The reaction `2SO_(2) + O_(2) rarr 2SO_(3) + heat` . The equilibrium reaction proceeds in forward direction by :

Options

A. Addition of `O_(2)`
B. Removal of `O_(2)`
C. Addition of inert gas
D. Cannot proceed

Explanation

To solve the question regarding the equilibrium reaction \(2SO_2 + O_2 \rightleftharpoons 2SO_3 + \text{heat}\), we need to analyze how the equilibrium can be shifted in the forward direction. Here’s a step-by-step solution:

### Step 1: Understand the Reaction
The given reaction is:
\[ 2SO_2 + O_2 \rightleftharpoons 2SO_3 + \text{heat} \]
This is an exothermic reaction, meaning it releases heat as a product.

### Step 2: Apply Le Chatelier's Principle
Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.

### Step 3: Identify Factors Affecting Equilibrium
The factors that can affect the equilibrium position include:
- Concentration of reactants or products
- Temperature
- Pressure (for gaseous reactions)

### Step 4: Determine How to Shift Equilibrium Forward
To shift the equilibrium to the right (forward direction), we can:
1. Increase the concentration of reactants (in this case, \(SO_2\) or \(O_2\)).
2. Remove products (\(SO_3\)).
3. Increase the pressure (if applicable).
4. Decrease the temperature (since it’s an exothermic reaction).

### Step 5: Analyze the Given Options
The question asks how the equilibrium proceeds in the forward direction. The most direct method is to add more reactants.

- **Adding \(O_2\)** (which is a reactant) will shift the equilibrium to the right, producing more \(SO_3\).
- Other options (not specified in the question) may involve adding products or changing temperature in a way that does not favor the forward reaction.

### Conclusion
Thus, the equilibrium reaction proceeds in the forward direction primarily by adding the reactant \(O_2\).

**Final Answer: The equilibrium reaction proceeds in the forward direction by adding \(O_2\) (Option A).**

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