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Action Potential

The s†an ded ...

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The s†an ded reduction potential for the half cell NO3-(aq) + 2H+(aq) + e- → NO2 (g) + H2O(l) is 0.78 v . The reduction potnetial in 8M H+ , 1 bar N2 (g) and 1M NO3- aat 298 k will be 1> 0.886 v 2> 0.533v

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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

0.78

V. Calculate the reduction potential in

8 M H^{+}

1 M N O_{3}^{-}

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 $8 M H^{+}$ .

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

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.

Q. The standard oxidation potential for the half cell

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

- 0.78 V

.
Calculate the reduction potential in

9

H^{+}

assuming all other species at unit concentration. What will be the reduction potential in neutral medium?
(Given,

log 9 = 0.95

Q. The standard reduction potential for the half-cell having reaction,

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

0.78 v o l t

.
(i) Calculate the reduction potential in

8 M H^{+}

.
(ii) What will be the reduction potential of the half-cell in a neutral solution?
Assume all other species to be at unit concentration.

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