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Chapter 11: The Mole

Practice Test
      
  1.How many particles are present in one mole of particles?  
  a.   12  
  b.   6.02 × 1023  
  c.   1  
  d.   3.0 × 108  
  Hint    
      
  2.What is the SI base unit used to measure the amount of a substance?  
  a.   kilogram  
  b.   meter  
  c.   kelvin  
  d.   mole  
  Hint    
      
  3.How is one gram defined?  
  a.   10 moles of amu  
  b.   one mole of amu  
  c.   0.1 mole of amu  
  d.   one mole of protons  
  Hint    
      
  4.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.   0.5 kg  
  d.   0.4 kg  
  Hint    
      
  5.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   5.54 × 1020 atoms  
  b.   3.24 × 1023 atoms  
  c.   1.05 × 1018 atoms  
  d.   3.92 × 1019 atoms  
  Hint    
      
  6.What is the percent composition of carbon dioxide CO(2)?  
  a.   33% C and 66% O  
  b.   50% C and 50% O  
  c.   73% C and 27% O  
  d.   27% C and 73% O  
  Hint    
      
  7.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.   17 units  
  c.   0.5 unit  
  d.   1 unit  
  Hint    
      
  8.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    
      
  9.What is the mass of one mole of carbon-12 atoms?  
  a.   6 amu  
  b.   12 grams  
  c.   12 amu  
  d.   6 grams  
  Hint    
      
  10.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    
      
  11.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
 
  a.   1.0 mol  
  b.   4.0 mol  
  c.   2.0 mol  
  d.   0.5 mol  
  Hint    
      
  12.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.   Fe3O4  
  b.   FeO2  
  c.   Fe2O3  
  d.   FeO  
  Hint    
      
  13.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   mono-  
  b.   di-  
  c.   tri-  
  Hint    
      
  14.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    
      
  15.What is the mass of 5.0 × 1021 molecules of water?  
  a.   8.3 x 10-3 g  
  b.   0.15 g  
  c.   6.02 x 1023 g  
  d.   5.0 g  
  Hint    
      
  16.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   1.9 × 1013 g  
  b.   5.3 × 10-11 g  
  c.   6.0 × 1011 g  
  d.   2.7 × 10-11 g  
  Hint    
      
  17.How many moles of atoms are present in one mole of water?  
  a.   1 mol  
  b.   2 mol  
  c.   3 mol  
  d.   6 mol  
  Hint    
      
  18.How can the actual molecular formula be determined?  
  a.   from the molar mass divided by the mass of the empirical formula  
  b.   from the molar mass multiplied by the mass of the empirical formula  
  c.   from the molar mass alone  
  d.   from the empirical formula alone  
  Hint    
      
  19.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
 
  a.   Avogadro’s number  
  b.   mole ratio  
  c.   percent composition  
  d.   empirical formula  
  Hint    
      
  20.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   6.0 mol  
  b.   2.0 mol  
  c.   8.0 mol  
  d.   3.0 mol  
  Hint    

 
   
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