For the reaction, for which the activation energies for forward and backward reactions are same, then:

Options

A. `DeltaH=0`
B. `DeltaS=0`
C. The order is zero
D. None of these

Explanation

To solve the problem regarding the activation energies for a reaction where the activation energies for the forward and backward reactions are the same, we can follow these steps:

### Step 1: Understand the concept of activation energy
Activation energy (Ea) is the minimum energy required for a chemical reaction to occur. For a given reaction, there are two activation energies to consider: one for the forward reaction (Ea forward) and one for the reverse reaction (Ea backward).

**Hint:** Recall that activation energy is a barrier that must be overcome for a reaction to proceed.

### Step 2: Relate activation energy to enthalpy change
The relationship between the activation energies and the enthalpy change (ΔH) of the reaction can be expressed as:
\[ \Delta H = E_a \text{(forward)} - E_a \text{(backward)} \]

**Hint:** Remember that ΔH indicates whether the reaction is exothermic or endothermic.

### Step 3: Apply the given condition
According to the problem, the activation energies for the forward and backward reactions are the same:
\[ E_a \text{(forward)} = E_a \text{(backward)} \]

**Hint:** Think about what happens to the equation when both activation energies are equal.

### Step 4: Substitute the values into the equation
Substituting the condition into the equation for ΔH gives:
\[ \Delta H = E_a \text{(forward)} - E_a \text{(forward)} = 0 \]

**Hint:** Simplifying the equation will help you see the result clearly.

### Step 5: Conclude the result
Since ΔH equals zero, this indicates that the reaction is at equilibrium, and there is no net change in energy when moving from reactants to products or vice versa.

**Hint:** Consider what it means for a reaction to have zero enthalpy change.

### Final Answer
The conclusion is that if the activation energies for the forward and backward reactions are the same, then:
\[ \Delta H = 0 \]

Thus, the correct answer to the question is that the enthalpy change (ΔH) for the reaction is zero.