For the reaction `A(g) +3B(g) hArr 2C(g) `at `27^(@)C`, 2 moles of `A`, 4 moles of B and 6 moles of C are present in 2 litre vessel. If `K_(c)` for the reaction is 1.2, the reaction will proceed in `:`

Options

A. Forward direction
B. backward direction
C. neither direction
D. none of these

Answer

To determine the direction in which the reaction will proceed, we need to calculate the reaction quotient (Q) and compare it with the equilibrium constant (Kc).

### Step-by-Step Solution:

1. **Identify the Reaction and Given Data:**
The reaction is:
\[ A(g) + 3B(g) \rightleftharpoons 2C(g) \]
Given:
- Moles of A = 2
- Moles of B = 4
- Moles of C = 6
- Volume of the vessel = 2 L
- \( K_c = 1.2 \)

2. **Calculate the Concentrations:**
Concentration is calculated using the formula:
\[ \text{Concentration} = \frac{\text{Number of moles}}{\text{Volume in liters}} \]
- Concentration of A:
\[ [A] = \frac{2 \text{ moles}}{2 \text{ L}} = 1 \text{ M} \]
- Concentration of B:
\[ [B] = \frac{4 \text{ moles}}{2 \text{ L}} = 2 \text{ M} \]
- Concentration of C:
\[ [C] = \frac{6 \text{ moles}}{2 \text{ L}} = 3 \text{ M} \]

3. **Calculate the Reaction Quotient (Q):**
The reaction quotient (Q) is calculated using the formula:
\[ Q = \frac{[C]^2}{[A][B]^3} \]
Substituting the concentrations:
\[ Q = \frac{(3)^2}{(1)(2)^3} = \frac{9}{8} = 1.125 \]

4. **Compare Q with Kc:**
- Given \( K_c = 1.2 \)
- We found \( Q = 1.125 \)

Since \( K_c > Q \) (1.2 > 1.125), the reaction will proceed in the forward direction to reach equilibrium.

5. **Conclusion:**
The reaction will proceed in the forward direction.

### Final Answer:
The reaction will proceed in the forward direction.

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