If the value of an equilibrium constant for a particular reaction is 1.6 × 10 12 , then at equilibrium the system will contain:

Similar amounts of reactants and products

For the reaction: 2 NO 2 g ⇌ 2 NO g + O 2 g , K c = 1 .8 × 10 - 6 at 184 o C , R = 0 .0831 J / molK When K p and K c are compared at 184 o C. It is found that

Whether K p is greater than, less than or equal to K c depends upon the total gas pressure.

In which one of the following equilibria, K p ≠ K c ?

N O 2 g + S O 2 g ⇌ N O g + S O 3 g

MEDIUM

Earn 100

$1$ mole of $N O$ and $1$ mole of $O_{3}$ are taken in a $10 L$ vessel and heated. At equilibrium, $50 %$ of $N O$ (by mass) reacts with $O_{3}$ according to the equation:
$N O_{(g)} + O_{3 (g)} ⇋ N O_{2 (g)} + O_{2 (g)}$
What will be the equilibrium constant for this reaction?

50% studentsanswered this correctly

Important Questions on Equilibrium

EASY

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

Consider the following reversible chemical reactions:

A_{2} (g) + B_{2} (g) \overset{k_{1}}{⇌} 2 A B (g)

.....(1)

6 A B (g) \overset{k_{2}}{⇌} 3 A_{2} (g) + 3 B_{2} (g)

.....(2)

The relation between

K_{1}

and

K_{2}

is:

EASY

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

If the equilibrium constant for

N_{2} (g) + O_{2} (g) ⇌ 2 N O (g)

is K, the equilibrium constant for

\frac{1}{2} N_{2} (g) + \frac{1}{2} O_{2} (g) ⇌ N O (g)

will be:

HARD

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

20 litre

container at

400 K

contains

{CO}_{2} (g)

at pressure

0.4 atm

and an excess of

SrO

(neglect the volume of solid

SrO

). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when the pressure of

{CO}_{2}

attains its maximum value, will be:

(Given that : {SrCO}_{3} (s) ⇌ SrO (s) + {CO}_{2} (g), K_{p} = 1 .6 atm)

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

The equilibrium constant

(K_{c})

of two reactions

H_{2} + I_{2} ⇌ 2 HI and N_{2} + 3 H_{2} ⇌ 2 {NH}_{3}

are

50 and 1000

, respectively. The equilibrium constant of the reaction

N_{2} + 6 HI ⇌ 2 {NH}_{3} + 3 I_{2}

is closest to:

HARD

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

What are the values of

\frac{K_{p}}{K_{c}}

for the following reactions at

300 K

respectively?

(At

300 K, RT = 24 .62 {dm}^{3} atm {mol}^{- 1}

)

N_{2} (g) + O_{2} (g) ⇌ 2 NO (g); \frac{K_{p}}{K_{c}} = x_{1}

N_{2} O_{4} (g) ⇌ 2 {NO}_{2} (g); \frac{K_{p}}{K_{c}} = x_{2}

N_{2} (g) + 3 H_{2} (g) ⇌ 2 {NH}_{3} (g); \frac{K_{p}}{K_{c}} = x_{3}

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

Consider the equilibria

(i) a n d (i i)

with equilibrium constants

K_{1} a n d K_{2}

, respectively

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

.... (i)

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

.... (ii)

K_{1} a n d K_{2}

are related as

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

For the reaction,

A ⇌ n B

the concentration of A decreases from

0.06 t o 0.03 m o l L^{- 1}

and that of B rises from

0 t o 0.06 m o l L^{- 1}

at equilibrium. The values of n and the equilibrium constant for the reaction, respectively, are

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

For the following reaction, equilibrium constant are given:

$S (s) + O_{2} (g) ⇌ S O_{2} (g); K_{1} = 10^{52}$

$2 S (s) + 3 O_{2} (g) ⇌ 2 S O_{3} (g); K_{2} = 10^{129}$

The equilibrium constant for the reaction, $2 {S O}_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)$ is:

