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Byju's Answer

Standard XI

Chemistry

Gibb's Energy and Nernst Equation

The electroch...

Question

The electrochemical cell shown below is a concentration cell. $M | M^{2 +}$ (Saturated solution of a sparingly soluble salt, $M X_{2}) | | M^{2 +} (0.001 m o l d m^{- 3}) M .$ The emf of the cell depends on the difference in concentration of $M^{2 +}$ ions at the two electrodes. The emf of the cell at 298K is 0.059

The value of $Δ G (k J m o l^{- 1})$ for the given cell is: (take $1 F = 96500 C m o l^{- 1})$

- 5.7

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11.4

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- 11.4

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Solution

The correct option is D $- 11.4$
$Δ G = - n E F = \frac{2 \times 0.059 \times 96500}{1000} k J = - 11.4 k J$

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Similar questions

Q. The electrochemical cell shown below is a concentration cell.

M | M^{2 +}

(Saturated solution of a sparingly soluble salt,

M X_{2}) | | M^{2 +} (0.001 m o l d m^{- 3}) M .

The emf of the cell depends on the difference in concentration of

M^{2 +}

ions at the two electrodes. The emf of the cell at 298K is 0.059

The value of

Δ G (k J m o l^{- 1})

for the given cell is: (take

1 F = 96500 C m o l^{- 1})

Q. The electrochemical cell shown below is a concentration cell.

M | M^{2 +}

(Saturated solution of a sparingly soluble salt,

M X_{2}) | | M^{2 +} (0.001 m o l d m^{- 3}) M .

The emf of the cell depends on the difference in concentration of

M^{2 +}

ions at the two electrodes. The emf of the cell at 298K is 0.059

The value of

Δ G (k J m o l^{- 1})

for the given cell is: (take

1 F = 96500 C m o l^{- 1})

Q. The electrochemical cell shown below is a concentration cell,

M | M^{2 +}

(Saturated solution of a sparingly soluble salt,

M X_{2}) | | M^{2 +} (0.001 m o l d m^{- 3}) M .

The emf of the cell depends on the difference in concentration of

M^{2 +}

ions at the two electrodes. The emf of the cell at 298K is 0.059

The solubility product

(K_{s p} : m o l^{3} d m^{- 9})

M X_{2}

at 298 K based on the information available the given concentration cell is (take

2.303 \times R \times 298 / F = 0.059 V)

The electrochemical cell shown below is a concentration cell.

M | M^{2 +}

(saturated solution of a sparingly soluble salt,

M X_{2}

)

| | M^{2 +} (0.001 m o l d m^{- 3}) | M

The emf of the cell depends on the difference in concentrations of

M^{2 +}

ions at the two electrodes.

The emf of the cell at

298

0.059 V

The value of

Δ G

( kJ mol

^{- 1}

) for the given cell is:

[take 1F

= 96500

C mol

^{- l}

]

Q. The electrochemical cell shown below is a concentration cell,

M | M^{2 +}

(Saturated solution of a sparingly soluble salt,

M X_{2}) | | M^{2 +} (0.001 m o l d m^{- 3}) M .

The emf of the cell depends on the difference in concentration of

M^{2 +}

ions at the two electrodes. The emf of the cell at 298K is 0.059

The solubility product

(K_{s p} : m o l^{3} d m^{- 9})

M X_{2}

at 298 K based on the information available the given concentration cell is (take

2.303 \times R \times 298 / F = 0.059 V)

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The correct option is D −11.4ΔG=−nEF=2×0.059×965001000kJ=−11.4kJ

The correct option is D $- 11.4$
$Δ G = - n E F = \frac{2 \times 0.059 \times 96500}{1000} k J = - 11.4 k J$