The standard electrode potential (E^ ) for the half-cell reaction Fe ^ 3+ +e^- Fe ^ 2+ at 298 K is (Given: E^ ( Fe ^ 3+ / Fe )=-0.04 V and E^ ( Fe ^ 2+ / Fe )=-0.44 V at 298 K)

Question

Quantrex Academy · Accepted Answer

Correct answer: C. +0.76 V

The given half-cell reactions are: Fe ^ 3+ + 3e^- Fe , E^ _1 = -0.04 V G^ _1 = -n_1FE^ _1 = -3 F (-0.04) = 0.12F Fe ^ 2+ + 2e^- Fe , E^ _2 = -0.44 V G^ _2 = -n_2FE^ _2 = -2 F (-0.44) = 0.88F The required half-cell reaction is: Fe ^ 3+ + e^- Fe ^ 2+ This reaction can be obtained by subtracting the second reaction from the first reaction: G^ _3 = G^ _1 - G^ _2 -1 F E^ _3 = 0.12F - 0.88F -FE^ _3 = -0.76F E^ _3 = +0.76 V Answer: +0.76 V

NEET Chemistry Question (2026) — Solution

Question

Options

Answer

Step-by-step solution