What would be the effect of increasing the volume of each of the following system on its equilibrium.
1. `2CO(g)+O_2(g)hArr2CO_2(g)`
2. `N_2O_4(g)hArr2NO_2(g)`

Options

A. 1 in forward and 2 in backward
B. both forward
C. both backward
D. 1 is backward and 2 in forward direction

Answer

To solve the problem of how increasing the volume affects the equilibrium of the given chemical reactions, we will apply Le Chatelier's principle. This principle states that if an external change is applied to a system at equilibrium, the system will adjust itself to counteract that change and restore a new equilibrium.

### Step-by-Step Solution:

1. **Identify the reactions and their equilibrium states:**
- For the first reaction:
\[ 2 \text{CO}(g) + \text{O}_2(g) \rightleftharpoons 2 \text{CO}_2(g) \]
- For the second reaction:
\[ \text{N}_2\text{O}_4(g) \rightleftharpoons 2 \text{NO}_2(g) \]

2. **Count the number of moles of gas on each side of the reactions:**
- For the first reaction:
- Left side: \(2 \text{CO} + 1 \text{O}_2 = 3 \text{ moles}\)
- Right side: \(2 \text{CO}_2 = 2 \text{ moles}\)
- For the second reaction:
- Left side: \(1 \text{N}_2\text{O}_4 = 1 \text{ mole}\)
- Right side: \(2 \text{NO}_2 = 2 \text{ moles}\)

3. **Analyze the effect of increasing volume:**
- Increasing the volume of a gas system decreases the pressure. According to Le Chatelier's principle, the equilibrium will shift toward the side with more moles of gas to counteract the decrease in pressure.

4. **Determine the direction of the shift for each reaction:**
- For the first reaction:
- Since there are 3 moles of gas on the left and 2 moles on the right, increasing the volume will shift the equilibrium to the left (toward the reactants) where there are more moles (3 moles).
- For the second reaction:
- There is 1 mole of gas on the left and 2 moles on the right. Increasing the volume will shift the equilibrium to the right (toward the products) where there are more moles (2 moles).

5. **Summarize the effects:**
- For the reaction \(2 \text{CO}(g) + \text{O}_2(g) \rightleftharpoons 2 \text{CO}_2(g)\), increasing the volume shifts the equilibrium to the left.
- For the reaction \(\text{N}_2\text{O}_4(g) \rightleftharpoons 2 \text{NO}_2(g)\), increasing the volume shifts the equilibrium to the right.

### Final Answer:
1. The equilibrium for \(2 \text{CO}(g) + \text{O}_2(g) \rightleftharpoons 2 \text{CO}_2(g)\) shifts to the left.
2. The equilibrium for \(\text{N}_2\text{O}_4(g) \rightleftharpoons 2 \text{NO}_2(g)\) shifts to the right.