Which of the following statement is/are wrong?

Options

A. At equilibrium, concentrations of reactants and products become constant because the reaction stops.
B. Addition of catalyst speeds up the forward reaction more than the backward reaction.
C. Equilibrium constant of an exothermic reaction decreases with increase of temperature.
D. `K_(p)` is always greater than K.

Answer

To determine which statements are wrong regarding chemical equilibrium, let's analyze each option step by step:

### Step 1: Analyze the First Statement
**Statement:** "At equilibrium, concentrations of the reactants and products become constant because the reaction stops."

**Analysis:**
- The first part of the statement is correct; at equilibrium, the concentrations of reactants and products remain constant.
- However, the reason provided is incorrect. The reaction does not stop; it continues in both the forward and backward directions at equal rates. Therefore, this statement is **wrong**.

### Step 2: Analyze the Second Statement
**Statement:** "Addition of a catalyst speeds up the forward reaction more than the backward reaction."

**Analysis:**
- This statement is misleading. A catalyst speeds up both the forward and backward reactions equally. It does not favor one over the other. Hence, this statement is also **wrong**.

### Step 3: Analyze the Third Statement
**Statement:** "Equilibrium constant of an exothermic reaction decreases with increase of temperature."

**Analysis:**
- This statement is true. For an exothermic reaction, increasing the temperature shifts the equilibrium position to favor the reactants, which results in a decrease in the equilibrium constant (K). Thus, this statement is **correct**.

### Step 4: Analyze the Fourth Statement
**Statement:** "Kp is always greater than Kc."

**Analysis:**
- This statement is incorrect. The relationship between Kp and Kc depends on the change in the number of moles of gas during the reaction (stoichiometry). Kp can be equal to, greater than, or less than Kc depending on the specific reaction. Therefore, this statement is **wrong**.

### Conclusion
Based on the analysis, the wrong statements are:
1. The first statement is wrong.
2. The second statement is wrong.
3. The fourth statement is wrong.

Thus, the answer to the question is that the wrong statements are options 1, 2, and 4.

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