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Byju's Answer

Standard VII

Chemistry

Gibb's Energy and Nernst Equation

The electroch...

Question

The electrochemical cell show below is a concentration cell. $M | M^{2 +}$ (saturated solution of a sparingly soluble salt, $M X_{2}$ ) $| | M^{2 +} (0.001 {mol dm}^{- 3})$ $| M$

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 $298 K$ is $0.059 V$

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Solution

The correct option is A 1
1

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Similar questions

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)

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)

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The electrochemical cell show below is a concentration cell. M|M2+ (saturated solution of a sparingly soluble salt, MX2) ||M2+(0.001 mol dm−3) |M The emf of the cell depends on the difference in concentration of M2+ ions at the two electrodes. The emf of the cell at 298 K is 0.059 V

The correct option is A 11

The correct option is A 1
1