For a reaction `A(g) hArr B(g)+C(g)`. `K_(p)` at `400^(@)C` is `1.5xx10^(-4)` and `K_(p)` at `600^(@)C` is `6xx10^(-3)`. Which statement is incorrect?

Options

A. The reaction is exothermic
B. Increase in temperature increases the formation of B
C. Increase in pressure increases the formation of A
D. Decrease in temperature and increase in pressure shift the equilibrium towards left

Explanation

To determine which statement is incorrect regarding the equilibrium reaction \( A(g) \rightleftharpoons B(g) + C(g) \) with given equilibrium constants \( K_p \) at two different temperatures, we can follow these steps:

### Step 1: Understand the given data
We have:
- \( K_{p1} \) at \( 400^\circ C = 1.5 \times 10^{-4} \)
- \( K_{p2} \) at \( 600^\circ C = 6 \times 10^{-3} \)

### Step 2: Analyze the effect of temperature on \( K_p \)
Since \( K_p \) increases with temperature (from \( 1.5 \times 10^{-4} \) to \( 6 \times 10^{-3} \)), this suggests that the reaction is endothermic. According to Le Chatelier's principle, if the temperature of an endothermic reaction is increased, the equilibrium will shift to favor the formation of products.

### Step 3: Determine the implications of the reaction being endothermic
For an endothermic reaction:
- Increasing temperature shifts the equilibrium to the right (towards products).
- Decreasing temperature shifts the equilibrium to the left (towards reactants).

### Step 4: Analyze the effect of pressure on the equilibrium
The reaction has:
- 1 mole of \( A \) (reactant)
- 2 moles of \( B \) and \( C \) (products)

When pressure is increased, the equilibrium shifts towards the side with fewer moles of gas. In this case, that means the equilibrium will shift to the left (towards \( A \)) since there is 1 mole of \( A \) compared to 2 moles of products.

### Step 5: Evaluate the provided statements
1. **Statement about the reaction being exothermic**: This is incorrect because we established that the reaction is endothermic.
2. **Statement about the formation of \( B \) increasing with temperature**: This is correct.
3. **Statement about increasing pressure increasing the formation of \( A \)**: This is also correct, as increasing pressure shifts the equilibrium towards the side with fewer moles (which is \( A \)).
4. **Statement about decreasing temperature and increasing pressure shifting equilibrium to the left**: This is correct; decreasing temperature shifts left and increasing pressure also shifts left.

### Conclusion
The incorrect statement is the first one, which claims that the reaction is exothermic.