Understanding Endothermic Reactions
Endothermic reactions *absorb* heat from their surroundings. This means that energy is required for the reaction to occur. The products of an endothermic reaction have higher energy content than the reactants.
Representing Heat in Chemical Equations
* On the Reactant Side: In an endothermic reaction, heat is considered a *reactant*. It's written on the left side of the chemical equation with a positive sign.
* 예:
```
N₂(g) + O₂(g) + 180.5 kJ → 2 NO(g)
```
This equation shows that 180.5 kJ of heat energy is needed to convert nitrogen and oxygen gas into nitrogen monoxide gas.
* 엔탈피 변화 (ΔH) : Another way to represent heat in an endothermic reaction is using the enthalpy change (ΔH), which is always positive for endothermic reactions.
* 예:
```
N₂(g) + O₂(g) → 2 NO(g) ΔH =+180.5 kJ/mol
```
This equation indicates that 180.5 kJ of energy is absorbed (taken in) per mole of nitrogen monoxide produced.
키 포인트
* Positive Sign: The positive sign before the heat value or in the enthalpy change signifies that heat is being absorbed.
* 에너지 흐름 : The heat term in an endothermic reaction represents the amount of energy needed for the reaction to occur.
Let me know if you would like examples of specific endothermic reactions!
