one mole of water?  
  a.   2 mol  
  b.   6 mol  
  c.   3 mol  
  d.   1 mol  
  12.How many moles of C3H8 are present in 451 g C3H8?  
  a.   3.84 mol  
  b.   1.44 mol  
  c.   10.2 mol  
  d.   0.879 mol  
  13.What is the molar mass of H2CrO4?  
  a.   2 g  
  b.   52 g  
  c.   64 g  
  d.   118 g  
  14.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.   CH2  
  c.   CH  
  d.   C2 H3  
  15.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   mono-  
  c.   di-  
  16.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   5.54 × 1020 atoms  
  b.   1.05 × 1018 atoms  
  c.   3.24 × 1023 atoms  
  d.   3.92 × 1019 atoms  
  17.How can the actual molecular formula be determined?  
  a.   from the molar mass divided by the mass of the empirical formula  
  b.   from the empirical formula alone  
  c.   from the molar mass multiplied by the mass of the empirical formula  
  d.   from the molar mass alone  
  18.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.77 × 1022  
  b.   1.20 × 1024  
  c.   6.02 × 1023  
  d.   34  
  19.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  
  20.What is the percent composition of carbon dioxide CO(2)?  
  a.   33% C and 66% O  
  b.   73% C and 27% O  
  c.   27% C and 73% O  
  d.   50% C and 50% O  

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