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Chapter 11: The Mole

Practice Test
  1.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   mono-  
  b.   tri-  
  c.   di-  
  2.What is the mass of 1.0 1012 molecules of O2?  
  a.   1.9 1013 g  
  b.   5.3 10-11 g  
  c.   2.7 10-11 g  
  d.   6.0 1011 g  
  3.How many particles are present in one mole of particles?  
  a.   12  
  b.   3.0 108  
  c.   6.02 1023  
  d.   1  
  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.   CH  
  d.   CH2  
  5.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   aqueous  
  b.   a hydrate  
  c.   waterlogged  
  d.   an anhydrate  
  6.What is the SI base unit used to measure the amount of a substance?  
  a.   meter  
  b.   mole  
  c.   kelvin  
  d.   kilogram  
  7.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   58.5 g  
  b.   31.7 g  
  c.   40.3 g  
  d.   29.2 g  
  8.How many moles of atoms are present in one mole of water?  
  a.   1 mol  
  b.   6 mol  
  c.   3 mol  
  d.   2 mol  
  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.   Fe2O3  
  b.   Fe3O4  
  c.   FeO  
  d.   FeO2  
  10.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   3.0 mol  
  b.   6.0 mol  
  c.   2.0 mol  
  d.   8.0 mol  
  11.How is one gram defined?  
  a.   one mole of protons  
  b.   one mole of amu  
  c.   0.1 mole of amu  
  d.   10 moles of amu  
  12.What is the molar mass of H2CrO4?  
  a.   2 g  
  b.   118 g  
  c.   52 g  
  d.   64 g  
  13.How can the actual molecular formula be determined?  
  a.   from the empirical formula alone  
  b.   from the molar mass multiplied by the mass of the empirical formula  
  c.   from the molar mass divided by the mass of the empirical formula  
  d.   from the molar mass alone  
  14.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.05 kg  
  b.   0.4 kg  
  c.   0.5 kg  
  d.   0.2 kg  
  15.What is the mass of 5.0 1021 molecules of water?  
  a.   8.3 x 10-3 g  
  b.   5.0 g  
  c.   0.15 g  
  d.   6.02 x 1023 g  
  16.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.   0.5 unit  
  b.   17 units  
  c.   2 units  
  d.   1 unit  
  17.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   34  
  b.   6.02 1023  
  c.   1.20 1024  
  d.   1.77 1022  
  18.What is the mass of one mole of carbon-12 atoms?  
  a.   6 amu  
  b.   12 amu  
  c.   12 grams  
  d.   6 grams  
  19.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.   SOCl2.  
  b.   SOCl  
  c.   SO2Cl  
  d.   SO2Cl2.  
  20.How many moles of C3H8 are present in 451 g C3H8?  
  a.   0.879 mol  
  b.   3.84 mol  
  c.   10.2 mol  
  d.   1.44 mol  

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