Science Home Product Information Site Map Search Contact Us   Glencoe Online
Quizzes Quiz
 
Chapter 11: The Mole

Practice Test
      
  1.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.   FeO2  
  d.   Fe2O3  
  Hint    
      
  2.How many moles of C3H8 are present in 451 g C3H8?  
  a.   10.2 mol  
  b.   1.44 mol  
  c.   3.84 mol  
  d.   0.879 mol  
  Hint    
      
  3.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   31.7 g  
  b.   58.5 g  
  c.   40.3 g  
  d.   29.2 g  
  Hint    
      
  4.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.   C2 H3  
  b.   CH2  
  c.   CH2  
  d.   CH  
  Hint    
      
  5.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.   FeO  
  b.   Fe2O3  
  c.   Fe3O4  
  d.   FeO2  
  Hint    
      
  6.How is one gram defined?  
  a.   one mole of protons  
  b.   one mole of amu  
  c.   10 moles of amu  
  d.   0.1 mole of amu  
  Hint    
      
  7.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
 
  a.   mole ratio  
  b.   empirical formula  
  c.   percent composition  
  d.   Avogadro’s number  
  Hint    
      
  8.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   2.0 mol  
  b.   6.0 mol  
  c.   8.0 mol  
  d.   3.0 mol  
  Hint    
      
  9.What is the molar mass of H2CrO4?  
  a.   52 g  
  b.   118 g  
  c.   2 g  
  d.   64 g  
  Hint    
      
  10.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   3.92 × 1019 atoms  
  b.   5.54 × 1020 atoms  
  c.   3.24 × 1023 atoms  
  d.   1.05 × 1018 atoms  
  Hint    
      
  11.How can the actual molecular formula be determined?  
  a.   from the empirical formula alone  
  b.   from the molar mass 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    
      
  12.What is the percent composition of carbon dioxide CO(2)?  
  a.   27% C and 73% O  
  b.   73% C and 27% O  
  c.   33% C and 66% O  
  d.   50% C and 50% O  
  Hint    
      
  13.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
 
  a.   1.0 mol  
  b.   0.5 mol  
  c.   2.0 mol  
  d.   4.0 mol  
  Hint    
      
  14.How many particles are present in one mole of particles?  
  a.   3.0 × 108  
  b.   1  
  c.   12  
  d.   6.02 × 1023  
  Hint    
      
  15.How many moles of atoms are present in one mole of water?  
  a.   2 mol  
  b.   6 mol  
  c.   3 mol  
  d.   1 mol  
  Hint    
      
  16.What is the mass of one mole of carbon-12 atoms?  
  a.   12 grams  
  b.   12 amu  
  c.   6 amu  
  d.   6 grams  
  Hint    
      
  17.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    
      
  18.What is the SI base unit used to measure the amount of a substance?  
  a.   mole  
  b.   kelvin  
  c.   kilogram  
  d.   meter  
  Hint    
      
  19.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   mono-  
  b.   tri-  
  c.   di-  
  Hint    
      
  20.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.20 × 1024  
  b.   6.02 × 1023  
  c.   34  
  d.   1.77 × 1022  
  Hint    

 
   
McGraw-Hill / Glencoe
The McGraw-Hill Companies