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Chapter 11: The Mole

Practice Test
  1.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.   SOCl2.  
  c.   SO2Cl  
  d.   SO2Cl2.  
  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.   0.5 unit  
  b.   2 units  
  c.   17 units  
  d.   1 unit  
  3.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   3.24 × 1023 atoms  
  b.   1.05 × 1018 atoms  
  c.   3.92 × 1019 atoms  
  d.   5.54 × 1020 atoms  
  4.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  
  5.What is the mass of 5.0 × 1021 molecules of water?  
  a.   6.02 x 1023 g  
  b.   0.15 g  
  c.   8.3 x 10-3 g  
  d.   5.0 g  
  6.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  
  7.How many particles are present in one mole of particles?  
  a.   12  
  b.   1  
  c.   3.0 × 108  
  d.   6.02 × 1023  
  8.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.   CH2  
  d.   C2 H3  
  9.How many moles of hydrogen are present in 2.0 grams of hydrogen gas?
  a.   0.5 mol  
  b.   2.0 mol  
  c.   4.0 mol  
  d.   1.0 mol  
  10.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.20 × 1024  
  b.   1.77 × 1022  
  c.   6.02 × 1023  
  d.   34  
  11.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.5 kg  
  b.   0.2 kg  
  c.   0.05 kg  
  d.   0.4 kg  
  12.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.   FeO2  
  d.   Fe3O4  
  13.How is one gram defined?  
  a.   one mole of amu  
  b.   one mole of protons  
  c.   0.1 mole of amu  
  d.   10 moles of amu  
  14.What is the SI base unit used to measure the amount of a substance?  
  a.   mole  
  b.   kelvin  
  c.   kilogram  
  d.   meter  
  15.How many moles of atoms are present in one mole of water?  
  a.   2 mol  
  b.   1 mol  
  c.   3 mol  
  d.   6 mol  
  16.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 multiplied by the mass of the empirical formula  
  d.   from the molar mass divided by the mass of the empirical formula  
  17.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   mono-  
  c.   di-  
  18.How many moles of hydrogen atoms are present in 2.0 moles of ammonia NH(3)?  
  a.   2.0 mol  
  b.   8.0 mol  
  c.   6.0 mol  
  d.   3.0 mol  
  19.What is the percent composition of carbon dioxide CO(2)?  
  a.   73% C and 27% O  
  b.   33% C and 66% O  
  c.   50% C and 50% O  
  d.   27% C and 73% O  
  20.What is the molar mass of H2CrO4?  
  a.   2 g  
  b.   118 g  
  c.   52 g  
  d.   64 g  

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