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Chapter 11: The Mole

Practice Test
      
  1.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
 
  a.   4.0 mol  
  b.   2.0 mol  
  c.   0.5 mol  
  d.   1.0 mol  
  Hint    
      
  2.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   5.3 × 10-11 g  
  b.   6.0 × 1011 g  
  c.   2.7 × 10-11 g  
  d.   1.9 × 1013 g  
  Hint    
      
  3.What is the mass of 5.0 × 1021 molecules of water?  
  a.   8.3 x 10-3 g  
  b.   5.0 g  
  c.   6.02 x 1023 g  
  d.   0.15 g  
  Hint    
      
  4.How many moles of C3H8 are present in 451 g C3H8?  
  a.   3.84 mol  
  b.   0.879 mol  
  c.   1.44 mol  
  d.   10.2 mol  
  Hint    
      
  5.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    
      
  6.How many moles of atoms are present in one mole of water?  
  a.   2 mol  
  b.   6 mol  
  c.   1 mol  
  d.   3 mol  
  Hint    
      
  7.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   2.0 mol  
  b.   8.0 mol  
  c.   6.0 mol  
  d.   3.0 mol  
  Hint    
      
  8.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    
      
  9.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.   Fe3O4  
  c.   Fe2O3  
  d.   FeO2  
  Hint    
      
  10.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.   SOCl  
  b.   SOCl2.  
  c.   SO2Cl2.  
  d.   SO2Cl  
  Hint    
      
  11.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.   CH2  
  b.   CH  
  c.   C2 H3  
  d.   CH2  
  Hint    
      
  12.How many particles are present in one mole of particles?  
  a.   3.0 × 108  
  b.   12  
  c.   6.02 × 1023  
  d.   1  
  Hint    
      
  13.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    
      
  14.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   58.5 g  
  b.   29.2 g  
  c.   31.7 g  
  d.   40.3 g  
  Hint    
      
  15.How is one gram defined?  
  a.   10 moles of amu  
  b.   one mole of protons  
  c.   0.1 mole of amu  
  d.   one mole of amu  
  Hint    
      
  16.What is the percent composition of carbon dioxide CO(2)?  
  a.   73% C and 27% O  
  b.   27% C and 73% O  
  c.   50% C and 50% O  
  d.   33% C and 66% O  
  Hint    
      
  17.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    
      
  18.What is the SI base unit used to measure the amount of a substance?  
  a.   kelvin  
  b.   kilogram  
  c.   mole  
  d.   meter  
  Hint    
      
  19.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   di-  
  c.   mono-  
  Hint    
      
  20.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    

 
   
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