absorbs energy, and it is negative if the system releases energy. (Figure 1) The total change in internal energy is the sum of the heat, q, and work, w: AE=q+w. Part B Figure AE, > 0 system. system <0 Surroundings E System An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at a constant pressure of 35.0 atm and releases 71.1 kJ of heat. Before the reaction, the volume of the system was 8.40 L. After the reaction, the volume of the system was 2.00 L. Calculate the total internal energy change, AE, in kilojoules. Express your answer with the appropriate units. View Available Hint(s) 1 of 2 AE= Value Units Submit ? Surroundings System E AE=q+w State functions versus path functions The change in internal energy, AE, is a state function because it depends only on the initial and final states of the system, and not on the path of change. In contrast, q and w are path functions because they depend on the path of change and not just the initial and final states of the system. Part C An ideal gas (which is is a hypothetical gas that conforms to the laws governing gas behavior) confined to a container with a massless piston at the top. (Figure 2) A massless wire is attached to absorbs energy, and it is negative if the system releases energy. (Figure 1) The total change in internal energy is the sum of the heat, q, and work, w: AE=q+w. The change in internal energy, AE, is a state function because it depends only on the initial and final states of the system, and not on the path of change. In contrast, q and w are path functions because they depend on the path of change and not just the initial and final states of the system. Figure AE, > 0 system. Surroundings E System Surroundings system <0 System E AE=q+w 1 of 2 Part C An ideal gas (which is is a hypothetical gas that conforms to the laws governing gas behavior) confined to a container with a massless piston at the top. (Figure 2) A massless wire is attached to the piston. When an external pressure of 2.00 atm is applied to the wire, the gas compresses from 4.40 to 2.20 L. When the external pressure is increased to 2.50 atm, the gas further compresses from 2.20 to 1.76 L. In a separate experiment with the same initial conditions, a pressure of 2.50 atm was applied to the ideal gas, decreasing its volume from 4.40 to 1.76 L in one step. If the final temperature was the same for both processes, what is the difference between q for the two-step process and q for the one-step process in joules? Express your answer with the appropriate units. View Available Hint(s) ? Value Units Submit Provide Feedback Next >