Compute the equilibrium constant for the spontaneous reaction between Ni2+(aq) and Cd(s).
Express your answer using two significant figures.

9.8 × 10^21

Explanation:

Equation of the reaction;

Cd(s) + Ni^2+(aq) > Cd^2+(aq) + Ni(s)

E°cell= E°cathode - E°anode

E°cathode= -0.25 V

E°anode = -0.40 V

E°cell= -0.25 - (-0.40)

E°cell = 0.65 V

∆G= -nFE°cell

∆G= -(2 × 96500 × 0.65)

∆G = -125450 J

From;

∆G= -RTlnK

lnK = ∆G/-RT

K= e^∆G/-RT

K= e^-[-(125450/8.314 × 298)]

K= 9.78 × 10^21

that's just how they are

explanation:

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