The correct value of cell potential in volt for the reaction that occurs when the following two half-cells are connected, is [2023]

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Solution

Q.
The correct value of cell potential in volt for the reaction that occurs when the following two half-cells are connected, is

${Fe}_{(a q)}^{2 +} + 2 e^{-} \to {Fe}_{(s)}, E ° = - 0.44$ $V$

${Cr}_{2} {O_{7}}_{(a q)}^{2 -} + 14 H^{+} + 6 e^{-} \to 2 {Cr}^{3 +} + 7 H_{2} O, E ° = + 1.33$ $V$ [2023]

1 + 1.77 V

2 + 2.65 V

3 + 0.01 V

4 + 0.89 V

Ans.
(1)

$E_{cell}^{\circ} = E_{cathode}^{\circ} - E_{anode}^{\circ}$

$= (+ 1.33) - (- 0.44) = + 1.77$ $V$

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