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Relation betw...

Relation between Kp and Kc

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Q.

The $\frac{K_{P}}{K_{C}}$ ratio will be highest in case of

$C O (g) + \frac{1}{2} O_{2} (g) ⇌ C O_{2} (g)$
$H_{2} (g) + I_{2} (g) ⇌ 2 H l (g)$
$P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g)$
$7 H_{2} (g) + 2 N O_{2} (g) ⇌ 2 N H_{3} (g) + 4 H_{2} O (g)$

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Q.

Thermal decomposition of gaseous $X_{2}$ to gaseous X at 298 K takes place according to the following equation:
$X_{2} (g) ⇌ 2 X (g)$
The standard reaction Gibbs energy, $Δ G^{o},$ of this reaction is positive. At the start of the reaction, there is one mole of $X_{2}$ and no X. As the reaction proceeds, the number of moles of X formed is given by $β,$ Thus, $β_{e q u i l i b r i u m}$ is the number of moles of X formed at equilibrium. The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally.
(Given: R = 0.083 L bar $K^{- 1} m o l^{- 1}$ )

The equilibrium constant $K_{p}$ for this reaction at 298 K, in terms of $β_{e q u i l i b r i u m},$ is

$\frac{8 β_{e q u i l i b r i u m}^{2}}{2 - β_{e q u i l i b r i u m}}$
$\frac{8 β_{e q u i l i b r i u m}^{2}}{4 - β_{e q u i l i b r i u m}^{2}}$
$\frac{4 β_{e q u i l i b r i u m}^{2}}{2 - β_{e q u i l i b r i u m}}$
$\frac{4 β_{e q u i l i b r i u m}^{2}}{4 - β_{e q u i l i b r i u m}^{2}}$

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Q. The value of

K_{p}

for the following reaction

2 H_{2} S (g) ⇌ 2 H_{2} (g) + S_{2} (g) i s 1.2 \times 10^{- 2} a t {106.5}^{o} C .

The value of

K_{C}

for this reaction is

$1.2 \times 10^{- 2}$
$< 1.2 \times 10^{- 2}$
83
$> 1.2 \times 10^{- 2}$

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Q. The relation between

K_{p}

and

K_{c}

for the following reactions.

(i) N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

(i i) 2 H_{2} O (g) ⇌ 2 H_{2} (g) + O_{2} (g)

For these two reactions;
(i)

K_{p_{1}} = K_{c} (R T)^{x}

(ii)

K_{p_{2}} = K_{c} (R T)^{y}

Find the sum (x+y).

$1$
$- 1$
$2$
$- 1.5$

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Q.

In which of the following reaction, the value of $K_{p}$ will be equal to $K_{c}$

$H_{2} + I_{2} ⇌ 2 H I$
$P C l_{5} ⇌ P C l_{3} + C l_{2}$
$2 N H_{3} ⇌ N_{2} + 3 H_{2}$
$2 S O_{2} + O_{2} ⇌ 2 S O_{3}$

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Q.

For which one of the following homogenous equilibrium equations will K_p equal K_c?

3H₂(g) + N₂ (g) ⇌ 2NH₃ (g)
PCl₅ (g) ⇌ PCl₃ (g) + Cl₂ (g)
COCl₂ (g) ⇌ CO (g) + Cl₂ (g)
H₂ (g) + I₂ (g) ⇌ 2HI (g)

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Q.

The ratio of $K_{p}$ to $K_{c}$ for the equilibrium $C O (g) + \frac{1}{2} O_{2} (g) ⇌ C O_{2} (g)$ is

1
RT
$\frac{1}{\sqrt{R T}}$
$(R T)^{\frac{1}{2}}$

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Q. For the synthesis of ammonia,

K_{p}

and

K_{c}

are related as:

$K_{p} = K_{c} (R T)^{2}$
$K_{c} = K_{p} (R T)^{- 2}$
$K_{c} = K_{p} (R T)^{2}$
$K_{p} = K_{c}$

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Q.

For a general reaction aA(g) + bB(g) $⇋$ cC(g)+ dD(g), what is the relationship between the equilibrium constants $K_{c}$ and $K_{p}$ ? [assume $Δ$ n = $μ$ = (c + d) - (a+b)

$K_{p}$ = $K_{c}$ ${(R T)}^{Δ n}$
$K_{c}$ = $K_{p}$ ${(R T)}^{- Δ n}$
$K_{p} K_{c}$ = 1
$K_{p}$ = $K_{c}$

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Q. Ammonium carbamate dissociates as:

N H_{2} C O O N H_{4} (s) ⇌ 2 N H_{3} (g) + C O_{2} (g)

In a closed vessel containing ammonium carbamate in equilibrium, ammonia is added such that the partial pressure of

N H_{3}

now equals the original total pressure. Calculate the ratio of the partial pressure of

C O_{2}

now to the original partial pressure of

C O_{2}

:

4
9
$\frac{4}{9}$
$\frac{2}{9}$

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Q. At a temperature of

1000 K

, equilibrium constant

K_{c}

for the following reaction is

100 m o l^{2} L^{- 2}

.

N_{2} (g) + 3 H_{2} (g) ⇋ 2 N H_{3} (g)

What will be the value of

K_{p}

for the reaction below?

N H_{3} (g) ⇋ \frac{1}{2} N_{2} (g) + \frac{3}{2} H_{2} (g)

0.1 atm
8.21 atm
831.4 atm
8.314 atm

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Q. The relation between

K_{p}

and

K_{c}

for the following reactions.

(i) N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

(i i) 2 H_{2} O (g) ⇌ 2 H_{2} (g) + O_{2} (g)

For these two reactions;
(i)

K_{p_{1}} = K_{c} (R T)^{x}

(ii)

K_{p_{2}} = K_{c} (R T)^{y}

Find the sum (x+y).

