A cell reaction with n = 2 has E deg_cell = 0.0591 V at 298 K. Take (2.303RT)/(F) = 0.0591 V and F = 96500 C mol^-1. Which statements are correct?

Delta_r G deg = -11.41 kJ mol^-1

When the reaction quotient Q = 10, the cell EMF is negative

JEE Main levelOne or more correct optionsDifficulty 2 of 3ec066

A cell reaction with $n = 2$ has $E_{cell}^{\circ} = 0.0591 V$ at 298 K. Take $\frac{2.303 RT}{F} = 0.0591 V$ and $F = 96500 C mo l^{- 1}$ . Which statements are correct?

lo g K = n E^{\circ} /0.0591 = 2 \times 0.0591/0.0591 = 2

, so

K = 100

(A, B).

Δ_{r} G^{\circ} = - n F E^{\circ} = - 2 \times 96500 \times 0.0591 = - 11406 J = - 11.41 kJ

(C). The EMF becomes zero only when

Q = K = 100

; at

Q = 10 < K

E = E^{\circ} - (0.0591/2) lo g 10 = 0.0591 - 0.0296 = + 0.0296 V

, still positive. D is wrong.