Question

Edison also developed a nickel-zinc battery for use in electric automobiles. The battery is now used in some cellphones and digital cameras. This battery operates in much the same way as the iron-nickel battery; both use NiO(OH) as the cathode. The E_cell^o for the nickel-zinc cell is 1.65 V at 25 °C.

(a)Calculate the ∆G° (kJ/mol) for each of the battery reactions.

(b)Which battery—the iron-nickel or nickel-zinc—has the more product-favored reaction at standard conditions? Explain your answer.

(c)Does the nickel-zinc battery have a very small or very large equilibrium constant under standard conditions? Explain your answer.

Answer 1

Solution A per given in the question The Potential difference or Eceu of Ni-Zn cell = 1.650 The cell reaction is Luta Ni(64) tho 2 zno + NiColl), (1) No of election transter 2 @ AG = ? Ex96JColoчт6 we knows AG = nFEO -2x9600x165 2318450 porile = 2-318.45 KT o Ni-zon battery is more product favoured because ago for Ni-n is more negative than Nire (E²21,200 and El Ni-zn> Eni-re) © we know 492 -2.33RT log k -318.450. J= -2°303X 8.314x 298 logk 72 २१k of Standlare Sjale logka 55.811 or ka 6,5x1055 k has very large value.