are these endothermic or exothermic?

2H2O2 (l) �¨ 2H2O(l) + O2(g)
∆H = -190 kj

C(s) + H2O (g) �¨ CO (g) + H2 (g)
∆H = +113

A negative delta H means the heat is given up by the reaction. A + delta H means the heat is added to the reaction.

thanks

to this, the first reaction is exothermic and the second reaction is endothermic.

The first reaction, 2H2O2(l) → 2H2O(l) + O2(g), has a delta H of -190 kJ. Since the delta H is negative, it means that heat is given off during the reaction. This indicates an exothermic reaction.

The second reaction, C(s) + H2O(g) → CO(g) + H2(g), has a delta H of +113 kJ. Since the delta H is positive, it means that heat is added to the reaction. This indicates an endothermic reaction.

So, to determine if a reaction is endothermic or exothermic, you need to look at the sign of the delta H value. Negative delta H represents an exothermic reaction, and positive delta H represents an endothermic reaction.

The first reaction:

2H2O2 (l) → 2H2O (l) + O2 (g) with ∆H = -190 kJ

Since the ∆H value is negative (-190 kJ), this indicates that the reaction is exothermic. In an exothermic reaction, heat is released as a product.

The second reaction:
C(s) + H2O (g) → CO (g) + H2 (g) with ∆H = +113 kJ

Since the ∆H value is positive (+113 kJ), this indicates that the reaction is endothermic. In an endothermic reaction, heat is absorbed as a reactant.