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CHXII03:ELECTROCHEMISTRY

330437 For the cell reaction,
${Cu}^{2 +} (C_{1}) (aq) + Zn (s) \to {Zn}^{2 +} (C_{2})$
$(aq) + Cu (s)$ of an electrochemical cell, the change in free energy $Δ G$ at a given temperature is a function of

1

\ln (C_{2})

2

\ln (C_{2} / C_{1})

3

\ln (C_{1})

4

\ln (C_{1} + C_{2})

Explanation:

$Δ G = - {nFE}_{cell} = - RT \ln K_{eq}$
$K_{eq} = \frac{C_{2}}{C_{1}}$
So, $Δ G$ is a function of $\ln (\frac{C_{2}}{C_{1}})$

CHXII03:ELECTROCHEMISTRY

330438 The $E^{\circ}$ in the given figure is :
supporting img

1 0.5

2 0.6

3 0.7

4 0.8

Explanation:

$\overset{+ 5}{C} {l O}_{3}^{-} + 6 e^{-} \to C l^{-} (1)$
$\overset{+ 1}{C l O} + e^{-} \to \frac{1}{2} \overset{0}{C l_{2}} (2)$
$\frac{1}{2} {C l}_{2}^{0} + e^{-} \to C l^{-} (3)$
$\overset{+ 5}{C} O_{3}^{-} + 4 e^{-} \to \overset{- 1}{C} O^{-} (4)$
$Δ G_{1} = Δ G_{2} + Δ G_{3} + Δ G_{4}$
$6 \times E_{0} = (1 \times 0.45) + (1 \times 1.07) + (4 \times 0.54)$
$6 E_{0} = 0.45 + 1.07 + 2.16$
$E_{0} = 0.613 V$

CHXII03:ELECTROCHEMISTRY

330439 The equilibrium constant of the reaction,
$C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s)$
$E^{\circ} = 0.46 V a t 298 K i s$

1

2.4 \times 10^{10}

2

2.0 \times 10^{10}

3

4.0 \times 10^{10}

4

4.0 \times 10^{15}

Explanation:

$Cu (s) + 2 {Ag}^{+} (a q) ⟶$
$C u^{2 +} (aq) + 2 Ag (s)$
$E^{^{\circ}} = 0.46 V a t 298 K$
$E^{\circ} = \frac{0.059}{2} l o g K_{C}, a t 298 K$
$0.46 = \frac{0.059}{2} \log K_{C}$
$l o g K_{C} = 15.59$
$K_{C} = a n t i l o g 15.59$
$K_{C} = 3.89 \times 10^{15} \approx 4 \times 10^{15}$

CHXII03:ELECTROCHEMISTRY

330440 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is

1

1 0^{25}

2

1 0^{20}

3

1 0^{15}

4

1 0^{30}

Explanation:

${n F E}_{c e l l}^{o} = 2 .303 R T l o g K$
$E_{c e l l}^{o} = \frac{2 .303 R T}{n F} l o g K = \frac{0 .0591}{n} l o g K$
$n = 3$
$l o g K = \frac{0 .59 \times 3}{0 .0591} = 29 .9 \Rightarrow K \approx 1 0^{30}$ .

KCET - 2010

CHXII03:ELECTROCHEMISTRY

330437 For the cell reaction,
${Cu}^{2 +} (C_{1}) (aq) + Zn (s) \to {Zn}^{2 +} (C_{2})$
$(aq) + Cu (s)$ of an electrochemical cell, the change in free energy $Δ G$ at a given temperature is a function of

1

\ln (C_{2})

2

\ln (C_{2} / C_{1})

3

\ln (C_{1})

4

\ln (C_{1} + C_{2})

Explanation:

$Δ G = - {nFE}_{cell} = - RT \ln K_{eq}$
$K_{eq} = \frac{C_{2}}{C_{1}}$
So, $Δ G$ is a function of $\ln (\frac{C_{2}}{C_{1}})$

CHXII03:ELECTROCHEMISTRY

330438 The $E^{\circ}$ in the given figure is :
supporting img

1 0.5

2 0.6

3 0.7

4 0.8

Explanation:

