Statement1: `PCl_(5)hArrPCl_(3)(g)+Cl_(2)(g).` Final pressure is more than the initial pressure.
Statement2: `Deltangt0,` more no. of moles on product side.

Options

A. Statement 1 is true, stetement 2 is true, statement 2 is a correct explanation for statement 1
B. Statement 1 is true, statement 2 is true, statement 2 is not a correct explanation for statement 1
C. Statement 1 is true, statement 2 is false
D. Statement 1 is false, statement 2 is true

Explanation

To analyze the statements given in the question, we will break down the chemical equilibrium reaction and the implications of the changes in pressure and moles of gas.

### Step 1: Write the balanced chemical equation
The reaction provided is:
\[ \text{PCl}_5 (g) \rightleftharpoons \text{PCl}_3 (g) + \text{Cl}_2 (g) \]

### Step 2: Identify the number of moles on each side
- On the left side (reactants), we have 1 mole of PCl5.
- On the right side (products), we have 1 mole of PCl3 and 1 mole of Cl2, which totals 2 moles.

### Step 3: Analyze the change in moles
When PCl5 dissociates into PCl3 and Cl2, the total number of moles increases from 1 mole (PCl5) to 2 moles (PCl3 + Cl2).

### Step 4: Understand the relationship between moles and pressure
According to the ideal gas law, pressure is directly proportional to the number of moles of gas when temperature and volume are constant. Therefore, if the number of moles increases, the pressure will also increase.

### Step 5: Conclusion about the statements
- **Statement 1**: "Final pressure is more than the initial pressure." This statement is **true** because the number of moles of gas increases from 1 to 2, leading to an increase in pressure.
- **Statement 2**: "Δn > 0, more no. of moles on product side." This statement is also **true** since Δn (the change in the number of moles) is indeed greater than 0 (it increases from 1 to 2).

### Final Answer
Both statements are true.

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