Nitrogen gas reacts with oxygen gas to produce dinitrogen monoxide gas.
2 N2(g) + O2(g) + 163.2 kJ → 2 N2O(g)
Is this reaction endothermic or exothermic?
How do you know?
It is endothermic. How do you know?
2 N2(g) + O2(g) + 163.2 kJ → 2 N2O(g)
The equation tells you that 2 mols N2 will react with 1 mol of O2 and when you ADD 163.2 kJ, it gives you the products. So if you must ADD heat it is endotheric. If the 163.2 kJ was on the other side, like this, it would be exothermic. 2 N2(g) + O2(g) → 2 N2O(g) + 163.2 kJ BECAUSE that reaction tell you that 1 mols N2 react with 1 mol O2 to produce 2 mols N2O AND gives off 163.2 kJ heat.
The given reaction is exothermic. We can determine this by looking at the energy term on the right side of the chemical equation. In this case, there is a negative sign in front of the energy term (+163.2 kJ). This indicates that energy is released during the reaction, making it exothermic.
To determine whether a reaction is endothermic or exothermic, we need to consider the energy change associated with the reaction.
In the given reaction, it is stated that 163.2 kJ of energy is released. This release of energy indicates that the reaction is exothermic.
Exothermic reactions involve the release of energy in the form of heat, which usually causes an increase in temperature of the surroundings. In this case, the 163.2 kJ released indicates that the reaction is exothermic, as it releases energy in the form of heat.