To determine whether a chemical reaction is exothermic or endothermic, we need to consider the energy change involved in the reaction. Here's a detailed breakdown of the process:
1. Understand the Energy Change:
- In the given reaction:
[tex]\[
\text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O} + 58 \, \text{KJ}
\][/tex]
- The energy change for the reaction is given as +58 KJ.
2. Classify the Reaction:
- Exothermic Reaction: In an exothermic reaction, energy is released into the surroundings, usually in the form of heat. As a result, the temperature of the surroundings increases. These reactions have negative energy changes because energy is lost by the system.
- Endothermic Reaction: In an endothermic reaction, energy is absorbed from the surroundings, which usually leads to a decrease in the temperature of the surroundings. These reactions have positive energy changes because energy is gained by the system.
3. Interpret the Given Energy Change:
- Since the energy change given is +58 KJ, it means the system absorbs 58 KJ of energy.
4. Determine the Type of Reaction:
- According to our understanding:
- If the energy change is positive, it indicates an endothermic reaction because energy is absorbed.
- If the energy change is negative, it indicates an exothermic reaction because energy is released.
- Given the positive energy change of +58 KJ, this indicates that the reaction is endothermic.
5. Conclusion:
- Therefore, the reaction:
[tex]\[
\text{HCl} + \text{NaOH} \rightarrow \text{NaCl} + \text{H}_2\text{O} + 58 \, \text{KJ}
\][/tex]
is an endothermic reaction.
To summarize, based on the energy change of +58 KJ, we conclude that the reaction is endothermic.
