Final answer:
The ΔH for the reaction in question is not provided and cannot be deduced from the information available. Standard enthalpy of formation values or calorimeter experimental data would be needed. The provided information relates to redox reactions but does not directly answer the question.
Step-by-step explanation:
The student has asked for the value of the enthalpy change (ΔH) for the reaction CuO (s) + NO (g) = Cu2O (s) + NO2 (g). To determine the ΔH for this reaction, you would need to refer to standard enthalpy of formation values for each of the substances or perform a calorimeter experiment. Neither the enthalpy values nor experimental data for this specific reaction have been provided in the information given.
However, the information provided discusses various half-reactions and net ionic reactions involving copper and nitric acid which are related to redox reactions but not directly to the given reaction. In redox reactions, species like Cu(s) are oxidized (oxidation) to Cu2+ (aq) while other species are reduced (reduction). Spectator ions, which do not participate in the redox change, may appear unchanged on both sides of the full ionic equation.
It is important to note that the ΔH for this reaction could be calculated using Hess's law if the standard enthalpies of formation or reaction enthalpies for other known reactions are provided. This reaction appears to be a redox reaction, and solving it may require the use of half-reaction methods and balancing redox equations.