Problem: Consider the redox reaction: PbO2(s)  +  Ba(s)  +  4H+ (aq)  →  Pb+2 (aq)  +  Ba +2 (aq) + 2H2O(l)  At standard conditions ε° = 4.36 V (highly spontaneous). Suppose the voltage ε, is measured for the above reaction when the [H+] concentration is [H+] = 10 -7 M instead of [H+] = 1M. How does ε compare to ε° (circle one): ε > ε°        ε < ε°         ε = ε°        Can't be determined

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Problem Details

Consider the redox reaction:

PbO2(s)  +  Ba(s)  +  4H(aq)  →  Pb+2 (aq)  +  Ba +2 (aq) + 2H2O(l) 

At standard conditions ε° = 4.36 V (highly spontaneous). Suppose the voltage ε, is measured for the above reaction when the [H+] concentration is [H+] = 10 -7 M instead of [H+] = 1M.

How does ε compare to ε° (circle one):

ε > ε°        ε < ε°         ε = ε°        Can't be determined

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