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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 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    
      
  2.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
 
  a.   percent composition  
  b.   Avogadro’s number  
  c.   mole ratio  
  d.   empirical formula  
  Hint    
      
  3.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    
      
  4.How is one gram defined?  
  a.   10 moles of amu  
  b.   one mole of amu  
  c.   one mole of protons  
  d.   0.1 mole of amu  
  Hint    
      
  5.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
 
  a.   2.0 mol  
  b.   0.5 mol  
  c.   1.0 mol  
  d.   4.0 mol  
  Hint    
      
  6.What is the molar mass of H2CrO4?  
  a.   118 g  
  b.   52 g  
  c.   64 g  
  d.   2 g  
  Hint    
      
  7.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   di-  
  c.   mono-  
  Hint    
      
  8.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   5.54 × 1020 atoms  
  b.   3.24 × 1023 atoms  
  c.   3.92 × 1019 atoms  
  d.   1.05 × 1018 atoms  
  Hint    
      
  9.What is the mass of 5.0 × 1021 molecules of water?  
  a.   8.3 x 10-3 g  
  b.   6.02 x 1023 g  
  c.   0.15 g  
  d.   5.0 g  
  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.   1 unit  
  d.   2 units  
  Hint    
      
  11.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   8.0 mol  
  b.   6.0 mol  
  c.   3.0 mol  
  d.   2.0 mol  
  Hint    
      
  12.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   6.0 × 1011 g  
  b.   5.3 × 10-11 g  
  c.   2.7 × 10-11 g  
  d.   1.9 × 1013 g  
  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.   CH  
  b.   CH2  
  c.   C2 H3  
  d.   CH2  
  Hint    
      
  14.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.   Fe2O3  
  b.   FeO2  
  c.   FeO  
  d.   Fe3O4  
  Hint    
      
  15.How many moles of atoms are present in one mole of water?  
  a.   1 mol  
  b.   6 mol  
  c.   2 mol  
  d.   3 mol  
  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.   Fe3O4  
  b.   Fe2O3  
  c.   FeO  
  d.   FeO2  
  Hint    
      
  17.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.2 kg  
  b.   0.5 kg  
  c.   0.4 kg  
  d.   0.05 kg  
  Hint    
      
  18.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   an anhydrate  
  b.   a hydrate  
  c.   waterlogged  
  d.   aqueous  
  Hint    
      
  19.What is the mass of one mole of carbon-12 atoms?  
  a.   12 amu  
  b.   6 grams  
  c.   12 grams  
  d.   6 amu  
  Hint    
      
  20.How many particles are present in one mole of particles?  
  a.   12  
  b.   1  
  c.   6.02 × 1023  
  d.   3.0 × 108  
  Hint    

 
   
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