The variation of equilibrium constant with temperature is given below : Temperature EquilibriumConstant T 1 = 25 ° C K 1 = 10 T 2 = 100 ° C K 2 = 100 The values of ΔH ° , ΔG ° at T 1 and Δ G ° at T 2 (in kJ mol - 1 ) respectively, are close to [use R = 8 . 314 JK - 1 mol - 1 ]

28 . 4 , - 5 . 71 and - 14 . 29

0 . 64 , - 5 . 71 and - 14 . 29

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What is the ${logK}_{eq}$ of the following reaction?

$ΔG ° = - 0.10 kJ {mol}^{- 1}$

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Important Questions on Equilibrium

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Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

If the value of

Δ G °

for the equilibrium reaction at

300 K

57.44 kJ {mol}^{- 1}

, the equilibrium constant

K_{c}

is:

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Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

Consider an electrochemical cell:

A (s) |A^{n +} (aq, 2 M)| |B^{2 n +} (aq, 1 M)| B (s)

. The value of

{ΔH}^{o}

for the cell reaction is twice that of

{ΔG}^{o}

300 K .

If the emf of the cell is zero, the magnitude of

Δ S^{o}

(in {JK}^{- 1} {mol}^{- 1})

of the cell reaction per mole of

B

formed at

300 K

is ____

{Jmol}^{- 1} K^{- 1}

. (Give answer after rounding off to the nearest integer value.)
(Given: R

= 8.3 {JK}^{- 1} {mol}^{- 1} .

H, S

and

G

are enthalpy, entropy and Gibbs energy, respectively.)

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

298 K

, the equilibrium constant of the process

1.5 O_{2 (g)} ⇌ O_{3 (g)}

3 \times 10^{- 29}

. Standard free energy change (in

kJ {mol}^{- 1}

) of the process is approximately

(R = 8.314 J {mol}^{- 1} K^{- 1}; \log 3 = 0.47)

HARD

Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

The gas phase reaction

$2 A (g) ⇌ A_{2} (g)$

at $400 K$ has $Δ G^{o} = + 25.2 kJ {mol}^{- 1}$ .

The equilibrium constant $K_{C}$ for this reaction is ___ $\times 10^{- 2}$ . (Round off to the Nearest integer)

Use : $R = 8.3 J {mol}^{- 1} K^{- 1}, \ln 10 = 2.3 \log_{10} 2 = 0.30, 1 atm = 1 bar$

antilog $(- 0.3) = 0.501$

EASY

Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

The incorrect match in the following is:

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Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

For the reaction

A_{(g)} \to B_{(g)}

, the value of the equilibrium constant at

300 K

and

1 atm

is equal to

100.0 .

The value of

{ΔG}^{o}

for the reaction at

300 K

and

1 atm

{Jmol}^{- 1}

- x R,

where

x

is (Rounded off to the nearest integer)

(R = 8.31 J {mol}^{- 1} K^{- 1} and \ln 10 = 2.3)

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Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

If the value of

K_{p}

for the reaction

\frac{1}{2} N_{2} + \frac{3}{2} H_{2} ⇌ 2 {NH}_{3}

is found to be

100 atm

, calculate

ΔG °

298 K

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Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

Which of the following options will be correct for the stage of half completion of the reaction

A ⇌ B

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Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

The variation of equilibrium constant with temperature is given below :

$\begin{matrix} Temperature & EquilibriumConstant \\ T_{1} = 25 ° C & K_{1} = 10 \\ T_{2} = 100 ° C & K_{2} = 100 \end{matrix}$

The values of $ΔH °, ΔG °$ at $T_{1}$ and $Δ G °$ at $T_{2}$ (in $kJ {mol}^{- 1}$ ) respectively, are close to [use $R = 8.314 {JK}^{- 1} {mol}^{- 1}$ ]

EASY

Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

Hydrolysis of sucrose is given by the following reaction.
Sucrose

+ H_{2} O ⇌

Glucose

+

Fructose
If the equilibrium constant

(K_{C})

2 \times 10^{13}

300 K

, the value of

Δ_{r} G^{⊖}

at the same temperature will be:

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Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

At 320 K, a gas

A_{2}

is 20 % dissociated to

A (g)

. The standard Gibbs free energy change at

320 K a n d 1 a t m i n J m o l^{- 1}

is approximately:

(R = 8 .314 {JK}^{- 1} {mol}^{- 1}; \ln 2 = 0 .693; \ln 3 = 1 .098)

HARD

Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

The standard Gibbs energy change at 300 K for the reaction

2 A ⇌ B + C

is 2494.2 J. At a given time, the composition of the reaction mixture is

[A] = \frac{1}{2}, [B] = 2

and

[C] = \frac{1}{2}

. The reaction proceeds in the:

[R = 8.314 J / K - m o l, e = 2.718]

{Given antilog (-0.44)=0.36}

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

The incorrect expression among the following is :

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Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

For the equilibrium, $H_{2} O (l) ⇌ H_{2} O (v),$ which of the following is correct?

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Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

60 {}^{\circ}C, 50 %

N_{2} O_{4} (g)

is dissociated to

{NO}_{2} (g)

. What is the approximate standard Gibbs free energy change at

60 {}^{\circ}C

and

1 atm

pressure for this process?

(R = 8.314 J K^{- 1} {mol}^{- 1})

HARD

Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

The standard free energy change $(ΔG °)$ for $50 %$ dissociation of $N_{2} O_{4}$ into ${NO}_{2}$ at $27 ° C$ and $1 atm$ pressure is $- x J {mol}^{- 1}$ . The value of $x$ is $- . . . . . J$ . (Nearest Integer)

[Given : $R = 8.31 J K^{- 1} {mol}^{- 1}, \log 1.33 = 0.1239 \ln 10 = 2.3$ ]

HARD

Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

$2 O_{3} (g) ⇌ 3 O_{2} (g)$

At $300 K$ , ozone is fifty percent dissociated. The standard free energy change at this temperature and $1 atm$ pressure is $(-) . . . . . . J {mol}^{- 1}$ . (Nearest integer)

[Given: $\ln 1.35 = 0.3$ and $R = 8.3 J K^{- 1} {mol}^{- 1}$ ]

HARD

Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

Consider the reaction $A ⇌ B$ at $1000 K$ . At the time $t^{'}$ , the temperature of the system was increased to $2000 K$ and the system was allowed to reach equilibrium. Throughout this experiment the partial pressure of $A$ was maintained at $1$ bar. Given below is the plot of the partial pressure of $B$ with time. What is the ratio of the standard Gibbs energy of the reaction at $1000 K$ to that at $2000 K$ ?

Question Image

Give your answer by multiplying with 100 and rounding off to nearest integer.

EASY

Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

Of the following reactions

(i)

A ⇌ B, ∆ G^{o} = 250 kJ {mol}^{- 1}

(ii)

D ⇌ E, ∆ G^{o} = - 100 kJ {mol}^{- 1}

(iii)

F ⇌ G, ∆ G^{o} = - 150 kJ {mol}^{- 1}

(iv)

M ⇌ N, ∆ G^{o} = 150 kJ {mol}^{- 1}

The reaction with the largest equilibrium constant is

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Relationship between Equilibrium Constant (K), Reaction Quotient (Q) and Gibbs Energy (G)

Which of the following statements is correct for a reversible process in the state of equilibrium?

What is the logKeq of the following reaction? ΔG°=-0.10 kJ mol-1

Important Questions on Equilibrium

Learn and Prepare for any exam you want !

What is the ${logK}_{eq}$ of the following reaction?

$ΔG ° = - 0.10 kJ {mol}^{- 1}$