August 2009 Chemistry Regents #73-76

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Questions

Base your answers to questions 73 through 76 on the information below.

 

In a laboratory investigation, a student constructs a voltaic cell with iron and copper electrodes. Another student constructs a voltaic cell with zinc and iron electrodes. Testing the cells during operation enables the students to write the balanced ionic equations below.

Cell with iron and copper electrodes: Cu2+(aq) + Fe(s) ==>Cu(s) + Fe2+(aq)

Cell with zinc and iron electrodes: Fe2+(aq) + Zn(s) ==>Fe(s) + Zn2+(aq)

73 State evidence from the balanced equation for the cell with iron and copper electrodes that indicates the reaction in the cell is an oxidation-reduction reaction. [1]

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Oxidation numbers change

74 Identify the particles transferred between Fe2+ and Zn during the reaction in the cell with zinc and iron electrodes. [1]

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electrons

75 Write a balanced half-reaction equation for the reduction that takes place in the cell with zinc and iron electrodes. [1]

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Fe2+ + 2e- ==>Fe

76 State the relative activity of the three metals used in these two voltaic cells. [1]

HIGHLIGHT TO SEE THE ANSWER

Zn > Fe > Cu

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Questions 1-10 Questions 11-20 Questions 21-30 Questions 31-40 Questions 41-50

Questions 51-55 Questions56-58 Questions 59-63 Question 64 Questions 65-67 Questions 68-72 Questions 73-76 Questions 77-79 Questions 80-81

 
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