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Chemical Reactions

Practice Test
  1.As a result of the experiments of Lavoisier, you know that in a chemical reaction the mass of the products __________.  
  a.   is less than the mass of the reactants  
  b.   always equals the mass of the reactants  
  c.   cannot be predicted based on the mass of the reactants  
  d.   is twice as great as the mass of the reactants  
  2.A(n) __________ is a substance that speeds up a chemical reaction without being permanently changed itself.  
  a.   exotherm  
  b.   inhibitor  
  c.   endotherm  
  d.   catalyst  
  3.In chemical equations, __________ represent the number of units of each substance.  
  a.   coefficients  
  b.   products  
  c.   precipitates  
  d.   reactants  
  4.In a __________ reaction, two or more substances combine to form another substance.  
  a.   synthesis  
  b.   double displacement  
  c.   decomposition  
  d.   single displacement  
  5.Which of the following is a chemical reaction?  
  a.   water evaporating from salt water leaving salt crystals  
  b.   rust forming on a car body  
  c.   dew forming on grass  
  d.   water freezing into ice  
  6.The law of conservation of mass states that __________ .  
  a.   in a chemical reaction, the final mass of the products is always greater than the starting mass of the reactants  
  b.   in a chemical reaction, matter is not created or destroyed, but is conserved  
  c.   in a chemical reaction, efforts should be made to preserve rare elements without changing them  
  d.   matter can be created and destroyed but does not change forms  
  7.New substances produced by a chemical reaction are __________ .  
  a.   products  
  b.   reactants  
  c.   coefficients  
  d.   resultants  
  8.What type of reaction produces a precipitate?  
  a.   single displacement  
  b.   synthesis  
  c.   decomposition  
  d.   double displacement  
  9.The chemical formula for a compound tells __________ .  
  a.   how electrons are arranged  
  b.   what type of chemical bond it forms  
  c.   what elements it contains  
  d.   how stable the compound is  
  10.Ten grams of mercury(II) oxide react to produce 9.3 g of mercury and oxygen. What is the mass of the oxygen produced?  
  a.   7.0 g  
  b.   0.7 g  
  c.   19.3 g  
  d.   1.7 g  
  11.Why is oxygen written with a subscript 2?  
  a.   Its mass is twice as great as the reactants'.  
  b.   It usually exists as a diatomic molecule.  
  c.   Its mass increases by two times as a result of the reaction.  
  d.   There are two times as many oxygen atoms as reactant atoms.  
  12.__________ is a way to describe a chemical reaction using chemical formulas and symbols.  
  a.   The law of conservation of matter  
  b.   A chemical equation  
  c.   A physical law  
  d.   Synthesis  
  13.If electric current passes through water and initiates a decomposition reaction, what are the expected products?  
  a.   oxygen and water  
  b.   hydrogen peroxide  
  c.   hydrogen and oxygen  
  d.   hydrogen oxide  
  14.When iron combines with oxygen and water in the air to form rust, what substance in the reaction is the product?  
  a.   oxygen  
  b.   iron  
  c.   rust  
  d.   water  
  15.Some elements usually exist in combinations of two atoms. These combinations are called __________ .  
  a.   diatomic molecules  
  b.   isotopes  
  c.   ions  
  d.   coefficients  
  16.An insoluble compound that comes out of solution during a double displacement reaction is called a __________ .  
  a.   precipitate  
  b.   solvent  
  c.   catalyst  
  d.   reactant  
  17.What does it mean for a chemical equation to be balanced?  
  a.   The reactants and the products are written with the same coefficients.  
  b.   The number of reactants is equal to the number of products.  
  c.   The solid products weigh the same as the reactants.  
  d.   The same number of atoms of each element is on both sides of the equation.  
  18.A change in which one or more substances are converted into new substances is a __________ .  
  a.   nuclear reaction  
  b.   chemical fusion  
  c.   physical change  
  d.   chemical reaction  

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