$\overset{+ 5}{C} {l O}_{3}^{-} + 6 e^{-} \to C l^{-} (1)$
$\overset{+ 1}{C l O} + e^{-} \to \frac{1}{2} \overset{0}{C l_{2}} (2)$
$\frac{1}{2} {C l}_{2}^{0} + e^{-} \to C l^{-} (3)$
$\overset{+ 5}{C} O_{3}^{-} + 4 e^{-} \to \overset{- 1}{C} O^{-} (4)$
$Δ G_{1} = Δ G_{2} + Δ G_{3} + Δ G_{4}$
$6 \times E_{0} = (1 \times 0.45) + (1 \times 1.07) + (4 \times 0.54)$
$6 E_{0} = 0.45 + 1.07 + 2.16$
$E_{0} = 0.613 V$

CHXII03:ELECTROCHEMISTRY

330439 The equilibrium constant of the reaction,
$C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s)$
$E^{\circ} = 0.46 V a t 298 K i s$

1

2.4 \times 10^{10}

2

2.0 \times 10^{10}

3

4.0 \times 10^{10}

4

4.0 \times 10^{15}

Explanation:

$Cu (s) + 2 {Ag}^{+} (a q) ⟶$
$C u^{2 +} (aq) + 2 Ag (s)$
$E^{^{\circ}} = 0.46 V a t 298 K$
$E^{\circ} = \frac{0.059}{2} l o g K_{C}, a t 298 K$
$0.46 = \frac{0.059}{2} \log K_{C}$
$l o g K_{C} = 15.59$
$K_{C} = a n t i l o g 15.59$
$K_{C} = 3.89 \times 10^{15} \approx 4 \times 10^{15}$

CHXII03:ELECTROCHEMISTRY

330440 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is

1

1 0^{25}

2

1 0^{20}

3

1 0^{15}

4

1 0^{30}

Explanation:

${n F E}_{c e l l}^{o} = 2 .303 R T l o g K$
$E_{c e l l}^{o} = \frac{2 .303 R T}{n F} l o g K = \frac{0 .0591}{n} l o g K$
$n = 3$
$l o g K = \frac{0 .59 \times 3}{0 .0591} = 29 .9 \Rightarrow K \approx 1 0^{30}$ .

KCET - 2010

CHXII03:ELECTROCHEMISTRY

330437 For the cell reaction,
${Cu}^{2 +} (C_{1}) (aq) + Zn (s) \to {Zn}^{2 +} (C_{2})$
$(aq) + Cu (s)$ of an electrochemical cell, the change in free energy $Δ G$ at a given temperature is a function of

1

\ln (C_{2})

2

\ln (C_{2} / C_{1})

3

\ln (C_{1})

4

\ln (C_{1} + C_{2})

Explanation:

$Δ G = - {nFE}_{cell} = - RT \ln K_{eq}$
$K_{eq} = \frac{C_{2}}{C_{1}}$
So, $Δ G$ is a function of $\ln (\frac{C_{2}}{C_{1}})$

CHXII03:ELECTROCHEMISTRY

330438 The $E^{\circ}$ in the given figure is :
supporting img

1 0.5

2 0.6

3 0.7

4 0.8

Explanation:

$\overset{+ 5}{C} {l O}_{3}^{-} + 6 e^{-} \to C l^{-} (1)$
$\overset{+ 1}{C l O} + e^{-} \to \frac{1}{2} \overset{0}{C l_{2}} (2)$
$\frac{1}{2} {C l}_{2}^{0} + e^{-} \to C l^{-} (3)$
$\overset{+ 5}{C} O_{3}^{-} + 4 e^{-} \to \overset{- 1}{C} O^{-} (4)$
$Δ G_{1} = Δ G_{2} + Δ G_{3} + Δ G_{4}$
$6 \times E_{0} = (1 \times 0.45) + (1 \times 1.07) + (4 \times 0.54)$
$6 E_{0} = 0.45 + 1.07 + 2.16$
$E_{0} = 0.613 V$

CHXII03:ELECTROCHEMISTRY

330439 The equilibrium constant of the reaction,
$C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s)$
$E^{\circ} = 0.46 V a t 298 K i s$

1

2.4 \times 10^{10}

2

2.0 \times 10^{10}

3

4.0 \times 10^{10}

4

4.0 \times 10^{15}

Explanation:

