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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.   Fe2O3  
  b.   Fe3O4  
  c.   FeO2  
  d.   FeO  
  Hint    
      
  2.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
 
  a.   1.0 mol  
  b.   4.0 mol  
  c.   2.0 mol  
  d.   0.5 mol  
  Hint    
      
  3.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   6.02 × 1023  
  b.   1.20 × 1024  
  c.   34  
  d.   1.77 × 1022  
  Hint    
      
  4.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   waterlogged  
  b.   a hydrate  
  c.   an anhydrate  
  d.   aqueous  
  Hint    
      
  5.How many moles of C3H8 are present in 451 g C3H8?  
  a.   3.84 mol  
  b.   1.44 mol  
  c.   0.879 mol  
  d.   10.2 mol  
  Hint    
      
  6.How is one gram defined?  
  a.   0.1 mole of amu  
  b.   10 moles of amu  
  c.   one mole of amu  
  d.   one mole of protons  
  Hint    
      
  7.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   mono-  
  c.   di-  
  Hint    
      
  8.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   58.5 g  
  b.   40.3 g  
  c.   29.2 g  
  d.   31.7 g  
  Hint    
      
  9.What is the SI base unit used to measure the amount of a substance?  
  a.   kelvin  
  b.   mole  
  c.   kilogram  
  d.   meter  
  Hint    
      
  10.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   5.3 × 10-11 g  
  b.   2.7 × 10-11 g  
  c.   1.9 × 1013 g  
  d.   6.0 × 1011 g  
  Hint    
      
  11.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.   FeO  
  b.   Fe2O3  
  c.   Fe3O4  
  d.   FeO2  
  Hint    
      
  12.How many particles are present in one mole of particles?  
  a.   6.02 × 1023  
  b.   3.0 × 108  
  c.   1  
  d.   12  
  Hint    
      
  13.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  
  Hint    
      
  14.What is the molar mass of H2CrO4?  
  a.   2 g  
  b.   118 g  
  c.   64 g  
  d.   52 g  
  Hint    
      
  15.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
 
  a.   Avogadro’s number  
  b.   empirical formula  
  c.   mole ratio  
  d.   percent composition  
  Hint    
      
  16.What is the mass of 5.0 × 1021 molecules of water?  
  a.   0.15 g  
  b.   8.3 x 10-3 g  
  c.   5.0 g  
  d.   6.02 x 1023 g  
  Hint    
      
  17.How many moles of atoms are present in one mole of water?  
  a.   3 mol  
  b.   6 mol  
  c.   2 mol  
  d.   1 mol  
  Hint    
      
  18.How can the actual molecular formula be determined?  
  a.   from the molar mass divided by the mass of the empirical formula  
  b.   from the molar mass multiplied by the mass of the empirical formula  
  c.   from the molar mass alone  
  d.   from the empirical formula alone  
  Hint    
      
  19.What is the mass of one mole of carbon-12 atoms?  
  a.   12 amu  
  b.   6 grams  
  c.   6 amu  
  d.   12 grams  
  Hint    
      
  20.What is the percent composition of carbon dioxide CO(2)?  
  a.   50% C and 50% O  
  b.   73% C and 27% O  
  c.   27% C and 73% O  
  d.   33% C and 66% O  
  Hint    

 
   
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