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Chapter 11: The Mole

Practice Test
      
  1.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
 
  a.   percent composition  
  b.   empirical formula  
  c.   mole ratio  
  d.   Avogadro’s number  
  Hint    
      
  2.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.   1 unit  
  b.   2 units  
  c.   17 units  
  d.   0.5 unit  
  Hint    
      
  3.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   5.54 × 1020 atoms  
  b.   1.05 × 1018 atoms  
  c.   3.92 × 1019 atoms  
  d.   3.24 × 1023 atoms  
  Hint    
      
  4.What is the molar mass of H2CrO4?  
  a.   64 g  
  b.   2 g  
  c.   52 g  
  d.   118 g  
  Hint    
      
  5.How many moles of C3H8 are present in 451 g C3H8?  
  a.   3.84 mol  
  b.   10.2 mol  
  c.   0.879 mol  
  d.   1.44 mol  
  Hint    
      
  6.How is one gram defined?  
  a.   0.1 mole of amu  
  b.   one mole of amu  
  c.   one mole of protons  
  d.   10 moles of amu  
  Hint    
      
  7.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.77 × 1022  
  b.   6.02 × 1023  
  c.   1.20 × 1024  
  d.   34  
  Hint    
      
  8.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
 
  a.   2.0 mol  
  b.   1.0 mol  
  c.   4.0 mol  
  d.   0.5 mol  
  Hint    
      
  9.What is the mass of 5.0 × 1021 molecules of water?  
  a.   0.15 g  
  b.   8.3 x 10-3 g  
  c.   6.02 x 1023 g  
  d.   5.0 g  
  Hint    
      
  10.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   29.2 g  
  b.   58.5 g  
  c.   31.7 g  
  d.   40.3 g  
  Hint    
      
  11.What is the percent composition of carbon dioxide CO(2)?  
  a.   73% C and 27% O  
  b.   27% C and 73% O  
  c.   33% C and 66% O  
  d.   50% C and 50% O  
  Hint    
      
  12.How many moles of atoms are present in one mole of water?  
  a.   2 mol  
  b.   3 mol  
  c.   6 mol  
  d.   1 mol  
  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.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.2 kg  
  b.   0.05 kg  
  c.   0.5 kg  
  d.   0.4 kg  
  Hint    
      
  15.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   3.0 mol  
  b.   6.0 mol  
  c.   2.0 mol  
  d.   8.0 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.   FeO  
  b.   Fe2O3  
  c.   Fe3O4  
  d.   FeO2  
  Hint    
      
  17.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.   SOCl2.  
  c.   SOCl  
  d.   SO2Cl2.  
  Hint    
      
  18.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   mono-  
  c.   di-  
  Hint    
      
  19.How many particles are present in one mole of particles?  
  a.   3.0 × 108  
  b.   12  
  c.   1  
  d.   6.02 × 1023  
  Hint    
      
  20.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    

 
   
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