An ideal gaseous reaction (which is a hypothetical gaseousreaction that conforms to the laws governing gas behavior) occursat a constant pressure of 50.0 atm and releases 60.4 kJ of heat.Before the reaction, the volume of the system was 7.80 L . Afterthe reaction, the volume of the system was 2.80 L . Calculate thetotal internal energy change, ΔE, in kilojoules. Express youranswer with the appropriate units. ΔE = -35.2 kJ SubmitHintsMyAnswersGive UpReview Part Correct Although the system absorbed someenergy in the form of work, the significant release of heat causedthe total change to be negative. State functions versus pathfunctions The change in internal energy, ΔE, is a state functionbecause it depends only on the initial and final states of thesystem, and not on the path of change. In contrast, q and w arepath functions because they depend on the path of change and notjust the initial and final states of the system.
Part C An ideal gas (which is is a hypothetical gas thatconforms to the laws governing gas behavior) confined to acontainer with a massless piston at the top. (Figure 2) A masslesswire is attached to the piston. When an external pressure of 2.00atm is applied to the wire, the gas compresses from 6.60 to 3.30 L. When the external pressure is increased to 2.50 atm, the gasfurther compresses from 3.30 to 2.64 L . In a separate experimentwith the same initial conditions, a pressure of 2.50 atm wasapplied to the ideal gas, decreasing its volume from 6.60 to 2.64 Lin one step. If the final temperature was the same for bothprocesses, what is the difference between q for the two-stepprocess and q for the one-step process in joules? Express youranswer with the appropriate units.
please answer for Part C
