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Equilibrium Constant - Practice Questions & MCQ
Edited By admin | Updated on Sep 18, 2023 18:35 AM | #JEE Main
Quick Facts
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Types of Equilibrium Constant is considered one of the most asked concept.
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26 Questions around this concept.
Solve by difficulty
The equilibrium constant (KC) for the reaction at temperature T is
. The value of KC for the given reaction at the same temperature is :
A vessel at 1000 K contains CO2 with a pressure of 0.5 atm. Some of the CO2 is converted into CO on the addition of graphite. If the total pressure at equilibrium is 0.8 atm, the value of K is
Kc for m1A + m2B = n1C + n2D is given by:
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The reaction quotient $(\Theta)$ for the reaction is given by:
$
\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \leftrightarrow 2 \mathrm{NH}_3 ; \quad \Theta=\frac{\left[\mathrm{NH}_3\right]^2}{\left[\mathrm{~N}_2\right]\left[H_2\right]^3}
$
The reaction will proceed from right to left if.
The values of KP1 and KP2 for the reactions ,
$\begin{aligned} & X \leftrightarrow Y+Z------1 \\ & A \leftrightarrow 2 B------2\end{aligned}$
are in the ratio 9:1 . If degree of dissociation of X and A be equal , then total pressure at equilibrium of equation 1 and 2 are in the ratio :
What range of Kc both reactants and products are equally present in mixture
Concepts Covered - 1
Types of Equilibrium Constant
It is the ratio of the rate of forward and backward reaction at a particular temperature or it is the ratio of active masses of the reactants to that of active masses of products at a particular temperature raised to their stoichiometric coefficients. It is denoted by Kc or Kp. The distinction between Keq and Kc is that the expression of Keq involves all the species (whether they are pure solids, pure liquids, gases, solvents or solutions) while the expression Kc involves only those species whose concentration is a variable (gases and solution). It means Kc is a devoid of pure components (like pure solids and pure liquids) and solvents.
Let us look at the definition of Equilibrium constant in terms of concentration and partial pressure
(1) Equilibrium constant in terms of Concentration
For a reaction:
We know that at equilibrium
The above expression gives us the value of Kc as the activity or the active mass is expressed in terms of the concentrations (c) or the molarity
(2) Equilibrium constant in terms of Partial pressure
In this case, the equilibrium constant is known as Kp. It is applicable only for gaseous systems.
For the reaction:
At equilibrium
The above expression gives us the value of KP as the activity is expressed in terms of partial pressures.
Note: This is generally used for gaseous systems or systems where gases are in equilibrium with liquids or solids
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