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Chapter 11: The Mole

Practice Test
  1.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.   Fe3O4  
  c.   FeO2  
  d.   Fe2O3  
  2.How many particles are present in one mole of particles?  
  a.   12  
  b.   1  
  c.   3.0 × 108  
  d.   6.02 × 1023  
  3.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   mono-  
  c.   di-  
  4.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   31.7 g  
  b.   29.2 g  
  c.   40.3 g  
  d.   58.5 g  
  5.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
  a.   empirical formula  
  b.   mole ratio  
  c.   percent composition  
  d.   Avogadro’s number  
  6.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   waterlogged  
  b.   aqueous  
  c.   a hydrate  
  d.   an anhydrate  
  7.How can the actual molecular formula be determined?  
  a.   from the empirical formula alone  
  b.   from the molar mass multiplied by the mass of the empirical formula  
  c.   from the molar mass alone  
  d.   from the molar mass divided by the mass of the empirical formula  
  8.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.   SO2Cl  
  b.   SOCl  
  c.   SO2Cl2.  
  d.   SOCl2.  
  9.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  
  10.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   3.24 × 1023 atoms  
  b.   3.92 × 1019 atoms  
  c.   1.05 × 1018 atoms  
  d.   5.54 × 1020 atoms  
  11.What is the SI base unit used to measure the amount of a substance?  
  a.   kelvin  
  b.   kilogram  
  c.   meter  
  d.   mole  
  12.How is one gram defined?  
  a.   10 moles of amu  
  b.   0.1 mole of amu  
  c.   one mole of protons  
  d.   one mole of amu  
  13.How many moles of atoms are present in one mole of water?  
  a.   2 mol  
  b.   6 mol  
  c.   3 mol  
  d.   1 mol  
  14.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   34  
  b.   1.20 × 1024  
  c.   6.02 × 1023  
  d.   1.77 × 1022  
  15.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  
  16.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   5.3 × 10-11 g  
  b.   1.9 × 1013 g  
  c.   6.0 × 1011 g  
  d.   2.7 × 10-11 g  
  17.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.   8.0 mol  
  d.   2.0 mol  
  18.What is the mass of 5.0 × 1021 molecules of water?  
  a.   6.02 x 1023 g  
  b.   0.15 g  
  c.   5.0 g  
  d.   8.3 x 10-3 g  
  19.What is the percent composition of carbon dioxide CO(2)?  
  a.   73% C and 27% O  
  b.   33% C and 66% O  
  c.   27% C and 73% O  
  d.   50% C and 50% O  
  20.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.   FeO2  
  c.   FeO  
  d.   Fe3O4  

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