The relationship between standard cell potential ($E^{\circ}_{cell}$) and the equilibrium constant ($K_c$) at $298\text{ K}$ ($25^{\circ}\text{C}$) is given by the Nernst equation at equilibrium: $E^{\circ}_{cell} = \frac{2.303RT}{nF} \log K_c = \frac{0.059}{n} \log K_c$ Given: $E^{\circ}_{cell} = 0.295\text{ V}$ $n = 2$ Substituting the values into the equation: $0.295 = \frac{0.059}{2} \log K_c$ $\log K_c = \frac{0.295 \times 2}{0.059} = \frac{0.590}{0.059} = 10$ Therefore, $K_c = 10^{10} = 1.0 \times 10^{10}$ .