Correct Answer - D
According to Nernst equation
`E_("cell")^(@) = (2.303 RT)/(nF)log Q`
At equilibrium
`E_("cell") = 0`
`Q = K_(eq.)` Thus,
`E_("cell")^(@) = (2.303 RT)/(nF) log K_(eq.)`
or `log K_(eq.) = (nFE_("cell")^(@))/(2.303 RT)` Substituting the value, we get
`= ((2 mol)(96500 C mol^(-1))(0.295 V))/((2.303)(8.314 JK^(-1) mol^(-1)(298 K))`
= 10
or `K^(eq.) = "antilog" 10`
`= 1.0 xx 10^(10)`