`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 analyze the effect of an increase in temperature on the equilibrium of the reaction:

**Reaction:**
\[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + \text{heat} \]

### Step 1: Identify the Nature of the Reaction
The given reaction is exothermic, meaning it releases heat as a product. In this reaction, the formation of ammonia (\(NH_3\)) from nitrogen (\(N_2\)) and hydrogen (\(H_2\)) releases heat.

**Hint:** Remember that exothermic reactions release heat, while endothermic reactions absorb heat.

### Step 2: Apply Le Chatelier's Principle
According to Le Chatelier's Principle, if a system at equilibrium is subjected to a change in temperature, pressure, or concentration, the equilibrium will shift in a direction that counteracts the change.

**Hint:** Le Chatelier's Principle helps predict how a system at equilibrium responds to changes in conditions.

### Step 3: Analyze the Effect of Increasing Temperature
When the temperature of the system is increased, it is equivalent to adding heat to the system. Since the reaction is exothermic and produces heat, the system will try to counteract this change by favoring the endothermic direction, which is the reverse reaction (the formation of \(N_2\) and \(H_2\)).

**Hint:** Think of temperature changes as adding or removing heat from the system.

### Step 4: Determine the Direction of the Shift
Since the forward reaction produces heat, increasing the temperature will shift the equilibrium to the left (towards the reactants) to absorb the excess heat.

**Hint:** The direction of the shift can be determined by identifying which side of the reaction absorbs heat.

### Conclusion
Thus, the effect of increasing the temperature on the equilibrium of the reaction \(N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + \text{heat}\) is that the equilibrium will shift to the left, favoring the formation of reactants (\(N_2\) and \(H_2\)).

**Final Answer:** The equilibrium shifts to the left.