Given the following half-reactions and their standard reduction potentials,

Ni2+ + 2e− Ni E° = -0.25 V
2H+ + 2e− H2 E° = 0.00 V
Ag+ + e− Ag E° = 0.80 V
a spontaneous reaction will occur between:

a. Ni2+ and H2
b. H+ and Ag
c. Ag+ and Ni
d. Ni2+ and Ag+
e. H+ can react spontaneously with any of the species here because its reduction potential is zero

I don't know I think the answer is 3 or 4? Some help? Thank you

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  1. The answer is c.
    a won't work. Why?
    Ni^2+ is -0.25 with
    H2 is 0 so Ecell is negative and that isn't spontaneous.

    But c will. Why?
    Ag^+ is 0.8
    Ni to Ni^+ is +0.25
    Add and Ecell is + so rxn is spontaneous.

    You can go through the others to convince yourself that all are negative.

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