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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.   12  
  c.   1  
  d.   6.02 × 1023  
  Hint    
      
  2.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.   SOCl2.  
  d.   SO2Cl2.  
  Hint    
      
  3.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   a hydrate  
  b.   waterlogged  
  c.   aqueous  
  d.   an anhydrate  
  Hint    
      
  4.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   6.02 × 1023  
  b.   34  
  c.   1.77 × 1022  
  d.   1.20 × 1024  
  Hint    
      
  5.How is one gram defined?  
  a.   10 moles of amu  
  b.   one mole of amu  
  c.   0.1 mole of amu  
  d.   one mole of protons  
  Hint    
      
  6.How many moles of C3H8 are present in 451 g C3H8?  
  a.   1.44 mol  
  b.   10.2 mol  
  c.   3.84 mol  
  d.   0.879 mol  
  Hint    
      
  7.What is the molar mass of H2CrO4?  
  a.   52 g  
  b.   64 g  
  c.   2 g  
  d.   118 g  
  Hint    
      
  8.What is the mass of 5.0 × 1021 molecules of water?  
  a.   0.15 g  
  b.   6.02 x 1023 g  
  c.   5.0 g  
  d.   8.3 x 10-3 g  
  Hint    
      
  9.How many moles of atoms are present in one mole of water?  
  a.   1 mol  
  b.   3 mol  
  c.   2 mol  
  d.   6 mol  
  Hint    
      
  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.   Fe3O4  
  b.   FeO2  
  c.   FeO  
  d.   Fe2O3  
  Hint    
      
  11.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
 
  a.   2.0 mol  
  b.   4.0 mol  
  c.   1.0 mol  
  d.   0.5 mol  
  Hint    
      
  12.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    
      
  13.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   2.7 × 10-11 g  
  b.   6.0 × 1011 g  
  c.   5.3 × 10-11 g  
  d.   1.9 × 1013 g  
  Hint    
      
  14.How can the actual molecular formula be determined?  
  a.   from the molar mass multiplied by the mass of the empirical formula  
  b.   from the empirical formula alone  
  c.   from the molar mass alone  
  d.   from the molar mass divided by the mass of the empirical formula  
  Hint    
      
  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.   0.5 unit  
  b.   17 units  
  c.   2 units  
  d.   1 unit  
  Hint    
      
  16.What is the mass of one mole of carbon-12 atoms?  
  a.   12 grams  
  b.   12 amu  
  c.   6 amu  
  d.   6 grams  
  Hint    
      
  17.What is the percent composition of carbon dioxide CO(2)?  
  a.   27% C and 73% O  
  b.   33% C and 66% O  
  c.   50% C and 50% O  
  d.   73% C and 27% O  
  Hint    
      
  18.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   1.05 × 1018 atoms  
  b.   5.54 × 1020 atoms  
  c.   3.24 × 1023 atoms  
  d.   3.92 × 1019 atoms  
  Hint    
      
  19.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   mono-  
  c.   di-  
  Hint    
      
  20.What is the SI base unit used to measure the amount of a substance?  
  a.   kilogram  
  b.   kelvin  
  c.   mole  
  d.   meter  
  Hint    

 
   
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