Given the hypothetical reaction $2 A + B ⇌ C + 3 D$ , the equilibrium constant for this reaction is:
I. Directly proportional to the concentration of $D^{3}$
II. Inversely proportional to the concentration of $A$
III. inversely proportional to the concentration of $C$

I, II, and III

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I and II only

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II and III only

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I only

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Solution

The correct option is C I only
Equilibrium constant of a reaction is expressed as the ratio of the concentration of the products to the concentration of the reactants, with their powers raised to their stoichiometric co-efficients in that particular reaction.
In the reaction $2 A$ $+$ $B$ $=$ $C$ $+$ $3 D$
The equilibrium constant will be written as $k$ $=$ $[C]^{1}$ $[D]^{3}$ $/$ $[A]^{2}$ $[B]^{1}$
Thus, we see that, the equilibrium constant for this reaction is directly proportional to the concentration of $D$ cubed.
Option D is the correct answer.

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Given the hypothetical reaction 2A+B⇌C+3D, the equilibrium constant for this reaction is:I. Directly proportional to the concentration of D3II. Inversely proportional to the concentration of AIII. inversely proportional to the concentration of C

Given the hypothetical reaction $2 A + B ⇌ C + 3 D$ , the equilibrium constant for this reaction is:
I. Directly proportional to the concentration of $D^{3}$
II. Inversely proportional to the concentration of $A$
III. inversely proportional to the concentration of $C$