Given an equilibrium reaction:
$N_{2} + 3 H_{2} ⇋ 2 N H_{3}$
In the above equilibrium system, if the pressure of the reactants at $25^{\circ} C$ is increased, then the value of $K_{c}$ will:

increase

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decrease

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remain the same

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depend on the nature of the reactants

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Solution

The correct option is C remain the same
The magnitude of the equilibrium constant is not affected by the changes in concentrations of reactants and products, pressure or volume. Thus, when the pressure of the reactants is increased, the value of the equilibrium constant $K_{c}$ remains the same.

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Given an equilibrium reaction:N2+3H2⇋2NH3 In the above equilibrium system, if the pressure of the reactants at 25∘C is increased, then the value of Kc will:

The correct option is C remain the sameThe magnitude of the equilibrium constant is not affected by the changes in concentrations of reactants and products, pressure or volume. Thus, when the pressure of the reactants is increased, the value of the equilibrium constant Kc remains the same.

Given an equilibrium reaction:
$N_{2} + 3 H_{2} ⇋ 2 N H_{3}$
In the above equilibrium system, if the pressure of the reactants at $25^{\circ} C$ is increased, then the value of $K_{c}$ will:

The correct option is C remain the same
The magnitude of the equilibrium constant is not affected by the changes in concentrations of reactants and products, pressure or volume. Thus, when the pressure of the reactants is increased, the value of the equilibrium constant $K_{c}$ remains the same.