1What is the defining characteristic of a thermodynamic state function?
2
For a process to occur under adiabatic conditions, what is the necessary condition?
3What is the standard enthalpy of all elements in their standard states?
4Given that the internal energy of combustion of methane is -X kJ/mol, how does the enthalpy of combustion (ΔH) compare to the internal energy of combustion (ΔU)?
5Using the given enthalpies of combustion for methane, graphite, and dihydrogen, calculate the enthalpy of formation of CH₄(g).
6A reaction, A + B → C + D + q, has a positive entropy change. Under what conditions is this reaction most likely to be spontaneous?
7In a process, 701 J of heat is absorbed by a system, and 394 J of work is done *by* the system. What is the change in internal energy (ΔU) for this process?
8The reaction of cyanamide, NH₂CN(s) with dioxygen results in a change in internal energy (ΔU) of -742.7 kJ/mol at 298 K. The reaction is NH₂CN(s) + 3/2O₂(g) → N₂(g) + CO₂(g) + H₂O(l). Calculate the enthalpy change (ΔH) for this reaction at 298 K.
9Which of the following is NOT a state function?
10Which type of process has zero heat transfer (q=0)?
