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Chemical Reactions

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

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