* The reaction you've described is the combustion of hydrogen with carbon dioxide: H₂ + CO₂ → H₂O + CO

* Combustion reactions are exothermic: This means they release energy into the surroundings. The energy content of the reactants is *higher* than the energy content of the products.

Therefore, the energy content of the reactants (H₂ and CO₂) should be higher than the energy content of the products (H₂O and CO).

Let's look at a more realistic example:

The combustion of methane (CH₄) with oxygen (O₂) to produce carbon dioxide (CO₂) and water (H₂O) is a well-known exothermic reaction.

* CH₄ + 2O₂ → CO₂ + 2H₂O

In this case, the energy content of the reactants (CH₄ and O₂) is indeed higher than the energy content of the products (CO₂ and H₂O). This energy difference is released as heat and light during the combustion process.

Key Point: Exothermic reactions have a negative enthalpy change (ΔH < 0), indicating that energy is released.