The standard reduction potential for the half cell- NO3-aq-2H-aq-e- NO2g-H2O is 0-78 V- Calculate the reduction potential in 8M H-

The correct option is C 0.886 V NO_3^ + 2H^+ +e^ → NO_2 + H_2O According to Nernst equation, #160; E=E^o + 0.0591 log [NO_3^ ][H^+]^2[NO_2] Standar ...

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Standard XII

Chemistry

Nernst Equation

The standard ...

Question

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 $8 M H^{+}$ .

0.43 V

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0.443 V

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0.886 V

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0.86 V

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Solution

The correct option is C 0.886 V
${N O_{3}}^{-} + 2 H^{+} + e^{-} \to N O_{2} + H_{2} O$

According to Nernst equation, $E = E^{o} + \frac{0.059}{1} l o g \frac{[{N O_{3}}^{-}] [H^{+}]^{2}}{[N O_{2}]}$

Standard reduction potential $E^{o} = 0.78 V$

$[{N O_{3}}^{-}] = [N O_{2}] = 1$

$[H^{+}] = 8 M$

$E = 0.78 + \frac{0.059}{1} l o g (8)^{2} = 0.78 + 0.059 l o g 64$

$E = 0.78 + (0.059) (1.8062) = 0.886 V$

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Similar questions

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^{+}

and

1 M N O_{3}^{-}

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 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.

Q. The standard reduction -potential for the half-cell:

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

is 0.78V.

[Take \frac{2.303 R T}{F} = 0.06, l o g 2 = 0.3]

Select correct options.

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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The standard reduction potential for the half cell: NO3−(aq.)+2H+(aq.)+e−→NO2(g)+H2O is 0.78 V. Calculate the reduction potential in 8M H+.

The correct option is C 0.886 VNO3−+2H++e−→NO2+H2OAccording to Nernst equation, E=Eo+0.0591log[NO3−][H+]2[NO2]Standard reduction potential Eo=0.78V[NO3−]=[NO2]=1[H+]=8ME=0.78+0.0591log(8)2=0.78+0.059log64E=0.78+(0.059)(1.8062)=0.886V

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 $8 M H^{+}$ .