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Relation between Kp and Kc MCQ - Practice Questions with Answers

Relation between Kp and Kc MCQ - Practice Questions with Answers

Edited By admin | Updated on Sep 25, 2023 25:23 PM | #NEET

Quick Facts

Relation between Kp and Kc is considered one the most difficult concept.
47 Questions around this concept.

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For the reaction, $\mathrm{CO_{(g)}+Cl_{2(g)}\rightleftharpoons COCl_{2(g)}}$ the value of $\mathrm {\frac{K_{p}}{K_{c} }}$ is equal to

$\mathrm{\frac{1}{RT}}$

Correct Answer

Wrong Answer

$\mathrm{RT}$

Correct Answer

Wrong Answer

$\mathrm{\sqrt{RT}}$

Correct Answer

Wrong Answer

$1.0$

Correct Answer

Wrong Answer

View Solution

For the reaction, $\mathrm{SO_{2(g)}+\frac{1}{2}O_{2(g)}\rightleftharpoons SO_{3(g)}}$ if $\mathrm{K_P=K_C(RT)^x}$ where the symbols have usual meaning then the value of x is

$-1$

Correct Answer

Wrong Answer

$-\\frac{1}{2}$

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Wrong Answer

$\\frac{1}{2}$

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Wrong Answer

$1$

Correct Answer

Wrong Answer

View Solution

Change in volume of the system does not alter the number of moles in which of the following equilibria?

$N_{2(g)}+O_{2(g)}\rightleftharpoons 2NO_{(g)}\; \; \;$

Correct Answer

Wrong Answer

$PC1_{5(g)}\rightleftharpoons PC1_{3(g)}+C1_{2(g)}\; \; \;$

Correct Answer

Wrong Answer

$N_{2(g)}+3H_{2(g)}\rightleftharpoons 2NH_{3(g)}\; \; \;$

Correct Answer

Wrong Answer

$SO_{2}C1_{2(g)}\rightleftharpoons SO_{2(g)}+C1_{2(g)}$

Correct Answer

Wrong Answer

View Solution

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In which of the following reactions, increase in the volume at constant temperature does not affect the number of moles at equilibrium ?

$2NH_{3}\rightarrow N_{2}+3H_{2}\; \; \;$

Correct Answer

Wrong Answer

$C_{(g)}+(1/2)O_{2(g)}\rightarrow CO_{(g)}\; \; \;$

Correct Answer

Wrong Answer

$H_{2(g)}+O_{2(g)}\rightarrow H_{2}O_{2(g)}\; \; \;$

Correct Answer

Wrong Answer

$none\; of \; these.$

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View Solution

In which of the following equilibrium $K_c$ and $K_p$ are not equal?

$2 N O_{(g)} \rightleftharpoons N_{2(g)}+O_{2(g)}$

Correct Answer

Wrong Answer

$S O_{2(g)}+N O_{2(G)} \rightleftharpoons S O_{3(g)}+N O_{(g)}$

Correct Answer

Wrong Answer

$H_{2(g)}+I_{2(g)} \rightleftharpoons 2 H I_{(g)}$

Correct Answer

Wrong Answer

$2 C_{(s)}+O_{2(g)} \rightleftharpoons 2 \mathrm{CO}_{2(g)}$

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View Solution

The equilibrium constants of the following are:

$\begin{aligned} & \mathrm{N}_2+3 \mathrm{H}_2 \rightleftharpoons 2 \mathrm{NH}_3 \quad \mathrm{~K}_1 \\ & \mathrm{~N}_2+\mathrm{O}_2 \rightleftharpoons 2 \mathrm{NO} \quad \mathrm{K}_2 \\ & \mathrm{H}_2+\frac{1}{2} \mathrm{O}_2 \rightarrow \mathrm{H}_2 \mathrm{O} \quad \mathrm{K}_3\end{aligned}$

The equilibrium constant (K) of the reaction:

$2 \mathrm{NH}_3+\frac{5}{2} \mathrm{O}_2 \stackrel{\mathrm{~K}}{=} 2 \mathrm{NO}+3 \mathrm{H}_2 \mathrm{O}$

$\frac{K_1 K_3^3}{K_2}$

Correct Answer

Wrong Answer

$\frac{K_2 K_3^3}{K_1}$

Correct Answer

Wrong Answer

$\frac{K_2 K_3}{K_1}$

Correct Answer

Wrong Answer

$\frac{K_3 K_2^3}{K_1}$

Correct Answer

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View Solution

If the equilibrium constant for

$N_{2}(g) +O_{2}(g)\rightleftharpoons 2NO(g)\ is\ K,$

the equilibrium constant for

$\frac{1}{2}N_{2} (g) +\frac{1}{2} O_{2}(g)\rightleftharpoons NO(g)$

will be:

$K^\frac{1}{2}$

Correct Answer

Wrong Answer

$\frac{1}{2} K$

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Wrong Answer

Correct Answer

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$K^{2}$

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View Solution

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What is the equilibrium expression for the reaction

$P_{4(s)}+5O_{2(g)}\rightleftharpoons P_{4}O_{10(s)}?$

$K_{c}= \frac{\left [ P_{4}O_{10} \right ]}{\left [ P_{4} \right ]\left [ O_{2} \right ]^{5}}$

Correct Answer

Wrong Answer

$K_{c}= \frac{\left [ P_{4}O_{10} \right ]}{5\left [ P_{4} \right ]\left [ O_{2} \right ]}$

Correct Answer

Wrong Answer

$K_{c}= \left [ O_{2} \right ]^{5}$

Correct Answer

Wrong Answer

$K_{c}=\frac{1}{ \left [ O_{2} \right ]^{5}}$

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Wrong Answer

View Solution

Concepts Covered - 2

Relation between Kp and Kc

Relation between K_p and K_c

The reaction we have:

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The equilibrium constant K_c for this reaction is given as:

For the reaction:

The equilibrium constant K_p is given as:

As we know:

PV = nRT

P = (n/V)RT

Also, n/V = C

Thus, P = CRT

Therefore, 𝚫n = (n₃ + n₄) - (n₁ + n₂)]

Hence, K_p = K_c(RT)𝚫n

Expressions of K_c and K_p for some reactions

Evaluation of K_c and K_p for HI formation

For the reaction:

Initially: a mole b mole 0 mole

At equil: (a - X) (b - X) 2X moles

Thus, according to the equilibrium constant equation we have:

Similarly, for Kp we have;

Partial pressure of individual species are given as follows:

On substituting these values in the above equation, we get:

Evaluation of K_c and K_p for PCl₅ dissociation

Similarly for PCl₅ dissociation reaction we have:

Characteristics of Equilibrium Constant

The equilibrium constant has the following characteristics:

The value of the equilibrium constant for a particular reaction is always constant depending only upon the temperature of the reaction and is independent of the concentrations of the reactants with which we start of the direction from which the equilibrium is approached.
If the reaction is reversed. The value of the equilibrium constant is inversed.
If the equation is divided by 2, the equilibrium constant for the new equation is the square root of K, i.e .
If the equation is multiplied by 2, the equilibrium constant for the new equation is the square of K, i.e K².
If the equation is written in two steps, then K = K₁ x K₂.
The magnitude of the equilibrium constant gives an idea of the relative amounts of reactants and the products.
The value of the equilibrium constant is not affected by the addition of a catalyst to the reaction.