The magnitude of the change in oxidising power of the ${MnO}_{4}^{-} / {Mn}^{2 +}$ couple is $x \times 10^{- 4} V$ if the $H^{+}$ concentration is decreased from $1 M$ to $10^{- 4} M$ at $25 ° C .$ (Assume concentration of ${MnO}_{4}^{-}$ and ${Mn}^{2 +}$ to be same on change in $H^{+}$ concentration). The value of $x$ is __________.
(Rounded off to the nearest integer)
[Given: $\frac{2.303 RT}{F} = 0.059$ ]

Question

The magnitude of the change in oxidising power of the ${MnO}_{4}^{-} / {Mn}^{2 +}$ couple is $x \times 10^{- 4} V$ if the $H^{+}$ concentration is decreased from $1 M$ to $10^{- 4} M$ at $25 ° C .$ (Assume concentration of ${MnO}_{4}^{-}$ and ${Mn}^{2 +}$ to be same on change in $H^{+}$ concentration). The value of $x$ is __________.

(Rounded off to the nearest integer)

[Given: $\frac{2.303 RT}{F} = 0.059$ ]

Aicharya · Accepted Answer

Eqn is- MnO 4 - + H &#8853; + 5 e - &#8594; Mn + 2 + 4 H 2 O Nernst equation: E cell &#160; = E Cell &#160; 0 - 0 . 059 5 log Mn + 2 MnO 4 - 1 H + 8 (I) Given H &#8853; = 1 M E 1 = E 0 - 0 . 059 5 log Mn + 2 MnO 4 - (II) Now: H &#8853; = 10 - 4 M E 2 = E 0 - 0 . 059 5 log Mn + 2 MnO 4 - &#215; 1 10 - 4 8 = E 0 - 0 . 059 5 log Mn + 2 MnO 4 - + 0 . 059 5 log 10 - 32 therefore: E 1 - E 2 = 0 . 059 5 &#215; 32 = 0 . 3776 &#160; V = 3776 &#215; 10 - 4 x = 3776

The magnitude of the change in oxidising power of the MnO 4 - / Mn 2 + couple is x × 10 - 4   V if…

Solution

The magnitude of the change in oxidising power of the MnO 4 - / Mn 2 + couple is x &#215; 10 - 4 &#160; V if…

Solution

The magnitude of the change in oxidising power of the MnO 4 - / Mn 2 + couple is x × 10 - 4 V if…