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

EASY

Earn 100

How will you find the direction of reaction on the basis of the value of reaction quotient $(Q_{c})$ and equilibrium constant $(K_{c})$ ?

Important Questions on Equilibrium

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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

HARD

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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:

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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>Applications of Equilibrium Constant

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}

EASY

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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}

EASY

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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)

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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.

EASY

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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}

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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 -

HARD

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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 :

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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>Applications of Equilibrium Constant

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>Applications of Equilibrium Constant

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?

EASY

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

The reaction quotient $(Q)$ for the reduction of $O_{2}$ 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>Applications of Equilibrium Constant

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>Applications of Equilibrium Constant

Some of the reactions and their equilibrium constants

K_{c}

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

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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>Applications of Equilibrium Constant

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:

EASY

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

The equilibrium constant,

K_{c} for 3 C_{2} H_{2} (g) ⇌ C_{6} H_{6} (g)

4 L^{2} {mol}^{- 2}

. If the equilibrium concentration of benzene is

0 .5 mol L^{- 1},

that of acetylene in

mol L^{- 1}

must be

HARD

Chemistry>Physical Chemistry>Equilibrium>Applications of Equilibrium Constant

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

:

How will you find the direction of reaction on the basis of the value of reaction quotient Qc and equilibrium constant Kc?

Important Questions on Equilibrium

Learn and Prepare for any exam you want !

How will you find the direction of reaction on the basis of the value of reaction quotient $(Q_{c})$ and equilibrium constant $(K_{c})$ ?