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Chapter 11: The Mole

Practice Test
      
  1.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.77 × 1022  
  b.   34  
  c.   1.20 × 1024  
  d.   6.02 × 1023  
  Hint    
      
  2.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   58.5 g  
  b.   29.2 g  
  c.   40.3 g  
  d.   31.7 g  
  Hint    
      
  3.What is the mass of 5.0 × 1021 molecules of water?  
  a.   5.0 g  
  b.   0.15 g  
  c.   8.3 x 10-3 g  
  d.   6.02 x 1023 g  
  Hint    
      
  4.How many moles of atoms are present in one mole of water?  
  a.   6 mol  
  b.   3 mol  
  c.   2 mol  
  d.   1 mol  
  Hint    
      
  5.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
 
  a.   empirical formula  
  b.   percent composition  
  c.   mole ratio  
  d.   Avogadro’s number  
  Hint    
      
  6.What is the SI base unit used to measure the amount of a substance?  
  a.   meter  
  b.   kilogram  
  c.   kelvin  
  d.   mole  
  Hint    
      
  7.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.   FeO2  
  b.   FeO  
  c.   Fe2O3  
  d.   Fe3O4  
  Hint    
      
  8.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   3.24 × 1023 atoms  
  b.   1.05 × 1018 atoms  
  c.   5.54 × 1020 atoms  
  d.   3.92 × 1019 atoms  
  Hint    
      
  9.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.05 kg  
  b.   0.2 kg  
  c.   0.4 kg  
  d.   0.5 kg  
  Hint    
      
  10.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  
  Hint    
      
  11.How is one gram defined?  
  a.   one mole of amu  
  b.   one mole of protons  
  c.   0.1 mole of amu  
  d.   10 moles of amu  
  Hint    
      
  12.What is the molar mass of H2CrO4?  
  a.   64 g  
  b.   118 g  
  c.   52 g  
  d.   2 g  
  Hint    
      
  13.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   6.0 × 1011 g  
  b.   5.3 × 10-11 g  
  c.   1.9 × 1013 g  
  d.   2.7 × 10-11 g  
  Hint    
      
  14.What is the percent composition of carbon dioxide CO(2)?  
  a.   33% C and 66% O  
  b.   27% C and 73% O  
  c.   50% C and 50% O  
  d.   73% C and 27% O  
  Hint    
      
  15.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
 
  a.   2.0 mol  
  b.   4.0 mol  
  c.   0.5 mol  
  d.   1.0 mol  
  Hint    
      
  16.What is the mass of one mole of carbon-12 atoms?  
  a.   12 grams  
  b.   12 amu  
  c.   6 grams  
  d.   6 amu  
  Hint    
      
  17.How can the actual molecular formula be determined?  
  a.   from the empirical formula alone  
  b.   from the molar mass divided by the mass of the empirical formula  
  c.   from the molar mass multiplied by the mass of the empirical formula  
  d.   from the molar mass alone  
  Hint    
      
  18.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.   FeO2  
  c.   Fe2O3  
  d.   Fe3O4  
  Hint    
      
  19.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   mono-  
  b.   tri-  
  c.   di-  
  Hint    
      
  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.   CH2  
  c.   C2 H3  
  d.   CH  
  Hint    

 
   
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