Question

hydrogen bromide breaks down into diatomic hydrogen and bromine in the reaction shown. 2hbr → h₂ + br₂ the energy of the reactant is 732 kj/mol, and the energy of the products is 630 kj/mol. what is the total energy of the reaction? is this reaction endothermic or exothermic? (1 point) - 102 kj/mol, endothermic 102 kj/mol, endothermic - 102 kj/mol, exothermic 102 kj/mol, exothermic

Explanation:

Step1: Calculate energy change

The energy change ($\Delta H$) of a reaction is given by the formula $\Delta H=H_{products}-H_{reactants}$. Here, $H_{reactants} = 732$ kJ/mol and $H_{products}=630$ kJ/mol. So, $\Delta H=630 - 732=- 102$ kJ/mol.

Step2: Determine reaction type

If $\Delta H<0$, the reaction is exothermic as heat is released. Since $\Delta H=-102$ kJ/mol $<0$, the reaction is exothermic.

Answer:

C. - 102 kJ/mol, exothermic