Final answer:
The question addresses a chemical reaction between hydrogen gas and oxygen gas to produce liquid water and asks about the potential temperature of the resulting product if it absorbed all the energy released. It's not possible to determine the exact temperature without further data, but the significant amount of heat released suggests a substantial temperature rise.
Step-by-step explanation:
The question deals with a chemical reaction where hydrogen gas reacts with oxygen gas to form liquid water, and involves calculating the temperature of the product if it were to absorb all the energy released in the reaction. In the given scenario, 4.0 mol of H₂(g) reacts with 2.0 mol of O₂(g) to produce water, releasing energy in the form of heat. As per the information provided, we know that the enthalpy change for the formation of 1 mole of liquid water from hydrogen and oxygen gases at the same temperature and pressure is -286 kJ. Bearing in mind that enthalpy change (ΔH) is an extensive property, the total amount of heat released when forming water from the given amounts of hydrogen and oxygen in this reaction would be 4 times -286 kJ or -1144 kJ, since 4 moles of water would be formed.
It is not possible to determine the final temperature of the resulting gas without specific heat capacities and masses, but theoretically, if all this heat were absorbed by the water produced, it would result in a significant increase in temperature. Additionally, if the reaction generates water vapor instead of liquid water, each mole would release only 242 kJ, leading to a different amount of heat absorption and a possibly lower temperature increase.