The cell in which the following reactions occurs-2 Fe 3-a q-2 I a q- 2 Fe 2-a q- I 2shas Ecell 0-0-236 V at 298 K-Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction-

Here, n = 2, T = 298 K We know that: = −2 × 96487 × 0.236 = −45541.864 J mol−1 = −45.54 kJ mol−1 Again, −2.303RT log Kc = ...

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Lattice Energy

The cell in w...

Question

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.

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

E_{c e l l}^{\circ} = 0.236 V

298 K

1 F = 96, 500 C 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 +} (aq) + 2 I^{-} (aq) \to 2 F e^{2 +} (aq) + I_{2} (s) has E_{(cell)}^{⊙} = 0.236 V

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^{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}

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