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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.   6.02 × 1023  
  b.   1.20 × 1024  
  c.   1.77 × 1022  
  d.   34  
  Hint    
      
  2.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
 
  a.   4.0 mol  
  b.   2.0 mol  
  c.   1.0 mol  
  d.   0.5 mol  
  Hint    
      
  3.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.   Fe2O3  
  c.   FeO  
  d.   FeO2  
  Hint    
      
  4.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.   CH  
  b.   CH2  
  c.   C2 H3  
  d.   CH2  
  Hint    
      
  5.How can the actual molecular formula be determined?  
  a.   from the molar mass alone  
  b.   from the molar mass multiplied by the mass of the empirical formula  
  c.   from the empirical formula alone  
  d.   from the molar mass divided by the mass of the empirical formula  
  Hint    
      
  6.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   mono-  
  b.   di-  
  c.   tri-  
  Hint    
      
  7.What is the mass of 5.0 × 1021 molecules of water?  
  a.   6.02 x 1023 g  
  b.   8.3 x 10-3 g  
  c.   5.0 g  
  d.   0.15 g  
  Hint    
      
  8.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    
      
  9.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    
      
  10.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.   17 units  
  b.   0.5 unit  
  c.   2 units  
  d.   1 unit  
  Hint    
      
  11.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.5 kg  
  b.   0.4 kg  
  c.   0.2 kg  
  d.   0.05 kg  
  Hint    
      
  12.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   6.0 mol  
  b.   2.0 mol  
  c.   3.0 mol  
  d.   8.0 mol  
  Hint    
      
  13.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   aqueous  
  b.   waterlogged  
  c.   a hydrate  
  d.   an anhydrate  
  Hint    
      
  14.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.   SOCl2.  
  c.   SOCl  
  d.   SO2Cl  
  Hint    
      
  15.How is one gram defined?  
  a.   one mole of protons  
  b.   one mole of amu  
  c.   10 moles of amu  
  d.   0.1 mole of amu  
  Hint    
      
  16.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.   FeO2  
  c.   Fe3O4  
  d.   FeO  
  Hint    
      
  17.What is the mass of one mole of carbon-12 atoms?  
  a.   12 amu  
  b.   6 amu  
  c.   6 grams  
  d.   12 grams  
  Hint    
      
  18.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   29.2 g  
  b.   40.3 g  
  c.   58.5 g  
  d.   31.7 g  
  Hint    
      
  19.How many moles of C3H8 are present in 451 g C3H8?  
  a.   1.44 mol  
  b.   0.879 mol  
  c.   3.84 mol  
  d.   10.2 mol  
  Hint    
      
  20.What is the molar mass of H2CrO4?  
  a.   52 g  
  b.   2 g  
  c.   64 g  
  d.   118 g  
  Hint    

 
   
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