Tell whether reaction will get affected by increase of pressure? Also mention, whether change will cause the reaction to go into
the right or left direction?
`C_(2)H_(4(g))+H_(2(g))hArrC_(2)H_(6(g))`

Explanation

To determine whether the reaction will be affected by an increase in pressure and in which direction it will shift, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reaction**: The given reaction is:
\[ C_2H_4(g) + H_2(g) \rightleftharpoons C_2H_6(g) \]

2. **Count the Moles of Gases**:
- On the **reactant side**:
- \(C_2H_4\) has 1 mole.
- \(H_2\) has 1 mole.
- Total moles of reactants = \(1 + 1 = 2\) moles.
- On the **product side**:
- \(C_2H_6\) has 1 mole.
- Total moles of products = \(1\) mole.

3. **Apply Le Chatelier's Principle**: According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change in pressure, the equilibrium will shift in a direction that counteracts the change.

4. **Analyze the Effect of Pressure**:
- If pressure is increased, the equilibrium will shift towards the side with fewer moles of gas.
- In this case, we have:
- Reactants: 2 moles (1 mole of \(C_2H_4\) + 1 mole of \(H_2\))
- Products: 1 mole (1 mole of \(C_2H_6\))

5. **Determine the Direction of Shift**:
- Since there are more moles of gas on the reactant side (2 moles) than on the product side (1 mole), an increase in pressure will cause the equilibrium to shift to the right, towards the products.

6. **Conclusion**:
- Yes, the reaction will be affected by an increase in pressure.
- The change will cause the reaction to shift to the right (towards the formation of \(C_2H_6\)).

### Summary:
- **Effect of Pressure**: Yes, it will be affected.
- **Direction of Shift**: To the right (towards products).