Enthalpy Change for a Specific Amount of Reactant

Enthalpy Change for a Specific Amount of Reactant Here is how to determine  the change in enthalpy of a chemical reaction with a given amount of reactant.   You may wish to review the laws of thermochemistry and endothermic and exothermic reactions​ before you begin. Problem: For the decomposition of hydrogen peroxide, it is known that:H2O2(l) → H2O(l) 1/2 O2(g); ΔH -98.2 kJUsing this information, determine ΔH for the reaction:2 H2O(l) O2(g) → 2 H2O2(l) Solution: When looking at the second equation, we see it is double the first reaction and in the opposite direction. First, change the direction of the first equation.  When the direction of the reaction is changed, the sign on ΔH changes for the reaction H 2O2(l) → H2O(l) 1/2 O2(g); ΔH -98.2 kJ becomes H2O(l) 1/2 O2(g) → H2O2(l); ΔH 98.2 kJ Second, multiply this reaction by 2.  When multiplying a reaction by a constant, the ΔH is multiplied by the same constant.2 H2O(l) O2(g) → 2 H2O2(l); ΔH 196.4 kJ Answer: ΔH 196.4 kJ for the reaction: 2 H2O(l) O2(g) → 2 H2O2(l)