MIXED EQUATION PRACTICE #1

							                             MIXED EQUATION PRACTICE #1

For each of the following reactions, in part (i) write a BALANCED equation and in
part (ii) answer the question about the reaction. In part (i), coefficients should be in
terms of lowest whole numbers. Assume that solutions are aqueous unless otherwise
indicated. Represent substances in solutions as ions if the substances are extensively
ionized. Omit formulas for any ions or molecules that are unchanged by the reaction.

(a) (i)Ethene gas is burned in air.

      (ii) What specific type of hydrocarbon is ethene?

(b) (i) Solutions of cobalt(II) nitrate and sodium hydroxide are mixed.

      (ii) What are the spectator ions in this reaction?

(c) (i) A strip of zinc is added to a solution of 6.0-molar hydrobromic acid.

      (ii) What would you observe happening to the zinc strip in this reaction?

(d) (i) Solutions of tin(II) chloride and iron(III) chloride are mixed.

      (ii) Is this a redox reaction? If so, what is reduced?

(e) (i) Solid sodium oxide is added to distilled water.


      (ii) Estimate the pH of the final solution.

(f) (i) Excess hydrochloric acid is added to a solution of diamminesilver(I) nitrate.

      (ii) What would you observe happening in this reaction?


(g) (i)    Solid calcium sulfite is heated in a vacuum.

      (ii) Is this a redox reaction? If so, what is oxidized?


(h)     (i) Equal volumes of equimolar solutions of phosphoric acid and potassium
      hydroxide are mixed.


      (ii) Estimate the pH of the final solution.
MIXED EQUATION PRACTICE #2

For each of the following reactions, in part (i) write a BALANCED equation and in
part (ii) answer the question about the reaction. In part (i), coefficients should be in
terms of lowest whole numbers. Assume that solutions are aqueous unless otherwise
indicated. Represent substances in solutions as ions if the substances are extensively
ionized. Omit formulas for any ions or molecules that are unchanged by the reaction.

(a) (i) Powdered strontium oxide is added to distilled water.

    (ii) Is the product acidic or basic? How could you test to confirm this?


(b) (i) Butanol is burned in air.


    (ii) If insufficient air was present, what different product(s) could be formed?


(c) (i) A solution of copper(II) chloride is added to a solution of sodium sulfide.

    (ii) What color(s) would the two solutions be before the reaction?

(d) (i) A small piece of calcium metal is added to hot distilled water.

    (ii) What would you observe in this reaction?


(e) (i) Excess hydrobromic acid solution is added to a solution of potassium hydrogen
    carbonate.

    (ii) Is this a redox reaction?


(f) (i) Carbon monoxide gas is passed over hot iron(III) oxide.

    (ii) Name an industrial application of this reaction.

(g) (i)Excess concentrated ammonia solution is added to a solution of nickel(II) sulfate.

    (ii) Which species acts as a Lewis base in this reaction?


(h) (i)A solution of tin(II) nitrate is added to a solution of silver nitrate.

    (ii) Name the oxidizing agent in this reaction.
                      EQUATION PRACTICE TEST

There are four pages to this test. Answer all pages!!!

For each of the following reactions, in part (i) write a BALANCED equation and in
part (ii) answer the question about the reaction. In part (i), coefficients should be in
terms of lowest whole numbers. Assume that solutions are aqueous unless otherwise
indicated. Represent substances in solutions as ions if the substances are extensively
ionized. Omit formulas for any ions or molecules that are unchanged by the reaction.

Example: (i) A strip of magnesium is added to a solution of silver nitrate.
         (ii) What would your observe happening to the magnesium?

 Ex.             Mg + 2Ag+  Mg2+ + 2Ag
                 The Mg strip would become smaller and would become
                 coated with solid silver.
Set 1
(a) (i.) A small piece of sodium metal is added to distilled water.
    (ii)  Is this reaction endothermic or exothermic?




