Question

When Fe2O3(s) reacts with H2(g) to form Fe(s) and H2O(g), 98.8 kJ of energy are absorbed for each mole of Fe2O3(s) that reacts. Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation. Note that the answer box for the energy term is case sensitive. Use the SMALLEST INTEGER coefficients possible and put the energy term in the last box on the appropriate side of the equation. If a box is not needed, leave it blank.

Answer 1

The thermochemical equation for the reaction is Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(g) + 98.8 kJ.

Step-by-step explanation:

The thermochemical equation for the reaction when Fe2O3(s) reacts with H2(g) to form Fe(s) and H2O(g) with an energy term of 98.8 kJ is:

Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(g) + 98.8 kJ

In this balanced equation, Fe2O3 and H2 are the reactants, and Fe and H2O are the products. The energy term of 98.8 kJ is on the product side of the equation.