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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.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   mono-  
  b.   tri-  
  c.   di-  
  Hint    
      
  3.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.20 × 1024  
  b.   34  
  c.   1.77 × 1022  
  d.   6.02 × 1023  
  Hint    
      
  4.What is the percent composition of carbon dioxide CO(2)?  
  a.   50% C and 50% O  
  b.   33% C and 66% O  
  c.   73% C and 27% O  
  d.   27% C and 73% O  
  Hint    
      
  5.What is the SI base unit used to measure the amount of a substance?  
  a.   kelvin  
  b.   mole  
  c.   meter  
  d.   kilogram  
  Hint    
      
  6.What is the mass of 5.0 × 1021 molecules of water?  
  a.   5.0 g  
  b.   6.02 x 1023 g  
  c.   8.3 x 10-3 g  
  d.   0.15 g  
  Hint    
      
  7.How many particles are present in one mole of particles?  
  a.   6.02 × 1023  
  b.   3.0 × 108  
  c.   12  
  d.   1  
  Hint    
      
  8.What is the molar mass of H2CrO4?  
  a.   118 g  
  b.   64 g  
  c.   2 g  
  d.   52 g  
  Hint    
      
  9.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.   0.5 unit  
  c.   17 units  
  d.   1 unit  
  Hint    
      
  10.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   2.7 × 10-11 g  
  b.   6.0 × 1011 g  
  c.   5.3 × 10-11 g  
  d.   1.9 × 1013 g  
  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.   C2 H3  
  c.   CH  
  d.   CH2  
  Hint    
      
  12.How many moles of atoms are present in one mole of water?  
  a.   3 mol  
  b.   1 mol  
  c.   2 mol  
  d.   6 mol  
  Hint    
      
  13.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.   SO2Cl2.  
  c.   SO2Cl  
  d.   SOCl2.  
  Hint    
      
  14.How is one gram defined?  
  a.   one mole of amu  
  b.   10 moles of amu  
  c.   0.1 mole of amu  
  d.   one mole of protons  
  Hint    
      
  15.How can the actual molecular formula be determined?  
  a.   from the molar mass divided by the mass of the empirical formula  
  b.   from the empirical formula alone  
  c.   from the molar mass multiplied by the mass of the empirical formula  
  d.   from the molar mass alone  
  Hint    
      
  16.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    
      
  17.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   an anhydrate  
  b.   waterlogged  
  c.   aqueous  
  d.   a hydrate  
  Hint    
      
  18.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   8.0 mol  
  b.   2.0 mol  
  c.   3.0 mol  
  d.   6.0 mol  
  Hint    
      
  19.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.05 kg  
  b.   0.2 kg  
  c.   0.4 kg  
  d.   0.5 kg  
  Hint    
      
  20.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.   FeO2  
  c.   Fe2O3  
  d.   FeO  
  Hint    

 
   
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