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The temperature coefficient of the emf i.e., $\frac{dE}{dt} = - 0 .00065 {VK}^{- 1}$ for the cell $C d | C d C l_{2} (1 M) | | A g C l (s) | A g$ at $25 ° C$ . Calculate the entropy changes $ΔS at 298 K$ for the cell reaction $Cd + 2 AgCl \to {Cd}^{2 +} + 2 {Cl}^{-} + 2 Ag$ .

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Important Questions on Electrochemistry

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

The standard free energy change for the cell reaction

Z n_{(s)} + C u_{(a q)}^{2 +} \to Z n_{(a q)}^{2 +} + C u_{(s)}

(E_{Z n^{2 +} / Z n} ° = - 0.76 V, E_{C u^{2 +} / C u} ° = + 0.34 V, 1 F = 96500 {Cmol}^{- 1})

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

If the standard electrode potential for a cell is

2 V

300 K,

the equilibrium constant

(K)

for the reaction.

Zn (s) + {Cu}^{2 +} (aq) ⇌ {Zn}^{2 +} (aq) + Cu (s)

300 K

is approximately:

(R = 8 {JK}^{- 1} {mol}^{- 1}, F = 96000 C {mol}^{- 1})

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

The emf of the following cell is $1.229 V$ at $298 K$ .

$Pt, H_{2} (1 atm) |H^{+} (1 M)| O_{2} (1 atm), Pt$

$H_{2} + \frac{1}{2} O_{2} ⇌ H_{2} O$

The standard free energy change for the cell reaction is________ $[F = 9.649 \times 10^{4} C {mol}^{- 1}]$

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

The standard emf of the cell $(E_{cell} °$ and equilibrium constant $(K_{eq})$ of the following reaction of $298 K$

${Cd}^{2 +} + 4 {NH}_{3} ⇌ Cd {({NH}_{3})}_{4}^{2 +}$

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

For the cell reaction

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

$E_{c e l l}^{0} = 0.24 V$ at $298 K .$ The standard Gibbs energy $(Δ_{r} G^{o})$ of the cell reaction is:

[Given that Faraday constant $F = 96500 C m o l^{- 1}$ ]

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

The standard e.m.f. of the cell, $Cd (s) |{CdCl}_{2} (aq) (0.1 M)| | AgCl (s) | Ag (s)$ in which the cell reaction is $Cd (s) + 2 AgCl (s) ⟶ 2 Ag (s) + {Cd}^{2 +} (aq) + 2 {Cl}^{-} (aq)$ is $0.6915 V$ at $0 ° C$ and $0.6753 V$ at $25 ° C$ . The enthalpy change of the reaction at $25 ° C$ is

HARD

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

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The value of $E_{1}^{o}$ is

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

According to the expression $ΔG ° = - nFE °$ , the cell reaction is spontaneous when

(Notations and symbols carry their usual meanings)

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

For a cell involving one electron

E_{c e l l}^{⊝} = 0.59 V

298 K

, the equilibrium constant for the cell reaction is:

[G i v e n t h a t \frac{2.303 R T}{F} = 0.059 V a t T = 298 K]

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

Given

E_{{Mn}^{+ 7} | {Mn}^{+ 2}}^{\circ} = 1.5 V

and

E_{{Mn}^{+ 4} | {Mn}^{+ 2}}^{\circ} = 1.2 V

, then

E_{{Mn}^{+ 7} / {Mn}^{+ 4}}^{\circ}

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

The emf of the cell Cd

∣ {CdCl}_{2}

(solution) (

1 atm

)

| AgCl (s) | Ag

0.675

25 ° C

. The temperature coefficient of the cell is

- 65 \times 10^{- 4} V {degree}^{- 1}

. Find the change in heat content (kJ

{mol}^{- 1}

) and entropy

(V \deg^{- 1})

for the electrochemical reaction that occurs when

1 F

of electricity is drawn for it

EASY

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

What is the standard reduction potential

(E^{o})

for

{Fe}^{3 +} \to Fe ?

Given that:

{Fe}^{2 +} + 2 e^{-} \to Fe; E_{{Fe}^{2 +} / Fe}^{o} = - 0 .47 V

{Fe}^{3 +} + e^{-} \to {Fe}^{2 +}; E_{{Fe}^{3 +} / {Fe}^{2 +}}^{o} = + 0 .77 V

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

For a cell reaction involving two-electron changes,

E_{cell}^{\circ} = 0.3 V

25 ° C

. The equilibrium constant of the reaction is

EASY

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

If the

E_{c e l l}^{o}

for a given reaction has a negative value, which of the following gives the correct relationship for the values of

∆ G^{o}

and

K_{e q}

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

The standard electrode potential for Daniel cell is

1.1

volt. What is the standard Gibbs energy for the reaction?

EASY

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R:

Assertion A: In equation $∆_{r} G = - {nFE}_{cell}$ value of $∆_{r} G$ depends on $n$ .
Reason R: $E_{cell}$ is an intensive property and $∆_{r} G$ is an extensive property.

In the light of the above statements, choose the correct answer from the options given below:

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

$H_{2_{(g)}} + 2 {AgCl}_{(s)} ⇄ 2 {Ag}_{(s)} + 2 {HCl}_{(aq)}$

$E_{cell}^{°}$ at $25 ° C$ for the cell is $0.22 V .$ The equilibrium constant at $25 ° C$ is

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

For a reaction,

A + B^{2 +} ⟶ B + A^{2 +}

, at

25^{0} C E^{0} = 0.2955 V

. The value of

K_{eq}

EASY

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

The standard emf of a galvanic cell involving

2

moles of electrons in its redox reaction is

0.59 V

. The equilibrium constant for the redox reaction of the cell is:

HARD

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

The standard electrode potential $E^{o}$ and its temperature coefficient $(\frac{dE}{dT})$ for a cell are $2 V$ and $- 5 {\times10}^{- 4} V K^{- 1}$ at $300 K$ , respectively. The reaction is $Zn (s) + {Cu}^{2 +} (aq) \to {Zn}^{2 +} (aq) + Cu (s)$ . The standard reaction enthalpy $(Δ_{r} H^{-})$ at $300 K$ in $m o l^{- 1}$ is

$[$ Use $R = 8 J K^{- 1} {mol}^{- 1}$ and $F =96,500 C {mol}^{- 1}]$

The temperature coefficient of the emf i.e., dEdt=–0.00065 VK–1 for the cell Cd|CdCl21M||AgCls|Ag at 25°C. Calculate the entropy changes ΔS at 298 K for the cell reaction Cd+2AgCl→Cd2++2Cl–+2Ag .

Important Questions on Electrochemistry

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The temperature coefficient of the emf i.e., $\frac{dE}{dt} = - 0 .00065 {VK}^{- 1}$ for the cell $C d | C d C l_{2} (1 M) | | A g C l (s) | A g$ at $25 ° C$ . Calculate the entropy changes $ΔS at 298 K$ for the cell reaction $Cd + 2 AgCl \to {Cd}^{2 +} + 2 {Cl}^{-} + 2 Ag$ .