Question

Which answer best describes the transfer of heat that occurs when 1.20 mol of H2 reacts? given 2H₂ + O₂-----> 2H₂O delta H rxn = -484 kJ the answer includes kJ released or absorbed

Answer 1

The reaction 2H₂ + O₂ -> 2H₂O has a ΔH reaction of -484 kJ, indicating that it is exothermic and releases heat. When 1.20 mol of H2 reacts, 290.4 kJ of heat is released.

Step-by-step explanation:

The given reaction is 2H₂ + O₂ ----> 2H₂O with ΔH (delta H) reaction being -484 kJ. The negative sign indicates that the reaction is exothermic, meaning it releases heat into its surroundings. To calculate the amount of heat released when 1.20 mol of H2 reacts, we have to use the stoichiometric ratio. The reaction indicates that 2 mol of H2 produces 484 kJ of energy. So, for 1.20 mol of H2, we divide -484 kJ/2 mol (reaction heat per mol of H2) by 1.20 mol, which will give us -290.4 kJ. Hence, 290.4 kJ of heat is released when 1.20 mol of H2 reacts.

Learn more about Exothermic reaction