Statement -1: `DeltaH` of a reaction is independent of temperature.
and Statement -2: `DeltaH^(@)` of a reacction `=sum H^(@) ("products") - sum H^(@)("reactants")`

Options

A. Statement -1 is true, Statement -2 is true, Statement -2 is correct explanation for statement -4
B. Statement -1 is true, Statement-2 is True, Statement-2 is not a correct explanation for Statement -4
C. Statement-1 is true, Statement -2 is False.
D. Statement -1 is False, Statement -2 is True.

Answer

To solve the question, we need to evaluate the two statements provided:

**Statement 1**: ΔH of a reaction is independent of temperature.
**Statement 2**: ΔH° of a reaction = ΣH° (products) - ΣH° (reactants).

### Step-by-Step Solution:

1. **Evaluate Statement 1**:
- The change in enthalpy (ΔH) of a reaction is not independent of temperature.
- Enthalpy is defined as the total heat content of a system, and it can change with temperature.
- The relationship can be expressed as ΔH = Cp * ΔT, where Cp is the molar heat capacity at constant pressure and ΔT is the change in temperature.
- Therefore, as temperature changes, ΔH will also change.
- **Conclusion**: Statement 1 is **incorrect**.

2. **Evaluate Statement 2**:
- The change in standard enthalpy (ΔH°) for a reaction is calculated using the formula:
ΔH° = ΣH° (products) - ΣH° (reactants).
- This formula is derived from the definition of enthalpy change, which is the difference between the enthalpy of products and the enthalpy of reactants.
- This is a fundamental principle in thermochemistry.
- **Conclusion**: Statement 2 is **correct**.

3. **Final Conclusion**:
- Since Statement 1 is incorrect and Statement 2 is correct, the overall conclusion is that Statement 1 is false and Statement 2 is true.
- Therefore, the correct answer is option **D**: Statement 1 is false, Statement 2 is true.