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

The effect of addition of helium gas to the following reaction in equilibrium state at constant volume, is : PCI 5 ( g ) ⇌ PCl 3 ( g ) + Cl 2 ( g )

addition of helium will not affect the equilibrium.

the equilibrium will shift in the forward direction and more of Cl 2 and PCl 3 gases will be produced.

the equilibrium will go backward due to suppression of dissociation of PCl 5 .

helium will deactivate PCl 5 and reaction will stop.

EASY

JEE Main

IMPORTANT

Earn 100

Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of pH 6. If ionization constant of HA is $10^{- 5}$ , the ratio of salt to acid concentration in the buffer solution will be:

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Important Questions on Equilibrium

HARD

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 5 - Equilibrium>JEE Main - 7th January 2020 Shift 2>Q 30

3 g

of acetic acid is added to

250 m L

0.1 M H C l

and the solution made up to

500 m L

. To

20 m L

of this solution

\frac{1}{2} m L

5 M N a O H

is added. The

p H

of the solution is ________
[Given:

p K a

of acetic acid

= 4.75,

molar mass of acetic acid

60 g / m o l, \log 3 = 0.4771

, Neglect any changes in volume]

HARD

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 5 - Equilibrium>JEE Main - 7th January 2020 Shift 1>Q 31

Two solutions,

A

and

B,

each of

100 L

was made by dissolving

4 g

N a O H

and

9.8 g

H_{2} S O_{4}

in water, respectively. The

p H

of the resultant solution obtained from mixing

40 L

of solution

A

and

10 L

of solution

B

is ____________.

(\log 2 = 0.3)

MEDIUM

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 5 - Equilibrium>JEE Main - 7th April 2013>Q 32

How many litres of water must be added to

1

litre of aqueous solution of

HCl

with a pH of

1

to create an aqueous solution with pH of

2

EASY

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 5 - Equilibrium>JEE Main - 6th April 2014>Q 33

For the reaction

{SO}_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ {SO}_{3} (g)

, if

K_{P} = K_{C} {(RT)}^{x}

where the symbols have usual meaning then the value of

x

is:
(assuming ideality)

MEDIUM

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 5 - Equilibrium>JEE Main - 6 September 2020 Shift 2>Q 34

The value of $K_{c} us 64 at 800 K$ for the reaction

$N_{2} (g) + 3 H_{2} (g) \to 2 {NH}_{3} (g)$

The value of $K_{c}$ for the following reaction is :

${NH}_{3} (g) \to \frac{1}{2} N_{2} (g) + \frac{3}{2} H_{2} (g)$

EASY

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 5 - Equilibrium>JEE Main - 6 September 2020 Shift 2>Q 35

If the solubility product of ${AB}_{2}$ is $3.20 \times 10^{- 11} M^{3}$ , then the solubility of ${AB}_{2}$ in pure water is _______ $\times 10^{- 4} mol L^{- 1}$

[Assuming that neither kind of ion reacts with water]

EASY

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 5 - Equilibrium>JEE Main - 6 September 2020 Shift 1>Q 36

Arrange the following solutions in the decreasing order of pOH :
(A)

0.01 MHCl

(B)

0.01 MNaOH

(C)

0.01 {MCH}_{3} COONa

(D)

0.01 MNaCl

MEDIUM

JEE Main

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 5 - Equilibrium>JEE Main - 6 September 2020 Shift 1>Q 37

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 $R = 8.314 {JK}^{- 1} {mol}^{- 1}$ ]

Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of pH 6. If ionization constant of HA is 10-5, the ratio of salt to acid concentration in the buffer solution will be:

Important Questions on Equilibrium

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Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of pH 6. If ionization constant of HA is $10^{- 5}$ , the ratio of salt to acid concentration in the buffer solution will be: