Question

2H₂(g) + O₂(g) -> 2H₂O(g) ΔHrxn = -483.64 kJ

How much energy is released during the formation of 1 mol H₂O(g)? __kJ

Answer 1

The energy released during the formation of 1 mole of H₂O(g) is -241.82 kJ.

Step-by-step explanation:

The enthalpy change of the reaction is -483.64 kJ for the formation of 2 moles of H₂O(g). To find the energy released for the formation of 1 mole of H₂O(g), we need to divide the enthalpy change by the stoichiometric coefficient, which is 2 in this case. This gives us -483.64 kJ / 2 = -241.82 kJ/mol. Therefore, the energy released during the formation of 1 mol H₂O(g) is -241.82 kJ.