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Representation of Cell

The EMF of a ...

Question

The EMF of a cell is related to the equilibrium contant of the cell reaction as

A

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B

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C

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D

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Solution

The correct option is C

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Q. The emf of the cell

Z n | Z n^{2 +} (0.1 M) | | F e^{2 +} | F e (0.01 M)

0.2905 V

. Equilibrium constant for the cell reaction is

Z n | Z n^{2 +} (a = 0.1 M) | | F e^{2 +} (a = 0.01 M) | F e

.
The EMF of the above cell is

0.2905

. The equilibrium constant for the cell reaction is:

Q. Electrical energy produced by a reversible electrochemical cell is given by the free energy decrease

(- Δ G)

of the reaction occurring in the cell. According to Gibbs- Helmholtz equation, decrease in free energy is given by

- Δ G = - Δ H - T {[\frac{δ (Δ G)}{δ T}]}_{P}

- Δ H

is the decrease in enthalpy of the cell reaction at constant pressure. EMF of the cell,

E = \frac{- Δ H}{n F} + T {[\frac{δ E}{δ T}]}_{P}

. By measuring the emf of the cell and its temperature co-efficient, thermodynamic quantities like

Δ H, Δ G

Δ S

can be determined. Standard emf of the cell is related to equilibrium constant of the cell reaction as

E^{0} = \frac{2.303 R T l o g k}{n F}

.

EMF of the cell,

\begin{matrix} A & A^{2 +} & B^{+} & B (S) & (a q) & (a q) & (s) 1 M & 0.1 M \end{matrix}

is found to be 1.475 Volt. The equilibrium constant of the cell reaction at

25^{\circ}

C is (approximately)

Q. Electrical energy produced by a reversible electrochemical cell is given by the free energy decrease

(- Δ G)

of the reaction occurring in the cell. According to Gibbs- Helmholtz equation, decrease in free energy is given by

- Δ G = - Δ H - T {[\frac{δ (Δ G)}{δ T}]}_{P}

- Δ H

is the decrease in enthalpy of the cell reaction at constant pressure. EMF of the cell,

E = \frac{- Δ H}{n F} + T {[\frac{δ E}{δ T}]}_{P}

. By measuring the emf of the cell and its temperature co-efficient, thermodynamic quantities like

Δ H, Δ G

Δ S

can be determined. Standard emf of the cell is related to equilibrium constant of the cell reaction as

E^{0} = \frac{2.303 R T l o g k}{n F}

.

The standard emf of the cell,

\begin{matrix} Z n & Z n^{+ 2} & F e^{+ 3} F e^{+ 2} (S) & (a q) & (a q) (a q) \end{matrix}

25^{\circ}

C is 1.53 V and at

50^{\circ}

C is 1.55 V. The value of

Δ S^{\circ}

for the overall reaction is

| Z n^{2 +} (a = 0.1 M) ∥ F e^{2 +} (a = 0.01 M) |

F e

. The emf of the above cell is

0.2905 V

Equilibrium constant for the cell reaction is:

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