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The activation energies of the forward a...

The activation energies of the forward and backward reactions in the case of a chemical reaction are 30.5 and 45.5 KJ/mol , respectively . The reaction is:

A

exothermic

B

endothermic

C

neither exothermic

D

independent of temperature

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The correct Answer is:
To determine whether the given chemical reaction is exothermic or endothermic based on the provided activation energies, we can follow these steps: ### Step-by-Step Solution: 1. **Identify the Activation Energies**: - The activation energy of the forward reaction (Ea, forward) is given as 30.5 kJ/mol. - The activation energy of the backward reaction (Ea, backward) is given as 45.5 kJ/mol. 2. **Use the Formula for ΔH**: - The change in enthalpy (ΔH) for the reaction can be calculated using the formula: \[ \Delta H = E_a (\text{forward}) - E_a (\text{backward}) \] 3. **Substitute the Values**: - Plug in the values of the activation energies: \[ \Delta H = 30.5 \, \text{kJ/mol} - 45.5 \, \text{kJ/mol} \] 4. **Calculate ΔH**: - Perform the subtraction: \[ \Delta H = 30.5 - 45.5 = -15 \, \text{kJ/mol} \] 5. **Interpret the Result**: - Since ΔH is negative (-15 kJ/mol), this indicates that the reaction releases energy. - A negative ΔH signifies that the reaction is exothermic. ### Conclusion: The reaction is exothermic because the calculated ΔH is negative. ---
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