Question

determine the values of equilibrium constant Kc and delta G for the following reaction
Ni + 2 Ag+ gives to Ni2+ +2Ag
​Enot =1.05v , 1F=96500 CMOL^-1

Answer 1

please find your answer, feel free to write me about the answer, sorry about my hand writing :-)

Answer 2

Answer: The value of equilibrium constant $K_c$ is $3.16\times 10^{-36}$ and value of $\Delta G$ is 202600 J

Explanation:

1) The standard emf of a cell is related to Gibbs free energy by following relation:

$\DeltaG=-nFE^0$

$\Delta G$ = gibbs free energy

$Ni+2Ag^+\rightarrow Ni^{2+}+2Ag$

n= no of electrons gained or lost = 2

F= faraday's constant

$E^0$ = standard emf

$\Delta G=-2\times 96500\times 1.05$

$\Delta G=202600J$

2) The equilibrium constant is related to Gibbs free energy by following relation:

$\Delta G=-2.303RT\times logK$

$\Delta G$ = gibbs free energy

R = gas constant = 8.314J/Kmol

T = temperature in Kelvin = 298 K

$\Delta G=-2.303RT\times logK$

$202600J=-2.303\times 8.314\times 298\times logK$

$K= 3.16\times 10^{-36}$