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Consider the ...

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Consider the reaction, $C l_{2} + 2 B r^{-} (a q) ⟶ 2 C l^{-} (a q) + B r_{2}$
The emf of the cell when $[C l^{-}] = [B r_{2}] = [B r^{-}] = 0.01 M$ and $C l_{2}$ gas at $1$ atm pressure will be:
( $E^{o}$ for the above reaction is = 0.29 volt)

A

0.55

volt

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B

0.35

volt

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C

0.24

volt

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D

- 0.29

volt

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Solution

The correct option is B $0.35$ volt

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Similar questions

Q. Consider the reaction at

T = 298 K

{C l}_{2} (g) + {2 B r}^{-} (a q) ⟶ {2 C l}^{-} (a q) + {B r}_{2} (a q)

. The emf of the cell, when

[{C l}^{-}] = [{B r}^{-}] = 0.01 M

{C l}_{2}

gas is 1 atm pressure, will be (

E_{c e l l}^{o}

for the above reaction is

= 0.29 V

I_{2} + 2 e^{-} \to 2 I^{-}, standard reduction potential = + 0.54 Volt .

2 B r^{-} \to B r_{2} + 2 e^{-}, standard oxidation potential = - 1.09 Volt .

F e \to F e^{2 +} + 2 e^{-}, standard oxidation potential = + 0.44 Volt .

Out of the below given reactions, how many reactions are spontaneous in nature (predict from the above data) ?

B r_{2} + 2 I^{-} \to 2 B r^{-} + I_{2}

F e + B r_{2} \to F e^{2 +} + 2 B r^{-}

F e + I_{2} \to F e^{2 +} + 2 I^{-}

I_{2} + 2 B r^{-} \to 2 I^{-} + B r_{2}

I_{2} + 2 e^{-} \to 2 I^{-} standard reduction potential = + 0.54 Volt .

2 B r^{-} \to B r_{2} + 2 e^{-} standard oxidation potential = - 1.09 Volt .

F e \to F e^{2 +} + 2 e^{-}, standard oxidation potential = + 0.44 Volt .

Which of the following reaction(s) is/are spontaneous:

Q. Consider the following equations for a cell reaction, then:

A + B ⇌ C + D

E^{o} = x

K_{e q} = K_{1}

2 A + 2 B ⇌ 2 C + 2 D, E^{o} = y

K_{e q} = K_{2}

Q. The EMF of a cell corresponding to the reaction:

Z n_{(s)} + 2 H_{(a q)}^{+} \to Z n^{2 +} (0.1 M) + H_{2 (g)}

1

0.28

15^{o}

C.
What is the pH of the solution at the hydrogen electrode is?(Given:

E_{Z n^{2 +} / Z n}^{o} = - 0.76

E_{H^{+} / H_{2}}^{o} = 0

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