$1$
$- 1$
$2$
$- 1.5$

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Q. For the synthesis of ammonia,

K_{p}

and

K_{c}

are related as:

$K_{p} = K_{c} (R T)^{2}$
$K_{c} = K_{p} (R T)^{- 2}$
$K_{c} = K_{p} (R T)^{2}$
$K_{p} = K_{c}$

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Q. Ammonium carbamate dissociates as:

N H_{2} C O O N H_{4} (s) ⇌ 2 N H_{3} (g) + C O_{2} (g)

In a closed vessel containing ammonium carbamate in equilibrium, ammonia is added such that the partial pressure of

N H_{3}

now equals the original total pressure. Calculate the ratio of the partial pressure of

C O_{2}

now to the original partial pressure of

C O_{2}

:

4
9
$\frac{4}{9}$
$\frac{2}{9}$

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Q. Two solid compounds

^{'} X^{'}

and

^{'} Y^{'}

dissociates at certain temperature as follows:

X (s) ⇌ A (g) + 2 b (g) K p_{1} = 9 \times 10^{- 3} {atm}^{3}

Y (s) ⇌ 2 B (g) + C (g) K p_{2} = 4.5 \times 10^{- 3} {atm}^{3}

.
The total pressure (in atm) of gases over a mixture of

^{'} X^{'}

and

^{'} Y^{'}

is

1.5
0.45
0.6
0.9

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Q.

K_{p}

for a reaction at

25^{o} C

in 10 atm is 8.568. Then

K_{c}

for the reaction at

25^{o} C

will be:

N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)

$4.33 \times 10^{- 1} M$
$3.33 \times 10^{- 2} M$
$3.89 \times 10^{- 1} M$
none of these

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Q. At

800^{\circ}

C, the following equilibrium is established as

F_{2} (g) ⇌ 2 F (g)

The composition of equilibrium may be determined by measuring the rate of effusion of the mixture through a pin hole. It is found that at

800^{\circ}

C and 1 atm mixture effuses 1.6 times as fast as

S O_{2}

effuses under the similar conditions. (Atomic weight of F =19 amu). What is the value of

K_{p}

?

0.315 atm
0.685 atm
0.460 atm
1.490 atm

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Q.

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

is a gaseous phase equilibrium reaction taking place in a

5

litre flask at

1 a t m

. For this :

$K_{C} = K_{p}$
$K_{C} = 25 K_{p}$
$K_{p} = 25 K_{c}$
$K_{C} = 5 K_{p}$

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Q. Solid ammonium carbamate,

N H_{4} C O_{2} N H_{2} (s)

, dissociates into ammonia and carbon dioxide when it evaporates as shown by

N H_{4} C O_{2} N H_{2} (s) ⇌ 2 N H_{3} (g) + C O_{2} (g)

At

25^{\circ} C

, the total pressure of the gases in equilibrium with the solid is

0.116 atm

, if

0.1 atm

of

C O_{2}

is introduced after equilibrium is reached then:

The final pressure of $C O_{2}$ will be less than $0.1 atm$
The final pressure of $C O_{2}$ will be more than $0.1 atm$
The pressure of $N H_{3}$ will decrease due to addition of $C O_{2}$
The pressure of $N H_{3}$ will increase due to addition of $C O_{2}$

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Q.

The reaction A + 2B $⇌$ 2C + D is carried out at 298 K using only A and B initially. While mixing, the concentration of B was 1.5 times of that of A. When this system attained equilibrium, it was observed that the (new) concentrations of A and D were same. What is the value of $K_{c}$ (equilibrium constant) at 298 K?

6
4
1
$\frac{1}{64}$

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Q.

In which of the following reaction, the value of $K_{p}$ will be equal to $K_{c}$

$H_{2} + I_{2} ⇌ 2 H I$
$P C l_{5} ⇌ P C l_{3} + C l_{2}$
$2 N H_{3} ⇌ N_{2} + 3 H_{2}$
$2 S O_{2} + O_{2} ⇌ 2 S O_{3}$

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Q. The value of

K_{p}

for the following reaction

2 H_{2} S (g) ⇌ 2 H_{2} (g) + S_{2} (g) i s 1.2 \times 10^{- 2} a t {106.5}^{o} C .

The value of

K_{C}

for this reaction is

$1.2 \times 10^{- 2}$
$< 1.2 \times 10^{- 2}$
83
$> 1.2 \times 10^{- 2}$

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Q.

The ratio of $K_{p}$ to $K_{c}$ for the equilibrium $C O (g) + \frac{1}{2} O_{2} (g) ⇌ C O_{2} (g)$ is

1
RT
$\frac{1}{\sqrt{R T}}$
$(R T)^{\frac{1}{2}}$

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Q. The equilibrium constant

K_{P}

for the reaction

N_{2} O_{4} (g) ⇌ 2 N O_{2}

(g) is

4.5

.
What would be the average molar mass (in g⁄mol) of an equilibrium mixture of

N_{2} O_{4}

and

N O_{2}

formed by the dissociation of pure

N_{2} O_{4}

at a total pressure of 2 atm?

$69$
$57.5$
$85.5$
$80.5$

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Q.

K_{p}

for a reaction at

25^{o} C

in 10 atm is 8.568. Then

K_{c}

for the reaction at

25^{o} C

will be:

N_{2} (g) + 3 H_{2} (g) \to 2 N H_{3} (g)

$4.33 \times 10^{- 1} M$
$3.33 \times 10^{- 2} M$
$3.89 \times 10^{- 1} M$
none of these

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