$Cu (s) + 2 {Ag}^{+} (a q) ⟶$
$C u^{2 +} (aq) + 2 Ag (s)$
$E^{^{\circ}} = 0.46 V a t 298 K$
$E^{\circ} = \frac{0.059}{2} l o g K_{C}, a t 298 K$
$0.46 = \frac{0.059}{2} \log K_{C}$
$l o g K_{C} = 15.59$
$K_{C} = a n t i l o g 15.59$
$K_{C} = 3.89 \times 10^{15} \approx 4 \times 10^{15}$

CHXII03:ELECTROCHEMISTRY

330440 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is

1

1 0^{25}

2

1 0^{20}

3

1 0^{15}

4

1 0^{30}

Explanation:

${n F E}_{c e l l}^{o} = 2 .303 R T l o g K$
$E_{c e l l}^{o} = \frac{2 .303 R T}{n F} l o g K = \frac{0 .0591}{n} l o g K$
$n = 3$
$l o g K = \frac{0 .59 \times 3}{0 .0591} = 29 .9 \Rightarrow K \approx 1 0^{30}$ .

KCET - 2010

CHXII03:ELECTROCHEMISTRY

330437 For the cell reaction,
${Cu}^{2 +} (C_{1}) (aq) + Zn (s) \to {Zn}^{2 +} (C_{2})$
$(aq) + Cu (s)$ of an electrochemical cell, the change in free energy $Δ G$ at a given temperature is a function of

1

\ln (C_{2})

2

\ln (C_{2} / C_{1})

3

\ln (C_{1})

4

\ln (C_{1} + C_{2})

Explanation:

$Δ G = - {nFE}_{cell} = - RT \ln K_{eq}$
$K_{eq} = \frac{C_{2}}{C_{1}}$
So, $Δ G$ is a function of $\ln (\frac{C_{2}}{C_{1}})$

CHXII03:ELECTROCHEMISTRY

330438 The $E^{\circ}$ in the given figure is :
supporting img

1 0.5

2 0.6

3 0.7

4 0.8

Explanation:

$\overset{+ 5}{C} {l O}_{3}^{-} + 6 e^{-} \to C l^{-} (1)$
$\overset{+ 1}{C l O} + e^{-} \to \frac{1}{2} \overset{0}{C l_{2}} (2)$
$\frac{1}{2} {C l}_{2}^{0} + e^{-} \to C l^{-} (3)$
$\overset{+ 5}{C} O_{3}^{-} + 4 e^{-} \to \overset{- 1}{C} O^{-} (4)$
$Δ G_{1} = Δ G_{2} + Δ G_{3} + Δ G_{4}$
$6 \times E_{0} = (1 \times 0.45) + (1 \times 1.07) + (4 \times 0.54)$
$6 E_{0} = 0.45 + 1.07 + 2.16$
$E_{0} = 0.613 V$

CHXII03:ELECTROCHEMISTRY

330439 The equilibrium constant of the reaction,
$C u (s) + 2 A g^{+} (a q) \to C u^{2 +} (a q) + 2 A g (s)$
$E^{\circ} = 0.46 V a t 298 K i s$

1

2.4 \times 10^{10}

2

2.0 \times 10^{10}

3

4.0 \times 10^{10}

4

4.0 \times 10^{15}

Explanation:

$Cu (s) + 2 {Ag}^{+} (a q) ⟶$
$C u^{2 +} (aq) + 2 Ag (s)$
$E^{^{\circ}} = 0.46 V a t 298 K$
$E^{\circ} = \frac{0.059}{2} l o g K_{C}, a t 298 K$
$0.46 = \frac{0.059}{2} \log K_{C}$
$l o g K_{C} = 15.59$
$K_{C} = a n t i l o g 15.59$
$K_{C} = 3.89 \times 10^{15} \approx 4 \times 10^{15}$

CHXII03:ELECTROCHEMISTRY

330440 The standard emf of galvanic cell involving 3 moles of electrons in its redox reaction is 0.59 V. The equilibrium constant for the reaction of the cell is

1

1 0^{25}

2

1 0^{20}

3

1 0^{15}

4

1 0^{30}

Explanation:

${n F E}_{c e l l}^{o} = 2 .303 R T l o g K$
$E_{c e l l}^{o} = \frac{2 .303 R T}{n F} l o g K = \frac{0 .0591}{n} l o g K$
$n = 3$
$l o g K = \frac{0 .59 \times 3}{0 .0591} = 29 .9 \Rightarrow K \approx 1 0^{30}$ .

KCET - 2010

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