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Effective Equilibrium Constant

The equilibri...

Question

The equilibrium constant at $25^{\circ} C$ for the reaction $F e^{2 +} + A g^{+} ⇌ F e^{3 +} + A g$ is:
Given $E_{A g^{+} / A g}^{0} = 0.7998 V a n d E_{F e^{3 +} / F e^{2 +}}^{0} = 0.771 V$ , log 2 =0.30, log 3 = 0.48, $\frac{2.303 R T}{F} = 0.06$

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Solution

At equilibrium $E_{(C e l l)} = 0$
According to Nernst equation,
$E_{(C e l l)} = E_{(C e l l)}^{0} - \frac{2.303 R T}{n F} l o g Q_{c}$
$0 = (0.7998 - 0.771) - \frac{0.06}{1} l o g K_{c}$ So, $l o g K_{c} = 0.48 \Rightarrow K_{c} = 3$

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Similar questions

Q. The equilibrium constant at

25^{\circ} C

for the reaction

F e^{2 +} + A g^{+} ⇌ F e^{3 +} + A g

E_{A g^{+} / A g}^{0} = 0.7998 V a n d E_{F e^{3 +} / F e^{2 +}}^{0} = 0.771 V

, log 2 =0.30, log 3 = 0.48,

\frac{2.303 R T}{F} = 0.06

Q. Calculate the equilibrium constant for the reaction,

F e^{2 +} + C e^{4 +} ⇌ C e^{3 +} + F e^{3 +}

E_{C e^{4 +} / C e^{3 +}}^{\circ} = 1.44 V

E_{F e^{3 +} / F e^{2 +}}^{\circ} = 0.68 V

\frac{2.303 R T}{F} = 0.06

25^{o} C, l o g 4.68 = 0.67

Q. At equimolar concentrations of

F e^{2 +}

F e^{3 +}

[A g^{+}]

be so that the voltage of the galvanic cell made from

A g^{+} / A g

F e^{3 +} / F e^{2 +}

electrodes equals zero? The reaction is

F e^{2 +} + A g^{+} ⇌ F e^{3 +} + A g

. Determine the equilibrium constant at

25^{\circ} C

for the reaction. (Given:

E_{A g^{+} / A g}^{\circ} = 0.799 v o l t

E_{F e^{3 +} / F e^{2 +}}^{\circ} = 0.771 v o l t

Q. At equimolar concentration of

F e^{2 +} and F e^{3 +}

[A g^{+}]

be so that the voltage of the galvanic cell made from

(A g^{+} / A g and F e^{3 +} / F e^{2 +})

electrodes equals zero? The reaction is

F e^{2 +} + A g^{+} ⇌ F e^{3 +} + A g

E_{A g^{+} / A g}^{0} = 0.799

E_{F e^{+} / F e^{2 +}}^{0} = 0.771 volt., 10^{- 0.47} = 2.94)

Give your answer upto two decimal only.

Q. The two half-cell reactions of an electrochemical cell is given as

{A g}^{+} + e^{-} ⟶ A g; E_{{A g}^{+} | A g}^{o} = - 0.3995 V

{F e}^{2 +} ⟶ {F e}^{3 +} + e^{-}; E_{{F e}^{3 +} | {F e}^{2 +}}^{o} = - 0.7120 V

The value of cell EMF will be:

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