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Chapter 11: The Mole

Practice Test
  1.What is the percent composition of carbon dioxide CO(2)?  
  a.   50% C and 50% O  
  b.   73% C and 27% O  
  c.   27% C and 73% O  
  d.   33% C and 66% O  
  2.A compound that has a specific number of water molecules bound to the structure is ______________?  
  a.   waterlogged  
  b.   a hydrate  
  c.   aqueous  
  d.   an anhydrate  
  3.What is the SI base unit used to measure the amount of a substance?  
  a.   meter  
  b.   mole  
  c.   kilogram  
  d.   kelvin  
  4.How many moles of atoms are present in one mole of water?  
  a.   2 mol  
  b.   1 mol  
  c.   6 mol  
  d.   3 mol  
  5.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.   CH  
  c.   CH2  
  d.   CH2  
  6.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.   6.0 mol  
  d.   3.0 mol  
  7.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  
  8.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.   Fe3O4  
  b.   FeO2  
  c.   FeO  
  d.   Fe2O3  
  9.What is the mass of 1.0 × 1012 molecules of O2?  
  a.   1.9 × 1013 g  
  b.   2.7 × 10-11 g  
  c.   5.3 × 10-11 g  
  d.   6.0 × 1011 g  
  10.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   3.92 × 1019 atoms  
  b.   1.05 × 1018 atoms  
  c.   5.54 × 1020 atoms  
  d.   3.24 × 1023 atoms  
  11.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
  a.   0.5 mol  
  b.   1.0 mol  
  c.   4.0 mol  
  d.   2.0 mol  
  12.What is the mass of one mole of carbon-12 atoms?  
  a.   6 grams  
  b.   6 amu  
  c.   12 grams  
  d.   12 amu  
  13.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   mono-  
  c.   di-  
  14.How many moles of C3H8 are present in 451 g C3H8?  
  a.   3.84 mol  
  b.   1.44 mol  
  c.   10.2 mol  
  d.   0.879 mol  
  15.How is one gram defined?  
  a.   one mole of protons  
  b.   0.1 mole of amu  
  c.   one mole of amu  
  d.   10 moles of amu  
  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.   0.05 kg  
  c.   0.4 kg  
  d.   0.2 kg  
  17.How many particles are present in one mole of particles?  
  a.   6.02 × 1023  
  b.   12  
  c.   3.0 × 108  
  d.   1  
  18.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  
  19.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
  a.   mole ratio  
  b.   empirical formula  
  c.   Avogadro’s number  
  d.   percent composition  
  20.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.20 × 1024  
  b.   34  
  c.   1.77 × 1022  
  d.   6.02 × 1023  

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