Which of the following is a wrong statement about equilibrium state ?

Options

A. Rate of forward reaction = Rate of backward reaction
B. Equilibrium is dynamic
C. Catalysts increase value of equilibrium constant
D. Free energy change is zero

Explanation

To determine which statement about equilibrium is incorrect, let’s analyze each option step by step.

### Step 1: Analyze the First Statement
**Statement:** Rate of forward reaction is equal to rate of backward reaction.

**Analysis:**
At equilibrium, the rate of the forward reaction equals the rate of the backward reaction. This is a fundamental principle of chemical equilibrium. Therefore, this statement is **correct**.

### Step 2: Analyze the Second Statement
**Statement:** Equilibrium is a dynamic process.

**Analysis:**
Equilibrium does not mean that the reactions have stopped; rather, it indicates that the rates of the forward and backward reactions are equal. This means that although the concentrations of reactants and products remain constant, the reactions are still occurring. Thus, this statement is also **correct**.

### Step 3: Analyze the Third Statement
**Statement:** Catalyst increases the value of equilibrium constant.

**Analysis:**
A catalyst speeds up the rate at which equilibrium is reached but does not change the position of equilibrium or the equilibrium constant itself. The equilibrium constant is determined by the concentrations of reactants and products at equilibrium and is not affected by the presence of a catalyst. Therefore, this statement is **incorrect**.

### Step 4: Analyze the Fourth Statement
**Statement:** For equilibrium, free energy change is zero.

**Analysis:**
At equilibrium, the change in Gibbs free energy (ΔG) is indeed zero. This is a well-established concept in thermodynamics. Therefore, this statement is **correct**.

### Conclusion
The wrong statement about the equilibrium state is: **"Catalyst increases the value of equilibrium constant."**

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