1. Using a standard reduction potential table, such as Table 18, in our textbook

Question

1. Using a standard reduction potential table, such as Table 18, in our textbook a. Write the half-reaction for the reduction of Mg" and write its standard reduction potential. b. Write the half-reaction for the reduction of H and its standard reduction potential. c. Write the half-reaction for the reduction of Zn2 and its standard reduction potential. 2. If the half-cell containing Mg" and Mg (see la above) were combined with the half-cell in lb, what spontaneous reaction would occur? Write that overall reaction and calculate its standard cell potential, E [See example in the intro to this lab.] (Do you recognize this reaction from the Redox Activity?)

Explanation / Answer

1.

(a)

Mg2+ (aq.) + 2 e- ------------> Mg (s)

E0Mg2+/Mg = - 2.38 V

(b)

2 H+ (aq.) + 2 e- ----------> H2 (g)

E0H+/H2 = 0.00 V

(c)

Zn2+ (aq.) + 2 e- ------------> Zn (s)
E0Zn2+/Zn = - 0.76 V

2.

SPontaneous reaction that occurr is:

Mg (s) + 2 H+ (aq.) ----------> Mg2+ (aq.) + H2 (g)
E0cell = E0H+/H2 - E0Mg2+/Mg = 0.00 - ( - 2.38 ) = + 2.38 V

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