Types of Chemical Reactions - DATA CHART & QUESTIONS
OBSERVATIONS:

 

Before Rxn.

During rxn.

After rxn.

Special Notes

Part A

 

 

 

 

 

 

 

 

Part B

 

 

 

 

 

 

 

 

Part C

 

 

 

 

 

 

 

 

Part D

 

 

 

 

 

 

 

 

Part E

 

 

 

 

 

 

 

 

 



REACTIONS:
In this section, you will be writing the equations that you performed in Parts A, B, C, D, & E.  You will write out the equation in words (including states of matter - aq, s, l. g), then you will write it out using formulas.  (When using formulas, do not forget to balance the equations.  Also remember that some elements by themselves occur as diatomic molecules.)

EXAMPLE:  

- Aqueous silver nitrate plus aqueous sodiuum chloride yields aqueous sodium nitrate and solid silver chloride

- AgNO3 (aq) + NaCl (aq) --> NaNO3 (aq) + AgCl (s)

Part A
1.  Aqueous copper (II) sulfate solution is reacted with an aqueous solution of sodium hydroxide to produce


2.  Write the reaction using symbols and formulas.  (Do not forget to include the state of matter for each
substance.  (aq) means aqueous or dissolved in water, (s) means solid, (l) means liquid, and (g) means gas)


Part B
1.  solid zinc metal and an aqueous solution of sulfuric acid produces


2.  Zn(s) + ...


Part C
1.  solid iron plus copper (II) sulfate aqueous solution yields


2.  Rewrite the equation using symbols.



Part D

1. solid copper plus iron (II) sulfate aqueous solution yields


2.  Rewrite the equation using symbols.



Part E
1.  ___________________________________ solid is added to hydrogen peroxide as a catalyst to produce


2.  Rewrite using symbols.  Catalysts are usually placed on the arrow. 

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QUESTIONS:
Part A
1.  Why is this called a double replacement reaction?

2.  Using a solubility chart (like the one found on p. 900 of your textbook), which of the products is the
precipitate (ppt) in this reaction? 
EXTRA CREDIT: Give another likely reason for your answer to this question based on a visual observation of
the ppt.  (Hint: The fact that Cu is a transition metal has something to do with it.)

3.  What would be evidence in this procedure that the reaction was complete?  (Refer to step 3 and think about
what happened.)

Part B
1.  What evidence did you observe that indicated that a reaction was taking place?

2.  Why is this called a single replacement reaction?

3.  List two (2) other metals that could have worked in this procedure.  (Hint:  You will need to use the Activity
Series
for this question.)

4. a.  List two (2) other zinc compounds that are also soluble in water.
         (EXTRA CREDIT:  Write the formulas for these compounds.)
    b.  List one (1) zinc compound that is soluble in acid, but not in water. 
(EXTRA CREDIT:  Write the formula for this compound.)

Part C
1.  What is the purpose of using H2SO4 (sulfuric acid)?

2.  What formed on the iron?  Why?  (Hint:  Activity Series)

3.  List two (2) other metals that would produce the same results as the iron.

Part D
1.  What formed on the copper?  Why?

2.  List two (2) other metals that would produce the same results as the copper.

Part E
1.  Describe the physical appearance of hydrogen peroxide.

2.  What gas was produced?  EXTRA CREDIT: How could you prove your answer?

3.  Describe the role MnO2 played in the reaction.

4.  What is the correct name for the compound MnO2?

5.  What is one (1) everyday use of hydrogen peroxide?  (If your answer is correct and different from all other
answers in your class, you get 5 bonus points on your lab!)

* BONUS *
A bewildered but determined chemistry student is given 4 test tubes of colorless, odorless solutions.  None of the tubes are labeled, but he is told they contain individually one of the following:  AgNO3, Ca(NO3)2, Ba(NO3)2, and NaNO3.  Based on solubility, what kind of salt (compound) solution could he add to pick out the test tube that contained the silver?

 

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