1. Two moles of helium gas are placed in a cylindrical container with a piston. The gas is at room temperature 30 °C and under a pressure of 2.9 105 Pa. When the pressure from the outside is decreased; while keeping the temperature the same as the room temperature, the volume of the gas doubles. Use that the gas constant R= 8.31 J/(mol K). Think: What kind of process is this? Isobaric, isothermal, adiabatic, isochoric or non-quasi- static? (a) Find the work the external agent does on the gas in the process. Wext agent (b) Find the heat exchanged by the gas and indicate whether the gas takes in or gives up heat. Assume ideal gas behavior. Q=3492.27 O Q is realeased by gas O Q is absorbed by the gas

1. Two moles of helium gas are placed in a cylindrical container with a piston. The gas is at room temperature 30 °C and under a pressure of 2.9 105 Pa. When the pressure from the outside is decreased; while keeping the temperature the same as the room temperature, the volume of the gas doubles. Use that the gas constant R= 8.31 J/(mol K). Think: What kind of process is this? Isobaric, isothermal, adiabatic, isochoric or non-quasi- static? (a) Find the work the external agent does on the gas in the process. Wext agent (b) Find the heat exchanged by the gas and indicate whether the gas takes in or gives up heat. Assume ideal gas behavior. Q=3492.27 O Q is realeased by gas O Q is absorbed by the gas

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

17. 12.0 L. of an ideal gas at the pressure of 4.12 atm. is expanded against the external pressure of 2.55 atm. Calculate the work upon the expansion. The temperature is 312 K. Hint: This process is isothermal expansion. O 1910 ) O 2550 J O 1910 J O 585 kJ
1. Two moles of helium gas are placed in a cylindrical container with a piston. The gas is at room temperature 27 °C and under a pressure of 3.3.105 Pa. When the pressure from the outside is decreased, while keeping the temperature the same as the room temperature, the volume of the gas doubles. Use that the gas constant R = 8.31 J/(mol K). Think: What kind of process is this? Isobaric, isothermal, adiabatic, isochoric or non-quasi-static? (a) Find the work the external agent does on the gas in the process. W = ext. agent (b) Find the heat exchanged by the gas and indicate whether the gas takes in or gives up heat. Assume ideal gas behavior. Q= ✓J Q is realeased by gas Q is absorbed by the gas
The molar volumes of dry gas, measured at 200 °F, are given in TableQ2(a). i. Determine the coefficient of isothermal compressibility of the gas at 900 psia and 200 °F? (4 mark) ii. Compare your result with compressibility of an ideal gas at 900 psia and 200°F. (1 mark) TableQ2(a) Molar Volume (cu ft/lb Pressure, psi mole) 600 10.6 700 6.7 800 8.9 900 8.4 1000 8.1 1100 7.9 1200 7.8
A gas in a cylinder is held at a constant pressure of 2.20×105 Pa and is cooled and compressed from 1.90 m3 to 1.10 m3 . The internal energy of the gas decreases by 1.15×105 J. a) Find the work done by the gas. Express your answer in joules b)Find the amount of the heat that flowed into or out of the gas. Express your answer in joules to two significant figures. c) State the direction (inward or outward) of the flow.
1. Two monoatomic ideal gases A and B are at the same temperature. If 2 g of gas A has the same internal energy as 0.2 g of gas B. (a) Calculate the ratio of the number of moles of each gas. nA nв (b) Calculate the ratio of the atomic masses of the two gases. MA MB =
1. In a quasi-static isobaric expansion, 600 J of work are done by the gas. If the gas pressure is 0.7 atm, what is the fractional increase in the volume of the gas, assuming it was originally at 19 L? Use 1 atm≈ AV V 105 Pa & 1 L = 10-³ m³
1. An ideal diatomic gas at 63 K is slowly expanded adiabatically and reversibly to twice its original volume. What is its final temperature? Final temperature: K Think: Should the gas cool down or heat up during the adiabatic expansion? Does your answer validate your prediction.
1. A dilute gas at a pressure of 2.0 atm and a volume of 4.0 L is taken through the following quasi-static steps: (a) an isobaric expansion to a volume of 10.0 L, (b) an isochoric change to a pressure of 0.50 atm, (c) an isobaric compression to a volume of 4.0 L, and (d) an isochoric change to a pressure of 2.0 atm. Show these steps on a PV diagram drawn in your notebook and determine from your graph the net work done, Wgas by the gas. Use 1 atm~105 Pa and 1L = 10-3 m³. W gas
4. Ideal Gas Type Question: A piston comprises two nested cylinders which are 3 cm and 2.8 cm in diameter with 0.1 cm thick walls and are each 1 m long. Initially, the smaller cylinder sits completely inside the larger cylinder and is filled with N2 at 20 °C and atmospheric pressure. a. C. The gas is slowly heated, while the cylinder is allowed to freely expand. What kind of process is this? banc b. The smaller cylinder has a total mass of 1.5 kg. What temperature does the gas need to be for the cylinder to become fully extended? The cylinder can withstand an internal pressure of 20 atm. What's the maximum weight it can lift? e. d. A 100 kg weight is dropped on the cylinder while it is fully extended, causing it to rapidly compress. What kind of process is this? If the cylinder is fully depressed by this event, what is the peak pressure? The adiabatic constant for N2 is 7/5. f. If the weight is dropped from 2 m, assuming 1% of its energy is converted into thermal energy in the gas,…
1 8. Two moles of an ideal gas are heated at constant pressure from 27.0°C to 107°C. Calculate the work done by the gas. Draw the PV diagram for the process. (Answer: 1330 J)
1. In a quasi-static isobaric expansion, 550 J of work are done by the gas. If the gas pressure is 0.9 atm, what is the fractional increase in the volume of the gas, assuming it was originally at 16 L? Use 1 atm 105 Pa & 1 L = 10-³ m -3 3 AV ✓ V =