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Ammonium hydrogen sulphide dissociates according to the equation $N H_{4} H S (s) ⇌ N H_{3} (g) + H_{2} S (g)$ . If the observed pressure of the mixture is $1.12$ atmosphere at $106^{0} C$ , what is the equilibrium constant $K_{p}$ of the reaction ?

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Important Questions on Electrochemistry

EASY

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

Given the standard potentials

E^{o} (\frac{C u^{2 +}}{C u})

and

E^{o} (\frac{C u^{+}}{C u})

0.340 V

and

0.522 V

respectively, the value of

E^{o} (\frac{C u^{2 +}}{C u^{+}})

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

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}

HARD

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

Question Image

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

EASY

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

The standard electrode potential of

{Zn}^{2 +} / Zn is - 0 .76 V

and that of

{Cu}^{2 +} / Cu is 0 .34 V

. The emf

(V)

and the free energy change,

(in kJ {mol}^{- 1}),

respectively, for a Daniel cell will be

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}

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

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

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

EASY

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

The standard free energy change (in J) for the reaction

3 {Fe}^{2 +} (aq) + 2 Cr (s) \to 2 {Cr}^{3 +} (aq) + 3 Fe (s)

given

E_{{Fe}^{2 +} / Fe}^{0} = - 0 .44 V and E_{{Cr}^{3 +} / Cr}^{0} = - 0 .74 V

(F = 96500 C)

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:

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________ $[F = 9.649 \times 10^{4} C {mol}^{- 1}]$

EASY

Chemistry>Physical Chemistry>Electrochemistry>Thermodynamics of Cell

The equilibrium constant of a

2

electron redox reaction at

298 K

3.8 \times 10^{- 3} .

The cell potential

E^{o} (in V)

and the free energy change

{ΔG}^{o} (in kJ {mol}^{-})

for this equilibrium respectively, are

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})

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 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

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

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

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 $F = 96500 C m o l^{- 1}$ ]

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

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 $F =96,500 C {mol}^{- 1}]$

Ammonium hydrogen sulphide dissociates according to the equation NH4HS(s)⇌NH3(g)+H2S(g). If the observed pressure of the mixture is 1.12 atmosphere at 1060C, what is the equilibrium constant Kp of the reaction ?

Important Questions on Electrochemistry

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Ammonium hydrogen sulphide dissociates according to the equation $N H_{4} H S (s) ⇌ N H_{3} (g) + H_{2} S (g)$ . If the observed pressure of the mixture is $1.12$ atmosphere at $106^{0} C$ , what is the equilibrium constant $K_{p}$ of the reaction ?