HARD

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

5 .1 g {NH}_{4} SH

is introduced in

3 .0 L

evacuated flask at

327^{o} C

30 %

of the solid

{NH}_{4} SH

is decomposed to

{NH}_{3}

and

H_{2} S

as gases. The

K_{P}

of the reaction at

327^{o} C

(R = 0 .082 L atm {mol}^{- 1} K^{- 1}, Molar mass of S = 32 g {mol}^{- 1}, Molar mass of N = 14 g {mol}^{- 1})

EASY

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

If the value of an equilibrium constant for a particular reaction is

1.6 \times 10^{12}

, then at equilibrium the system will contain:

EASY

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

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

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

For the reaction:

2 {NO}_{2 (g)} ⇌ 2 {NO}_{(g)} + O_{2 (g)},

(K_{c} = 1 .8 \times 10^{- 6} at 184^{o} C), (R = 0 .0831 J / molK)

When

K_{p}

and

K_{c}

are compared at

184^{o} C.

It is found that

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

At a certain temperature, only 50% HI is dissociated into H₂ and I₂ at equilibrium. The equilibrium constant is :

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

The equilibrium constants of the following are:

\begin{matrix} N_{2} + 3 H_{2} ⇌ 2 {NH}_{3} & K_{1} \\ N_{2} + O_{2} ⇌ 2 NO & K_{2} \\ H_{2} + \frac{1}{2} O_{2} \to H_{2} O & K_{3} \end{matrix}

The equilibrium constant (

K

) of the reaction:

2 N H_{3} + \frac{5}{2} O_{2} \overset{K}{⇌} 2 N O + 3 H_{2} O

, will be:

HARD

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

For the following reaction, the equilibrium constant

K_{C}

298 K

1.6 \times 10^{17} .

F {e^{2 +}}_{(aq)} + {S^{2 -}}_{(aq)} ⇌ F e S_{(s)}

When equal volumes of

0.06 M F e^{2 +} (a q)

and

0.2 M S^{2 -} (a q)

solutions are mixed, the equilibrium concentration of

F {e^{2 +}}_{(aq)}

is found to be

Y \times 10^{- 17} M .

The value of

Y

is __________ (Answer should be given to the nearest integer value).

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

In the figure shown below reactant

A

(represented by square) is in equilibrium with product

B

(represented by circle). The equilibrium constant is (approx):

Question Image

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

In which one of the following equilibria,

K_{p} \neq K_{c} ?

HARD

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

Consider the equilibrium

X_{2} + Y_{2} ⇌ P

. Find the stoichiometric coefficient of the

P

using the data given in the following table:

$X_{2} / m o l L^{- 1}$	$Y_{2} / m o l L^{- 1}$	$P / m o l L^{- 1}$
$1.14 \times 10^{- 2}$	$0.12 \times 10^{- 2}$	$2.52 \times 10^{- 2}$
$0.92 \times 10^{- 2}$	$0.22 \times 10^{- 2}$	$3.08 \times 10^{- 2}$

MEDIUM

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

In a chemical reaction,

A + 2 B \overset{K}{⇌} 2 C + D

, the initial concentration of

B

was

1.5

times of the concentration of

A

, but the equilibrium concentrations of

A

and

B

were found to be equal. The equilibrium constant

(K)

for the chemical reaction is:

EASY

Chemistry>Physical Chemistry>Equilibrium>Equilibrium Constants and its Significance

A solid $XY$ kept in an evacuated sealed container undergoes decomposition to form a mixture of gases $X and Y$ at temperature $T$ .

The equilibrium pressure is $10 bar$ in this vessel. $K_{p}$ for this reaction is?

1 mole of NO and 1 mole of O3 are taken in a 10L vessel and heated. At equilibrium, 50% of NO (by mass) reacts with O3 according to the equation: NO(g)+O3(g)⇋NO2(g)+O2(g) What will be the equilibrium constant for this reaction?

Important Questions on Equilibrium

Learn and Prepare for any exam you want !

$1$ mole of $N O$ and $1$ mole of $O_{3}$ are taken in a $10 L$ vessel and heated. At equilibrium, $50 %$ of $N O$ (by mass) reacts with $O_{3}$ according to the equation:
$N O_{(g)} + O_{3 (g)} ⇋ N O_{2 (g)} + O_{2 (g)}$
What will be the equilibrium constant for this reaction?