For the reaction
`N_(2)(g)+O_(2)(g)hArr2NO(g)`
If pressure id increased by reducing the volume of the container then :

Options

A. total pressure at equilibrium will remain same
B. concentration of all the component at equilibrium will change
C. concentration of all the component at equilibrium will ramin same
D. equilibrium will shift in the beckward direction

Answer

To solve the problem, we will analyze the reaction and apply Le Chatelier's principle to understand the effects of increasing pressure by reducing the volume of the container.

### Step-by-Step Solution:

1. **Identify the Reaction**:
The given reaction is:
\[ N_2(g) + O_2(g) \rightleftharpoons 2NO(g) \]

2. **Count the Moles of Gases**:
- On the reactant side, we have:
- 1 mole of \(N_2\)
- 1 mole of \(O_2\)
- Total = 2 moles of gas (reactants)
- On the product side, we have:
- 2 moles of \(NO\)
- Total = 2 moles of gas (products)

3. **Apply Le Chatelier's Principle**:
Le Chatelier's principle states that if a system at equilibrium is subjected to a change in pressure, temperature, or concentration, the system will adjust to counteract that change and establish a new equilibrium.
- In this case, increasing the pressure by reducing the volume will favor the side with fewer moles of gas.
- Since both sides of the reaction have the same number of moles (2 moles), the equilibrium position will not shift in either direction.

4. **Effect of Volume Reduction**:
- Reducing the volume increases the concentration of all gaseous components because concentration is defined as the number of moles divided by the volume.
- Therefore, while the equilibrium position does not shift, the concentrations of all components (reactants and products) will increase.

5. **Conclusion**:
- The total pressure at equilibrium will remain the same because the number of moles of gas on both sides is equal.
- However, the concentration of all components at equilibrium will change (increase).

### Final Answer:
The correct statement is: **The concentration of all components at equilibrium will change (increase).**

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