For a cell involving one electron Ecell∘=0.59 VE^\circ_{cell} = 0.59\text{ V}Ecell∘=0.59 V at 298 K298\text{ K}298 K, the equilibrium constant for the cell reaction is : [Given that 2.303RTF=0.059 V at T=298 K\frac{2.303 RT}{F} = 0.059\text{ V at } T = 298\text{ K}F2.303RT=0.059 V at T=298 K]
1.0×1021.0 \times 10^21.0×102
1.0×1051.0 \times 10^51.0×105
1.0×10101.0 \times 10^{10}1.0×1010
1.0×10301.0 \times 10^{30}1.0×1030
Ecell=Ecell∘−0.059nlogQE_{cell} = E^\circ_{cell} - \frac{0.059}{n} \log QEcell=Ecell∘−n0.059logQ ...(i). At equilibrium, Q=KeqQ = K_{eq}Q=Keq and Ecell=0E_{cell} = 0Ecell=0. 0=Ecell∘−0.0591logKeq0 = E^\circ_{cell} - \frac{0.059}{1} \log K_{eq}0=Ecell∘−10.059logKeq (from equation (i)). logKeq=Ecell∘0.059=0.590.059=10\log K_{eq} = \frac{E^\circ_{cell}}{0.059} = \frac{0.59}{0.059} = 10logKeq=0.059Ecell∘=0.0590.59=10. Keq=1010=1×1010K_{eq} = 10^{10} = 1 \times 10^{10}Keq=1010=1×1010.
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