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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.   4.0 mol  
  b.   2.0 mol  
  c.   0.5 mol  
  d.   1.0 mol  
  2.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  
  3.What is the mass of 5.0 × 1021 molecules of water?  
  a.   8.3 x 10-3 g  
  b.   5.0 g  
  c.   6.02 x 1023 g  
  d.   0.15 g  
  4.How many moles of C3H8 are present in 451 g C3H8?  
  a.   3.84 mol  
  b.   0.879 mol  
  c.   1.44 mol  
  d.   10.2 mol  
  5.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.   17 units  
  b.   0.5 unit  
  c.   2 units  
  d.   1 unit  
  6.How many moles of atoms are present in one mole of water?  
  a.   2 mol  
  b.   6 mol  
  c.   1 mol  
  d.   3 mol  
  7.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  
  8.What relationship is described by the formula below?
(mass of the element/mass of the compound) × 100
  a.   Avogadro’s number  
  b.   empirical formula  
  c.   mole ratio  
  d.   percent composition  
  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.   FeO  
  b.   Fe3O4  
  c.   Fe2O3  
  d.   FeO2  
  10.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.   SO2Cl2.  
  d.   SO2Cl  
  11.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.   C2 H3  
  d.   CH2  
  12.How many particles are present in one mole of particles?  
  a.   3.0 × 108  
  b.   12  
  c.   6.02 × 1023  
  d.   1  
  13.What mass of calcium metal could be obtained from 1 kg of limestone that is 50.0% pure CaCO3?  
  a.   0.2 kg  
  b.   0.4 kg  
  c.   0.05 kg  
  d.   0.5 kg  
  14.What mass of iron is contained in 62.8 grams of pyrite FeS(2)?  
  a.   58.5 g  
  b.   29.2 g  
  c.   31.7 g  
  d.   40.3 g  
  15.How is one gram defined?  
  a.   10 moles of amu  
  b.   one mole of protons  
  c.   0.1 mole of amu  
  d.   one mole of amu  
  16.What is the percent composition of carbon dioxide CO(2)?  
  a.   73% C and 27% O  
  b.   27% C and 73% O  
  c.   50% C and 50% O  
  d.   33% C and 66% O  
  17.How many molecules of ammonia are present in 34.0 g of ammonia NH(3)?  
  a.   1.20 × 1024  
  b.   6.02 × 1023  
  c.   1.77 × 1022  
  d.   34  
  18.What is the SI base unit used to measure the amount of a substance?  
  a.   kelvin  
  b.   kilogram  
  c.   mole  
  d.   meter  
  19.Which word indicates that two water molecules are associated with a substance in a chemical compound?  
  a.   tri-  
  b.   di-  
  c.   mono-  
  20.Calculate the number of atoms in 4.00 × 10-5 g sodium.  
  a.   1.05 × 1018 atoms  
  b.   3.92 × 1019 atoms  
  c.   3.24 × 1023 atoms  
  d.   5.54 × 1020 atoms  

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