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Standard X

Chemistry

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The standard emf of a cell involving one electron change is found to be 0.591 V at 25°C. The equilibrium constant of the reaction is
[Given: $F = 96500 C m o l^{- 1}$ ]

1.0 \times 10^{1}

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1.0 \times 10^{5}

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1.0 \times 10^{10}

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1.0 \times 10^{30}

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Solution

The correct option is A $1.0 \times 10^{10}$

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Similar questions

The standard e.m.f. of a cell, involving one electron change is found to be 0.591 V at $25^{0}$ C. The equilibrium constant of the reaction is (F = 96500Cmol $^{- 1}$ , R = 8.314JK $^{- 1}$ mol $^{- 1}$ ) :

Q. For a cell involving one electron,

E_{c e l l}^{0}

= 0.59 V at 298 K, the equilibrium constant for the cell reaction is:
[Given that

\frac{2.303 R T}{F}

= 0.059 V at T = 298 K]

Q. The standard emf of a cell, involving one electron change is found to be

0.591 V

25

. The equilibrium constant of the reaction is

(F = 96500 C {m o l}^{- 1}, R = 8.314 K^{- 1} {m o l}^{- 1})

Q. The standard e.m.f. of a cell involving one electron change is found to 0.591 V at 25

^{o}

C. The equilibrium constant of the reaction is:

Q. The standard e.m.f. of a cell, involving one electron change is found to be 0.591 V at

25^{o} C

. The equilibrium constant of the reaction is

(F = 96, 500

Cmol

^{- 1}, R = 8.314 J K^{- 1}

mol

^{- 1})

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The standard emf of a cell involving one electron change is found to be 0.591 V at 25°C. The equilibrium constant of the reaction is [Given: F=96500Cmol−1]

The correct option is A 1.0×1010

The standard emf of a cell involving one electron change is found to be 0.591 V at 25°C. The equilibrium constant of the reaction is
[Given: $F = 96500 C m o l^{- 1}$ ]

The correct option is A $1.0 \times 10^{10}$