For a reaction 2 A ⇌ B + C , K c is 2 × 10 - 3 . At a given time, the reaction mixture has [ A ] = [ B ] = [ C ] = 3 × 10 - 4 M . Which of the following options is correct?

The reaction proceeds to the left

The reaction proceeds to the right

HARD

Earn 100

The following reaction takes place at $127 ° C$ and $5 L$ vessel,

${SO}_{2} {Cl}_{2} (g) ⇋ {SO}_{2} (g) + {Cl}_{2} (g) K_{p} = 1 atm$

$a)$ If initially only ${SO}_{2} {Cl}_{2} (g)$ gas was present at $2 atm$ , then calculate equilibrium pressure of each gas

$b)$ If after reaching equilibrium volume of the vessel is doubled, then what would be the partial pressure of each gas at new equilibrium.

$c)$ Calculate the vapour density at new equilibrium

Important Questions on Equilibrium

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

The reaction quotient $(Q)$ for the reduction of $p_{{SO}_{2}} = 1 atm & p_{{Cl}_{2}} = 1 atm$ to $H_{2} O$ in acid solution,
$O_{2} (g) + 4 H^{+} (aq) + 4 e^{-} ⟶ 2 H_{2} O (l)$ is,
[where, $α_{H^{+}} =$ activity of $H^{+}, p_{O_{2}} =$ pressure of $O_{2}$ when it is present in the reaction, $p ° =$ pressure of $O_{2}$ at standard state].

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

An equilibrium mixture at

300 K

contains

N_{2} O_{4}

and

{NO}_{2}

0.28

and

1.1 atm

pressure, respectively. If the volume of the container is doubled, the new equilibrium pressure of these two gases are respectively.

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

At $T (K)$ , for the gaseous reaction
$2 A ⇌ B + C, K_{C}$ is $2 \times 10^{- 3}$

at a given time the composition of reaction mixture is $[A] = [B] = [C] = 3.0 \times 10^{- 4} M,$ the state of the reaction is

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

Which among the following denotes the correct relationship between

K_{p}

and

K_{c}

for the reaction

2 A_{(g)} ⇌ B_{(g)} + C_{(g)}

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

The equilibrium constant

K_{c}

of the reaction,

2 A ⇌ B + C is 0 .5 at 25^{o}

and

1 atm

. The reaction will proceed in the backward direction when concentrations

[A], [B] and [C]

are, respectively -

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

What will be the expression of

Kp

for the given reaction if the total pressure inside the vessel is

P

and degree of dissociation of the reactant is

a ?

The reaction:

N_{2} O_{4} = 2 {NO}_{2}

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

For the following reaction, $K_{c} = 2 \times 10^{- 3}$

$2 A ⇌ B + C$

Identify the correct statement for the reaction when $[A] = [B] = [C] = 3 \times 10^{- 4} M$

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

The decomposition of dinitrogen tetroxide at

300 K

and

1.0

atm pressure is

20 %

. At equilibrium, the partial pressure (in atm) of a nitrogen peroxide is

HARD

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

For the decomposition of the compound, represented as

{NH}_{2} {COONH}_{4} (s) ⇌ 2 {NH}_{3} (g) + {CO}_{2} (g)

the

K_{p} = 2 .9 \times 10^{- 5} {atm}^{3}

. If the reaction is started with 1 mole of the compound, the total pressure at equilibrium would be :

HARD

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

An aqueous solution contains

0.10 M H_{2} S

and

0.20 M HCl

. If the equilibrium constant for the formation of

{HS}^{-}

from

H_{2} S

1.0 \times 10^{- 7}

and that of

S^{2 -}

from

{HS}^{-}

ions is

1.2 \times 10^{- 13}

, then, the concentration of

S^{2 -}

ions in the aqueous solution is:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

For a reaction

2 A ⇌ B + C, K_{c}

2 \times 10^{- 3} .

At a given time, the reaction mixture has

[A] = [B] = [C] = 3 \times 10^{- 4} M .

Which of the following options is correct?

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

The percentage of pyridine

(C_{5} H_{5} N)

that forms pyridinium ion

(C_{5} H_{5} N^{+} H)

in a

0.10 M

aqueous pyridine solution

(K_{b} for C_{5} H_{5} N = 1 .7 \times 10^{- 9})

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

The value of the reactant quotient

(\emptyset)

for the cell is

Zn (s) / {Zn}^{2 +} (0.01 M) ‖ {Cu}^{2 +} (1.25 M) / Cu (s)

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

The equilibrium constant for the reaction

A (s) ⇌ M (s) + \frac{1}{2} O_{2} (g)

K_{p} = 4 .

At equilibrium, the partial pressure of

O_{2}

is _____ atm. (Round off to the nearest integer)

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

For the reaction

{H_{2}}_{(g)} + {Br}_{2}_{(g)} ⇌ 2 {HBr}_{(g)},

the concentrations of

H_{2}, {Br}_{2}

and

HBr

at equilibrium are found to be

3.5 \times 10^{- 3} M, 4.7 \times 10^{- 3} M

and

3.3 \times 10^{- 3} M .

If the reaction takes place in a sealed vessel at

600 ° C,

then find the value of its

K_{c}

HARD

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

(i) $X (g) ⇌ Y (g) + Z (g) K_{p 1} = 3$

(ii) $A (g) ⇌ 2 B (g) K_{p 2} = 1$

If the degree of dissociation and initial concentration of both the reactants $X (g)$ and $A (g)$ are equal, then the ratio of the total pressure at equilibrium $(\frac{p_{1}}{p_{2}})$ is equal to $x : 1$ . The value of $x$ is (Nearest integer)

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

Some of the reactions and their equilibrium constants

K_{c}

are given. Choose the reaction which proceeds rarely at the given temperature.

HARD

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

The equilibrium constant at

298 K

for a reaction

A + B ⇌ C + D

100

. If the initial concentration of all the four species were

1 M

each, then the equilibrium concentration of

D

(in mol

L^{- 1}

) will be:

EASY

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

The equilibrium constants for the reactions

X ⇋ 2 Y

and

Z ⇋ P + Q

are

K_{1}

and

K_{2},

respectively. If the initial concentrations and the degree of dissociation of

X

and

Z

are the same, the ratio

K_{1} / K_{2}

HARD

Chemistry>Physical Chemistry>Equilibrium>Law of Chemical Equilibrium and Equilibrium Constants

Gaseous

N_{2} O_{4}

dissociates into gaseous

N O_{2}

according to the reaction

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g)

300 K

and

1 atm

pressure, the degree of dissociation of

N_{2} O_{4}

0.2

. If one mole of

N_{2} O_{4}

gas is contained in a vessel, then the density of the equilibrium mixture is

:

Important Questions on Equilibrium

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