In the manufacture of `NH_(3)` by Haber's process, the condition which would give maximum yield is `N_(2)+3H_(2)hArr2NH_(3)+Q` kcal

Options

A. High temperatue, high pressure and hig concentrations of the rectants
B. High temperatuer, low pressure and low concentrations of the reactants
C. Low temperaturee and high pressure
D. Low temperaturee, low pressure and low concentration of `H_(2)`

Explanation

To determine the conditions that would give the maximum yield of ammonia (NH₃) in the Haber process, we need to analyze the given reaction:

\[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + Q \, \text{kcal} \]

### Step 1: Identify the nature of the reaction
The reaction is exothermic, meaning it releases heat. This can be inferred from the presence of \( Q \) in the equation, indicating heat is produced when the reaction proceeds to the right.

**Hint:** Remember that exothermic reactions release heat, which influences how temperature affects the equilibrium.

### Step 2: Apply Le Chatelier's Principle regarding temperature
For exothermic reactions, lowering the temperature favors the formation of products. Therefore, to maximize the yield of ammonia, we should operate at a low temperature.

**Hint:** Think about how temperature changes affect the position of equilibrium in exothermic reactions.

### Step 3: Analyze the effect of pressure on the reaction
Next, we consider the effect of pressure. The reaction involves:
- Reactants: 1 mole of \( N_2 \) and 3 moles of \( H_2 \) (total = 4 moles of gas)
- Products: 2 moles of \( NH_3 \) (total = 2 moles of gas)

According to Le Chatelier's Principle, increasing the pressure will shift the equilibrium towards the side with fewer moles of gas. In this case, that is the product side, where there are only 2 moles of \( NH_3 \).

**Hint:** Recall that increasing pressure favors the side of the reaction with fewer gas moles.

### Step 4: Combine the conditions for maximum yield
To achieve maximum yield of ammonia, we conclude that the optimal conditions are:
- **Low temperature** (to favor the exothermic reaction)
- **High pressure** (to favor the production of fewer moles of gas)

Thus, the conditions that would give maximum yield in the Haber process are low temperature and high pressure.

**Final Answer:** The conditions for maximum yield of \( NH_3 \) in the Haber process are low temperature and high pressure.