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Chapter 11: The Mole

Practice Test
      
  1.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    
      
  2.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   1.05 × 1018 atoms  
  b.   3.24 × 1023 atoms  
  c.   5.54 × 1020 atoms  
  d.   3.92 × 1019 atoms  
  Hint    
      
  3.What is the molar mass of H2CrO4?  
  a.   118 g  
  b.   64 g  
  c.   52 g  
  d.   2 g  
  Hint    
      
  4.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.20 × 1024  
  b.   34  
  c.   6.02 × 1023  
  d.   1.77 × 1022  
  Hint    
      
  5.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   di-  
  b.   tri-  
  c.   mono-  
  Hint    
      
  6.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
 
  a.   Avogadro’s number  
  b.   percent composition  
  c.   mole ratio  
  d.   empirical formula  
  Hint    
      
  7.How can the actual molecular formula be determined?  
  a.   from the molar mass alone  
  b.   from the empirical formula alone  
  c.   from the molar mass divided by the mass of the empirical formula  
  d.   from the molar mass multiplied by the mass of the empirical formula  
  Hint    
      
  8.How many moles of atoms are present in one mole of water?  
  a.   6 mol  
  b.   1 mol  
  c.   3 mol  
  d.   2 mol  
  Hint    
      
  9.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    
      
  10.What is the percent composition of carbon dioxide CO(2)?  
  a.   27% C and 73% O  
  b.   50% C and 50% O  
  c.   73% C and 27% O  
  d.   33% C and 66% O  
  Hint    
      
  11.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.   FeO2  
  b.   Fe3O4  
  c.   FeO  
  d.   Fe2O3  
  Hint    
      
  12.What is the mass of 5.0 × 1021 molecules of water?  
  a.   0.15 g  
  b.   8.3 x 10-3 g  
  c.   5.0 g  
  d.   6.02 x 1023 g  
  Hint    
      
  13.What is the SI base unit used to measure the amount of a substance?  
  a.   meter  
  b.   kelvin  
  c.   kilogram  
  d.   mole  
  Hint    
      
  14.How is one gram defined?  
  a.   one mole of protons  
  b.   10 moles of amu  
  c.   0.1 mole of amu  
  d.   one mole of amu  
  Hint    
      
  15.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   40.3 g  
  b.   58.5 g  
  c.   29.2 g  
  d.   31.7 g  
  Hint    
      
  16.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.5 kg  
  b.   0.2 kg  
  c.   0.05 kg  
  d.   0.4 kg  
  Hint    
      
  17.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.   FeO2  
  b.   Fe3O4  
  c.   FeO  
  d.   Fe2O3  
  Hint    
      
  18.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.   CH2  
  d.   C2 H3  
  Hint    
      
  19.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   waterlogged  
  b.   a hydrate  
  c.   an anhydrate  
  d.   aqueous  
  Hint    
      
  20.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   5.3 × 10-11 g  
  b.   1.9 × 1013 g  
  c.   2.7 × 10-11 g  
  d.   6.0 × 1011 g  
  Hint    

 
   
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