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Standard Electrode Potentials

The standard ...

Question

The standard reduction potential for the half cell :

$N O_{3}^{-} (a q) + 2 H^{+} (a q) + e^{-} ⟶ N O_{2} (g) + H_{2} O$

is $0.78$ V. What will be the reduction potential of the half cell in a neutral solution? Assume all the other species to be at unit concentration.

1.1 V

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- 0.047 V

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0.75 V

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1.33 V

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Solution

The correct option is B $- 0.047 V$

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Similar questions

N O_{3}^{-} (a q .) + 2 H^{+} (a q .) + e^{-} \to N O_{2} (g) + H_{2} O

0.78 v o l t

8 M H^{+}

The standard reduction potential for the half cell:

$N O {_{3}}^{-} (a q .) + 2 H^{+} (a q .) + e^{-} \to N O_{2} (g) + H_{2} O$ is 0.78 V.

Calculate the reduction potential in $8 M H^{+}$ .

N O_{3}^{-} (a q) + 2 H^{+} (a q) + e^{-} ⟶ N O_{2} (g) + H_{2} O

0.78

8 M H^{+}

1 M N O_{3}^{-}

N O_{2}^{-} (g) + H_{2} O \to N O_{3}^{-} (aq) + 2 H^{+} (aq) + 2 e^{-}

- 0.78 V

9

H^{+}

log 9 = 0.95

The standard reduction potential for the half cell:

$N O_{3}^{⊖} (a q) + 2 H^{\oplus} + \to N O_{2} (g) H_{2} O$ is 0.78 V

The reduction potential in 8 M $H^{\oplus}$ is: (in V)

Assume all the other species to be at unit concentration. ( write your answer to nearest integer)

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