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Chapter 11: The Mole

Practice Test
      
  1.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   1.9 × 1013 g  
  b.   5.3 × 10-11 g  
  c.   2.7 × 10-11 g  
  d.   6.0 × 1011 g  
  Hint    
      
  2.What is the mass of one mole of carbon-12 atoms?  
  a.   6 amu  
  b.   12 grams  
  c.   6 grams  
  d.   12 amu  
  Hint    
      
  3.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  
  Hint    
      
  4.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.2 kg  
  b.   0.4 kg  
  c.   0.05 kg  
  d.   0.5 kg  
  Hint    
      
  5.What is the percent composition of carbon dioxide CO(2)?  
  a.   73% C and 27% O  
  b.   50% C and 50% O  
  c.   27% C and 73% O  
  d.   33% C and 66% O  
  Hint    
      
  6.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.   Fe3O4  
  b.   FeO  
  c.   Fe2O3  
  d.   FeO2  
  Hint    
      
  7.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
 
  a.   0.5 mol  
  b.   1.0 mol  
  c.   4.0 mol  
  d.   2.0 mol  
  Hint    
      
  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.   SO2Cl2.  
  b.   SOCl  
  c.   SOCl2.  
  d.   SO2Cl  
  Hint    
      
  9.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   di-  
  b.   tri-  
  c.   mono-  
  Hint    
      
  10.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   2.0 mol  
  b.   6.0 mol  
  c.   3.0 mol  
  d.   8.0 mol  
  Hint    
      
  11.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.   2 units  
  b.   1 unit  
  c.   0.5 unit  
  d.   17 units  
  Hint    
      
  12.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
 
  a.   percent composition  
  b.   mole ratio  
  c.   Avogadro’s number  
  d.   empirical formula  
  Hint    
      
  13.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.   C2 H3  
  b.   CH  
  c.   CH2  
  d.   CH2  
  Hint    
      
  14.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   1.05 × 1018 atoms  
  b.   3.92 × 1019 atoms  
  c.   3.24 × 1023 atoms  
  d.   5.54 × 1020 atoms  
  Hint    
      
  15.How many moles of atoms are present in one mole of water?  
  a.   6 mol  
  b.   1 mol  
  c.   2 mol  
  d.   3 mol  
  Hint    
      
  16.How can the actual molecular formula be determined?  
  a.   from the molar mass multiplied by the mass of the empirical formula  
  b.   from the molar mass alone  
  c.   from the molar mass divided by the mass of the empirical formula  
  d.   from the empirical formula alone  
  Hint    
      
  17.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   29.2 g  
  b.   58.5 g  
  c.   40.3 g  
  d.   31.7 g  
  Hint    
      
  18.What is the molar mass of H2CrO4?  
  a.   2 g  
  b.   52 g  
  c.   118 g  
  d.   64 g  
  Hint    
      
  19.How many particles are present in one mole of particles?  
  a.   6.02 × 1023  
  b.   12  
  c.   1  
  d.   3.0 × 108  
  Hint    
      
  20.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.20 × 1024  
  b.   6.02 × 1023  
  c.   1.77 × 1022  
  d.   34  
  Hint    

 
   
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