Let's analyze the given chemical reaction and the associated enthalpy change:
The reaction provided is:
[tex]\[ 2 \text{NH}_3(g) \rightarrow \text{N}_2(g) + 3 \text{H}_2(g) \][/tex]
The change in enthalpy ([tex]\(\Delta H\)[/tex]) for this reaction is given as [tex]\( \Delta H = 92.4 \, \text{kJ/mol} \)[/tex].
### Step-by-Step Solution
1. Understanding Enthalpy Change ([tex]\(\Delta H\)[/tex]):
- [tex]\(\Delta H\)[/tex] represents the change in enthalpy or heat content of the reaction. It tells us whether the reaction absorbs or releases heat.
- A positive [tex]\(\Delta H\)[/tex] value ([tex]\(\Delta H > 0\)[/tex]) indicates that the reaction absorbs heat from its surroundings.
2. Classifying the Reaction Based on [tex]\(\Delta H\)[/tex]:
- If the reaction absorbs heat ([tex]\(\Delta H > 0\)[/tex]), it is endothermic.
- If the reaction releases heat ([tex]\(\Delta H < 0\)[/tex]), it is exothermic.
3. Analyzing the Given Reaction:
- The given enthalpy change is [tex]\( \Delta H = 92.4 \, \text{kJ/mol} \)[/tex], which is a positive value.
- Since [tex]\(\Delta H\)[/tex] is positive, this means that the reaction consumes heat from its surroundings.
4. Conclusion:
- Because the reaction has a positive enthalpy change ([tex]\( \Delta H = 92.4 \, \text{kJ/mol} \)[/tex]), it is an endothermic reaction.
Thus, the correct answer is:
A. The reaction is endothermic.
