`2H_2(g) +CO(g) hArr CH_3OH(g) , DeltaH=-92.2` kJ. Which of the following condition will shift the equilibrium in the forward direction ?

Options

A. CO is removed
B. `CH_3 OH` is added
C. The pressure of the system is increased
D. Temperature of the system is increased

Answer

To determine which condition will shift the equilibrium of the reaction \(2H_2(g) + CO(g) \rightleftharpoons CH_3OH(g)\) in the forward direction, we can analyze the effects of concentration, temperature, and pressure based on Le Chatelier's principle.

### Step-by-Step Solution:

1. **Identify the Reaction and Conditions**:
The given reaction is:
\[ 2H_2(g) + CO(g) \rightleftharpoons CH_3OH(g) \]
with a change in enthalpy (\(\Delta H\)) of -92.2 kJ, indicating that the reaction is exothermic.

2. **Analyze the Effect of Concentration**:
- **Removing Reactants**: If the concentration of \(CO\) (reactant) is decreased, the equilibrium will shift to the left to produce more \(CO\). This does not favor the forward direction.
- **Adding Products**: If \(CH_3OH\) (product) is added, the equilibrium will shift to the left to consume the added product. This also does not favor the forward direction.

3. **Analyze the Effect of Temperature**:
- Since the reaction is exothermic, increasing the temperature will shift the equilibrium to the left (towards the reactants) to absorb the excess heat. Thus, increasing the temperature does not favor the forward direction. Conversely, lowering the temperature would favor the forward direction, but that is not one of the options given.

4. **Analyze the Effect of Pressure**:
- The reaction has 3 moles of gas on the reactant side (2 moles of \(H_2\) and 1 mole of \(CO\)) and 1 mole of gas on the product side (\(CH_3OH\)). According to Le Chatelier's principle, increasing the pressure will shift the equilibrium towards the side with fewer moles of gas, which is the product side in this case. Therefore, increasing the pressure will favor the forward direction.

5. **Conclusion**:
The condition that will shift the equilibrium in the forward direction is **increasing the pressure** of the system.

### Final Answer:
Increasing the pressure of the system will shift the equilibrium in the forward direction.

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