`N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g) + heat`.What is the effect of the increase of temperature on the equilibrium of the reaction ?

Options

A. Equilibrium is shifted to the left
B. Equilibrium is shifted to the right
C. Equilibrium is unaltered
D. Reactions rate does not change

Explanation

To determine the effect of an increase in temperature on the equilibrium of the reaction \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + \text{heat} \), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Nature of the Reaction**:
- The given reaction is \( N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + \text{heat} \).
- This reaction is exothermic because heat is produced as a product.

2. **Understand the Principle of Le Chatelier**:
- According to Le Chatelier's principle, if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium shifts to counteract the change.
- In an exothermic reaction, heat can be considered as a product.

3. **Analyze the Effect of Temperature Increase**:
- When the temperature of an exothermic reaction is increased, the system will try to counteract this change by favoring the endothermic direction (which absorbs heat).
- In this case, the endothermic direction is the reverse reaction (the formation of reactants \( N_2 \) and \( H_2 \)).

4. **Conclusion**:
- Therefore, increasing the temperature will shift the equilibrium to the left, favoring the reactants \( N_2 \) and \( H_2 \).
- The correct answer is that the equilibrium is shifted to the left.

### Final Answer:
The equilibrium of the reaction shifts to the left upon an increase in temperature.

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