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Chapter 11: The Mole

Practice Test
      
  1.How can the actual molecular formula be determined?  
  a.   from the molar mass alone  
  b.   from the molar mass divided by the mass of the empirical formula  
  c.   from the empirical formula alone  
  d.   from the molar mass multiplied by the mass of the empirical formula  
  Hint    
      
  2.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   6.02 × 1023  
  b.   1.20 × 1024  
  c.   1.77 × 1022  
  d.   34  
  Hint    
      
  3.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   di-  
  b.   mono-  
  c.   tri-  
  Hint    
      
  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.   SOCl2.  
  b.   SO2Cl2.  
  c.   SO2Cl  
  d.   SOCl  
  Hint    
      
  5.What is the mass of one mole of carbon-12 atoms?  
  a.   12 grams  
  b.   6 amu  
  c.   12 amu  
  d.   6 grams  
  Hint    
      
  6.How many particles are present in one mole of particles?  
  a.   12  
  b.   6.02 × 1023  
  c.   3.0 × 108  
  d.   1  
  Hint    
      
  7.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
 
  a.   1.0 mol  
  b.   2.0 mol  
  c.   0.5 mol  
  d.   4.0 mol  
  Hint    
      
  8.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    
      
  9.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    
      
  10.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    
      
  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.   FeO2  
  c.   Fe3O4  
  d.   Fe2O3  
  Hint    
      
  12.What is the molar mass of H2CrO4?  
  a.   52 g  
  b.   2 g  
  c.   64 g  
  d.   118 g  
  Hint    
      
  13.How many moles of C3H8 are present in 451 g C3H8?  
  a.   1.44 mol  
  b.   0.879 mol  
  c.   10.2 mol  
  d.   3.84 mol  
  Hint    
      
  14.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   1.9 × 1013 g  
  b.   5.3 × 10-11 g  
  c.   6.0 × 1011 g  
  d.   2.7 × 10-11 g  
  Hint    
      
  15.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   1.05 × 1018 atoms  
  b.   3.24 × 1023 atoms  
  c.   5.54 × 1020 atoms  
  d.   3.92 × 1019 atoms  
  Hint    
      
  16.How many moles of atoms are present in one mole of water?  
  a.   2 mol  
  b.   1 mol  
  c.   6 mol  
  d.   3 mol  
  Hint    
      
  17.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.   17 units  
  c.   2 units  
  d.   1 unit  
  Hint    
      
  18.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   31.7 g  
  b.   58.5 g  
  c.   29.2 g  
  d.   40.3 g  
  Hint    
      
  19.What is the percent composition of carbon dioxide CO(2)?  
  a.   27% C and 73% O  
  b.   50% C and 50% O  
  c.   33% C and 66% O  
  d.   73% C and 27% O  
  Hint    
      
  20.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   a hydrate  
  b.   an anhydrate  
  c.   waterlogged  
  d.   aqueous  
  Hint    

 
   
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