In the figure below, the change in internal energy of a gas that is taken from A to C along the blue path is +900 J. The work done on the gas along the red path ABC is -570 J. (b) If the pressure at point A is five times that of point C, what is the work done on the system in going from C to D?

An ideal gas initially at P₁, V₁, and T₁ is taken through a cycle as shown below. (Let the factor n = 3.9. Note, this is the factor by which volume and pressure increase, as noted on the PV-diagram; it is NOT the number of moles of gas.) P nP; P₁ B D nv; (a) Find the net work done on the gas per cycle for 1.35 mol of gas initially at 0°C. kJ (b) What is the net energy added by heat to the system per cycle? kJ

Consider the following two-step process. Heat is allowed to flow out of an ideal gas at constant volume so that its pressure drops from P₁ = 2.7 atm to P2 = 1.7 atm. Then the gas expands at constant pressure, from a volume of V₁ = 5.9 L to V₂ = 9.6 L, where the temperature reaches its original value. See the figure ( Figure 1). Figure P P₁ P2 σ P D HÅ AU = Value Units Submit Request Answer Part C 1 of 1 wwwww ? Calculate the total heat flow into or out of the gas. Express your answer to two significant figures and include the appropriate units. ☐ με Value Units Submit Request Answer

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If a (non-ideal) gas has non-negligible attractive intermolecular forces, would you expect the temperature to increase, decrease, or stay the same during an iso-enthalpic expansion of the gas? Explain your reasoning.

In the figure below, the change in internal energy of a gas that is taken from A to C along the blue path is +870 J. The work done on the gas along the red path ABC is -520 J. (a) How much energy must be added to the system by heat as it goes from A through B to C? (b) If the pressure at point A is five times that of point C, what is the work done on the system in going from C to D? (c) What is the energy exchanged with the surroundings by heat as the gas goes from C to A along the green path? (d) If the change in internal energy in going from point D to point A is +555 J, how much energy must be added to the system by heat as it goes from point C to point D?

= 2 is taken through a cycle as shown in the figure to the right, which is not necessarily drawn to scale. n moles of an ideal gas with adiabatic index Y The cycle proceeds as follows: 1– 2 is an isobaric compression to V2= Vo/2 2 – 3 is an isochoric process with P3 = 3P0 3 – 4 is an isothermal compression to V4 = Vo/4 4 – 5 is an isochoric heating process 5 – 1 is an adiabatic expansion back to Vo ЗРо Ро Vo/4 Vo/2 Vo (a) at constant pressure, What are Cv, the molar specific heat at constant volume, and Cp, the molar specific heat for this gas? Your answer should be in terms of n, R, T , or a subset of these quantities. (b) ( diagram) in terms of Po, and the temperatures T,, T3 , T4 , and T3 (the temperatures at points 2 – 5) in terms of To. All work must be shown. Find the unknown quantities P4 and P5 (which are the pressures at points 4 and 5 on the (c) Find the work done on the system in terms of n, R, T, , and pure numbers only for the 3, 3 → 4, 4 → 5, and 5 → 1. Make sure to show…

Part A: If you supply 2950 J of heat to 6.00 moles of an ideal diatomic gas initially at 23.0 ∘C in a perfectly rigid container, what will be the final temperature of the gas? Express in degrees Celsius. Part B: Suppose the gas in the container were an ideal monatomic gas instead. How much heat would you need to add to produce the same temperature change? Part C: Which pV diagram expresses these processes?