The equilibrium of the reaction `N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g)` will be shifted to the right when:

Options

A. `K_(p) lt Q`
B. `Q lt K_(p)`
C. `Q=K_(p)`
D. `Q lt 2K_(p)`

Answer

To determine when the equilibrium of the reaction \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \) will shift to the right, we need to analyze the factors that influence chemical equilibrium based on Le Chatelier's principle.

### Step-by-Step Solution:

1. **Understand the Reaction**: The given reaction is:
\[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \]
This is a synthesis reaction where nitrogen and hydrogen gases combine to form ammonia.

2. **Identify the Reaction Quotient (Q) and Equilibrium Constant (Kp)**:
- The reaction quotient \( Q \) is calculated using the concentrations of the reactants and products at any point in time:
\[ Q = \frac{[NH_3]^2}{[N_2][H_2]^3} \]
- The equilibrium constant \( K_p \) is the value of \( Q \) when the system is at equilibrium.

3. **Determine the Direction of Shift**:
- According to Le Chatelier's principle, if a system at equilibrium is disturbed, it will shift in the direction that counteracts the disturbance.
- The equilibrium will shift to the right (towards products) if \( Q < K_p \). This means that there are more reactants than what is present at equilibrium, prompting the reaction to produce more products.

4. **Factors that Shift Equilibrium to the Right**:
- **Increase in Reactants**: Adding more \( N_2 \) or \( H_2 \) will shift the equilibrium to the right.
- **Decrease in Products**: Removing \( NH_3 \) will also shift the equilibrium to the right.
- **Increase in Pressure**: Since there are 4 moles of gas on the reactant side (1 mole of \( N_2 \) and 3 moles of \( H_2 \)) and 2 moles on the product side (2 moles of \( NH_3 \)), increasing the pressure will shift the equilibrium to the side with fewer moles of gas, which is the right side in this case.
- **Increase in Temperature**: If the reaction is exothermic, increasing the temperature will shift the equilibrium to the left. Conversely, if it is endothermic, it will shift to the right.

5. **Conclusion**: The equilibrium of the reaction will shift to the right when:
- The concentration of reactants increases.
- The concentration of products decreases.
- The pressure is increased.
- The temperature is adjusted favorably (depending on the nature of the reaction).