 (a)



(b) (i) Solid ammonium carbonate is heated.
    (ii) Is this a redox reaction?




 (b)



(c) (i) A solution of potassium dichromate is added to an acidified solution of iron(II)
    chloride.
    (ii)   What color is the solution of potassium dichromate?


 (c)
Set 2
(a) (i)Excess sodium cyanide solution is added to a solution of silver nitrate.
        (ii) What undesirable product would result if this solution was acidified?




 (a)




   (b) (i) A concentrated solution of hydrochloric acid is added to solid potassium
       permanganate.
       (ii) What color changes, if any, would be observed in this reaction?




 (b)



   (c) (i) Phosphorus(V) oxide powder is sprinkled over distilled water.
       (ii) Estimate the pH of the resulting solution.




 (c)
Set 3
    a) (i) Sulfur trioxide gas is bubbled through a solution of sodium hydroxide.
       (ii) Is a precipitate formed in this reaction? If so, name it.




  (a)



    b) (i.) Ethanol is burned in oxygen.
       (ii) What is the oxidizing agent in this reaction? Justify your answer.




  (b)



c) (i)  A strip of zinc is placed in a solution of nickel(II) nitrate.
    (ii) What color change, if any, would you observe in this reaction?




  (c)
Set 4


(a) (i) Solid calcium hydride is added to distilled water.
    (ii) Give two laboratory tests that would help to identify the product(s) of this
reaction. Describe the results of these tests.




 (a)



(b) (i) Chlorine gas is bubbled into a cold, dilute solution of potassium hydroxide.
    (ii) Give the name for this specific type of redox reaction.




 (b)



(c) (i) Solid aluminum hydroxide is added to a concentrated solution of potassium
hydroxide.
    (ii) Name the product(s) of this reaction.




 (c)
Practice Test Set 1 Answers
Practice Test Set 2 Answers
   AP CHEMISTRY EQUATION UNIT TEST

There are two pages to this test (and two answer sheets). Answer both pages!!!

Answer FIVE of the eight choices in this problem. (Answers to more than five choices
will not be scored.)

Give the formulas to show the reactants and the products of the following chemical
reactions. Each of the reactions occurs in aqueous solution unless otherwise indicated.
Represent substances as ions if the substance is extensively ionized. Omit formulas for
any ions or molecules that are unchanged by the reaction. In all cases a reaction occurs.
Balance all equations.
Example: A strip of magnesium is added to a solution of silver nitrate.

 Ex.             Mg + Ag+  Mg2+ + Ag


(a) Ammonia gas is bubbled into a solution of ethanoic (acetic) acid.


(b) A piece of nickel metal is immersed in a solution of copper(II) sulfate.


(c) Solutions of potassium permanganate and sodium oxalate are mixed.


(d) Chlorine gas is bubbled into a solution of sodium bromide


(e) Drops of liquid dinitrogen trioxide are added to distilled water.


(c) Solid ammonium carbonate is added to a saturated solution of barium hydroxide.


(g) Solid calcium carbonate is strongly heated.


(h) Equal volumes of equimolar solutions of disodium hydrogen phosphate and
    hydrochloric acid are mixed.




Answer FIVE of the eight choices in this problem. (Answers to more than five choices
will not be scored.)
(a) Solid potassium amide is added to distilled water.



(b) Hydrogen gas is passed over hot iron(II) oxide powder.



(c) Sulfur dioxide gas is bubbled into distilled water.



(d) Phosphine (phosphorus trihydride) gas is bubbled into liquid boron trichloride.



(e) Excess potassium hydroxide solution is added to a solution of aluminum nitrate



(f) A solution of nickel chloride is added to a solution of sodium sulfide.



(g) A strip of magnesium metal is heated strongly in pure nitrogen gas.



(h) A solution of sodium bromide is added to an acidified solution of potassium bromate.




                             Equation Test Set 1 Answers
Equation Test Set 2 Answers