The cell in which the following reaction occurs:

$2 F e^{3 +} (a q) + 2 I^{-} (a q) \to 2 F e^{2 +} (a q) + I_{2} (s)$

has $E_{c e l l}^{\circ} = 0.236 V$ at $298 K$ .

Calculate the standard Gibbs energy of the cell reaction. (Given : $1 F = 96, 500 C m o l^{- 1})$

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Solution

Standard Gibbs free energy of the cell is given by the formula:

$Δ G^{o} = - n F E^{o} = - 2 \times 96500 \times 0.236 = - 45.54 K J$

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Similar questions

2 F e^{3 +} (a q) + 2 I^{-} (a q) \to 2 F e^{2 +} (a q) + I_{2} (s)

E_{cell}^{⊝} = 0.236 V

m o l^{- 1}

m o l^{- 1}

2 F e_{(a q)}^{3 +} + 2 I_{(a q)}^{-} \to 2 F e_{(a q)}^{2 +} + I_{2 (s)}

E_{c e l l}^{o} = 0.236 V

298 K

2 F e^{3 +} (a q) + 2 I^{-} (a q) \to 2 F e^{2 +} (a q) + I_{2} (s)

E_{cell}^{⊝} = 0.236 V

m o l^{- 1}

m o l^{- 1}

The cell in which the following reactions occurs:

has = 0.236 V at 298 K.

Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

2 F e^{3 +} (aq) + 2 I^{-} (aq) \to 2 F e^{2 +} (aq) + I_{2} (s) has E_{(cell)}^{⊙} = 0.236 V

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