The activation energies of the forward and backward reactions in the case of a chemical reaction are 37.5 and 51.3 kJ/mole respectively The reaction is

Options

A. Endothermic
B. Exothermic
C. Neither exothermic nor endothermic
D. Independent of temperature

Answer

To determine whether the reaction is exothermic or endothermic based on the given activation energies, we can follow these steps:

### Step 1: Identify the Activation Energies
- **Activation Energy of Forward Reaction (Ea, forward)** = 37.5 kJ/mol
- **Activation Energy of Backward Reaction (Ea, backward)** = 51.3 kJ/mol

### Step 2: Calculate the Change in Enthalpy (ΔH)
The change in enthalpy (ΔH) for the reaction can be calculated using the formula:
\[ \Delta H = E_a \text{ (backward)} - E_a \text{ (forward)} \]
Substituting the values:
\[ \Delta H = 51.3 \, \text{kJ/mol} - 37.5 \, \text{kJ/mol} \]

### Step 3: Perform the Calculation
Now, calculate the value:
\[ \Delta H = 51.3 - 37.5 = 13.8 \, \text{kJ/mol} \]

### Step 4: Determine the Nature of the Reaction
Since the value of ΔH is positive (13.8 kJ/mol), this indicates that the reaction absorbs energy. Therefore, the reaction is endothermic.

### Conclusion
The reaction is endothermic.

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