Question

When producing hydrogen iodide, the energy of the reactants is 581 kJ/mol, and the energy of the products is 590 kJ/mol. The equation is shown. H2 + I2 → 2HI What is the total energy of the reaction? Is this an endothermic or exothermic reaction? (1 point) Responses –9 kJ/mol, endothermic –9 kJ/mol, endothermic 9 kJ/mol, exothermic 9 kJ/mol, exothermic 9 kJ/mol, endothermic 9 kJ/mol, endothermic –9 kJ/mol, exothermic

Answer 1

To determine the total energy change of the reaction, we can calculate the difference between the energy of the products and the energy of the reactants:

\[ \text{Total Energy Change} = \text{Energy of Products} - \text{Energy of Reactants} \]

Given:

• Energy of Reactants = 581 kJ/mol
• Energy of Products = 590 kJ/mol

Substituting the values:

\[ \text{Total Energy Change} = 590 , \text{kJ/mol} - 581 , \text{kJ/mol} = 9 , \text{kJ/mol} \]

Since the total energy change is positive (+9 kJ/mol), it indicates that the reaction absorbs energy from the surroundings. Therefore, the reaction is endothermic.

So the correct response is:

9 kJ/mol, endothermic