gas. 2. Suppose there are two containers, A and B, both filled with the same diatomic ideal The containers are completely isolated from their environment, and are separated from each other by a non-permeable, rigid and adiabatic wall. The total energy in the composite system (container A + container B) is 50 kJ, and each container has a volume of 3 m³. Container A holds 5 moles of the gas, and container B holds 7 moles. Container A is initially at room temperature. (a) Calculate the energy in container A, the energy in container B, and the temperature of container B. (b) Calculate the pressure in each of the two containers. (c) If we allow heat to travel through the wall separating the two containers, what does the temperature in the two containers become at equilibrium? How does the pressure change in each of the containers? (d) If we make this wall flexible and, at the same time, also allow heat to travel through it, what does the temperature and pressure of the containers become at equilibrium?

gas. 2. Suppose there are two containers, A and B, both filled with the same diatomic ideal The containers are completely isolated from their environment, and are separated from each other by a non-permeable, rigid and adiabatic wall. The total energy in the composite system (container A + container B) is 50 kJ, and each container has a volume of 3 m³. Container A holds 5 moles of the gas, and container B holds 7 moles. Container A is initially at room temperature. (a) Calculate the energy in container A, the energy in container B, and the temperature of container B. (b) Calculate the pressure in each of the two containers. (c) If we allow heat to travel through the wall separating the two containers, what does the temperature in the two containers become at equilibrium? How does the pressure change in each of the containers? (d) If we make this wall flexible and, at the same time, also allow heat to travel through it, what does the temperature and pressure of the containers become at equilibrium?

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

See similar textbooks

Similar questions

The temperature of 10 moles of an ideal gas is 1000 K. Compute the work done by the gas when it expands isothermally to three times its initial volume. Given: Boltzmann constant: k = 1.38 x 10–23 J/K, Ideal Gas Constant: R = 8.31 J/(mol K) A. 91300 J B. 9130 J C. 913 J D. 91 J E. 9 J
100 J of work is done in compressing a gas adiabatically. What is the change in internal energy of the gas? Select one: O a. 150 J O b. zero O c. 100 J O d. There is not enough information to determine. O e. 200 J
91. ssm The pressure and volume of a gas are changed along the path ABCA. Using the data shown in the graph, determine the work done (in- cluding the algebraic sign) in each segment of the path: (a) A to B, (b) B to C, and (c) C to A. 7.0 x 105 3.0 x 105 2.0 x 10-3 5.0 x 10-3 Volume, m3 Pressure, Pa
Consider a 2.0 liter of an ideal gas expanding into a vacuum up to a volume of 4.0 liter. If 500 J of energy flows out of the container, is work done to or by the system? Explain.
statistical physics
a quantity ideal gas requires 800kj to raise the temperature of the gas by 10.0k when the gas is maintained at a constant volume. the same quantity of gas requires 900kj to raise the temperature of the gas by 10.0k when tha gas is maintained at a constant pressure. what is the adiabatic constant y for this gas?
A sealed cylinder has a piston and contains 8.90×103 cm3 of an ideal gas at a pressure of 7.50 atm. Heat is slowly introduced, and the gas isothermally expands to 1.70×104 cm3. How much work ? does the gas do on the piston?
All of the following are factors directly affecting the work by an ideal gas except:a. pressure in the initial and final stateb. heat transfer in the initial and final statec. thermodynamic path from initial to final stated. volume in the initial and final state
Q1) There are four main thermodynamic processes that you learned from Unit 3: isobaric, isochoric, isothermal, and adiabatic. For each process below, classify it has one of these processes and then determine the signs of Q (the heat energy that flows into the gas), W (the work done by the gas), and AU (the change in internal energy of the gas). a) A container filled with an ideal gas has been submerged in a large water bath for a long time such that both reach thermal equilibrium. You then slowly compress the gas in the container. Assume the container is not well insulted so heat energy can easily flow back and forth between the water and gas and that the water bath is so large that its temperature does not change very much. b) A container filled with an ideal gas has a well-sealed piston that you put a pin in such that it doesn't move up or down. You then put the container over a burner to heat it up. c) A container filled with an ideal gas has a well-sealed piston that can move up or…
**33. ssm The drawing shows an adiabatically isolated cylinder that is divided initially into two identical parts by an adiabatic parti- tion. Both sides contain one mole of a monatomic ideal gas (y =), with the initial temperature being 525 K on the left and 275 K on the right. The partition is then allowed to move slowly (i.e., quasi-statically) to the right, until the pressures on each side of the partition are the same. Find the final temperatures on the (a) left and (b) right. 525 K- -275 K Partition
A sample of N molecules of ideal gas expands with no energy transferred into or out of the gas by heating. The pressure and volume of the gas are measured as it expands, and a graph of pressure as a function of volume is used to calculate the work done by the gas. Which of the following indicates a quantity for the gas that can be determined using the calculated work and justifies why it can be determined? Select two answers. The magnitude of the change in internal energy of the gas can be determined. If no energy is transferred by heating, the magnitude A of the change in internal energy equals the magnitude of the work done by the gas. The change in potential energy of the gas can be determined. The internal energy of the gas equals its potential energy plus its kinetic energy, and the magnitude of the change in kinetic energy of the gas equals the work done by the gas. The magnitude of the change in the average kinetic energy of a molecule of the gas can be determined. The magnitude…
Which one of the following statements is true about a sealed ideal gas system? You can increase the internal energy of the system without increasing its temperature. To raise the temperature of the system, you must add heat. No work occurs during a constant-pressure process. In an adiabatic process, no energy leaves or enters the system. In an isothermal process, the internal energy of the system remains the same.