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Standard XII

Chemistry

Nernst Equation

Determine the...

Question

Determine the potential of the following cell:
$P t | H_{2} (g, 0.1 b a r) | H^{+} (a q, 10^{- 3} M) | | M n O_{4}^{-} (a q, 0.1 M)$ , $M n^{2 +} (a q, 0.01 M), H^{+} (a q, 0.01 M) | P t$
Given, $E_{M n O_{4}^{-} | M n^{2 +}}^{\circ} = 1.51 V$

1.54 V

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1.48 V

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1.84 V

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None of these

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Solution

The correct option is B $1.48 V$
Anode: $H_{2} (g) \to 2 H^{+} (a q) + 2 e^{-}; E^{\circ} = 0.0 V$

Cathode: $M n O_{4}^{-} (a q) + 8 H^{+} (a q) + 5 e^{-} \to M n^{2 +} (a q) + 4 H_{2} O (l); E^{\circ} 1.51 V$
$E_{c e l l} = E_{R P (R H S)} - E_{R P (L H S)}$
$\Rightarrow (1.51 - \frac{0.06}{5} l o g \frac{[M n^{2 +}]}{[M n O_{4}^{-}] [H^{+}]^{8}}) - (0 - \frac{0.06}{2} l o g \frac{P_{H_{2}}}{[H^{+}]^{2}})$
$= 1.51 - (\frac{0.06}{5} l o g \frac{0.01}{0.1 \times (10^{- 2})^{8}}) + \frac{0.06}{2} l o g (\frac{0.1}{(10^{- 3})^{2}})$
$= 1.48 V$

Hence option (B) is correct.

Suggest Corrections

Similar questions

Q. For the cell,

P t | C l_{2} (g, 0.4 b a r) | C l^{-} (a q, 0.1 M) | | C l^{-} (a q, 0.01 M) | C l_{2} (g, 0.2 b a r) | P t

. The cell potential at

298 K

is :

Q. Calculate the cell potential and Gibb's energy change for the following galvanic cell at

298 K

C d (s) | C d_{(a q)} {(0.001 M) | | H^{+}}_{(a q)} (0.01 M) | H_{2} (g), 1 a t m | P t

M n^{2 +} (a q)

can be determined by titration with

{M n O_{4}}^{-} (a q)

M n^{2 +} + {M n O_{4}}^{-} + {O H}^{-} \to M n O_{2} + H_{2} O (unbalanced)

25.0

mL sample of

M n^{2 +}

(aq) requires

34.77

mL of

0.05876 M K M n O_{4}

(aq) for its titration. The molarity of

M n^{2 +}

y \times 10^{- 4} M

, then y is ________.

Q. Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titrations. Some half cell reactions and their standard potentials are given below:

M n O_{4}^{-} (a q .) + 8 H^{+} (a q .) + 5 e^{-} \to M n^{2 +} (a q .) + 4 H_{2} O (l); E^{o} = 1.51 V

C r_{2} O_{7}^{2 -} (a q .) + 14 H^{+} (a q .) + 6 e^{-} \to 2 C r^{3 +} (a q .) + 7 H_{2} O (l); E^{o} = 1.38 V

F e^{3 +} (a q .) + e^{-} \to F e^{2 +} (a q .); E^{o} = 0.77 V

C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q .); E^{o} = 1.40 V

Identify the only incorrect statement regarding the quantitative estimation of aqueous

F e (N O_{3})_{2}

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox Titration. Some half – cell reactions and their standard potential are given below:
$M n O_{4}^{-} (a q) + 8 H^{+} (a q) + 5 e^{-} \to M n^{2 +} (a q) + 4 H_{2} O (I); E^{\circ} = 1.51 V$
$C r_{2} O_{7}^{2 -} (a q) + 14 H^{+} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q) + 7 H_{2} O (I); E^{\circ} = 1.38 V$
$F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{\circ} = 0.77 V$
$C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{\circ} = 1.40 V$

Identify the only incorrect statement regarding the quantitative estimation of aqueous $F e (N O_{3})_{2}$ .

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Determine the potential of the following cell:Pt|H2(g, 0.1 bar)|H+(aq, 10−3 M)||MnO−4(aq, 0.1 M), Mn2+(aq, 0.01 M),H+(aq,0.01 M)|PtGiven, E∘MnO−4|Mn2+=1.51 V

Determine the potential of the following cell:
$P t | H_{2} (g, 0.1 b a r) | H^{+} (a q, 10^{- 3} M) | | M n O_{4}^{-} (a q, 0.1 M)$ , $M n^{2 +} (a q, 0.01 M), H^{+} (a q, 0.01 M) | P t$
Given, $E_{M n O_{4}^{-} | M n^{2 +}}^{\circ} = 1.51 V$