In a galvanic cell, one half-cell consists of a nickel strip dipped into a 1.00 M...
In a galvanic cell, one half-cell consists of a
nickel strip dipped into a 1.00 M solution of
Ni(NO3)2. In the second
half-cell, solid manganese is in contact with a
1.00 M solution of Mn(NO3)2.
Ni is observed to plate out as the galvanic cell
operates, and the initial cell voltage is measured to be
0.935 V at 25°C.
(a) Write balanced equations for the half-reactions at the anode
and the cathode. Show electrons as e-. Use the smallest
integer coefficients possible and the pull-down boxes to indicate
states. If a box is not needed, leave it blank.
Half-reaction at anode (do not multiply by factor):
| _______ (aq)(s)(l)(g) | + | ________(aq)(s)(l)(g) | ---> | ________(aq)(s)(l)(g) | + | _______(aq)(s)(l)(g) |
Half-reaction at cathode (do not multiply by factor):
| ________(aq)(s)(l)(g) | + | __________(aq)(s)(l)(g) | ---> | ________(aq)(s)(l)(g) | + | ________(aq)(s)(l)(g) |
(b) Calculate the standard reduction potential of a
Mn2+|Mn half-cell. The
standard reduction potential of the
Ni2+|Ni electrode is
-0.250 V.
V
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