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Chapter 11: The Mole

Practice Test
  1.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  
  2.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.   1 unit  
  c.   17 units  
  d.   0.5 unit  
  3.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   6.0 mol  
  b.   8.0 mol  
  c.   3.0 mol  
  d.   2.0 mol  
  4.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   di-  
  b.   mono-  
  c.   tri-  
  5.How many particles are present in one mole of particles?  
  a.   1  
  b.   6.02 × 1023  
  c.   3.0 × 108  
  d.   12  
  6.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   1.05 × 1018 atoms  
  b.   5.54 × 1020 atoms  
  c.   3.24 × 1023 atoms  
  d.   3.92 × 1019 atoms  
  7.What is the mass of 5.0 × 1021 molecules of water?  
  a.   0.15 g  
  b.   5.0 g  
  c.   6.02 x 1023 g  
  d.   8.3 x 10-3 g  
  8.What is the molar mass of H2CrO4?  
  a.   118 g  
  b.   2 g  
  c.   52 g  
  d.   64 g  
  9.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   6.02 × 1023  
  b.   1.77 × 1022  
  c.   34  
  d.   1.20 × 1024  
  10.What is the mass of one mole of carbon-12 atoms?  
  a.   12 grams  
  b.   12 amu  
  c.   6 amu  
  d.   6 grams  
  11.What is the SI base unit used to measure the amount of a substance?  
  a.   kelvin  
  b.   meter  
  c.   kilogram  
  d.   mole  
  12.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
  a.   empirical formula  
  b.   Avogadro’s number  
  c.   percent composition  
  d.   mole ratio  
  13.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.   FeO  
  c.   Fe3O4  
  d.   FeO2  
  14.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.   Fe2O3  
  c.   FeO  
  d.   Fe3O4  
  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 molar mass multiplied by the mass of the empirical formula  
  c.   from the empirical formula alone  
  d.   from the molar mass alone  
  16.How many moles of C3H8 are present in 451 g C3H8?  
  a.   1.44 mol  
  b.   0.879 mol  
  c.   3.84 mol  
  d.   10.2 mol  
  17.How many moles of atoms are present in one mole of water?  
  a.   3 mol  
  b.   2 mol  
  c.   1 mol  
  d.   6 mol  
  18.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   aqueous  
  b.   an anhydrate  
  c.   a hydrate  
  d.   waterlogged  
  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.   SOCl  
  b.   SO2Cl2.  
  c.   SO2Cl  
  d.   SOCl2.  
  20.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   5.3 × 10-11 g  
  b.   6.0 × 1011 g  
  c.   2.7 × 10-11 g  
  d.   1.9 × 1013 g  

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