A certain heat engine operates on the PV diagram below. It contains 3.21mol of a monatomic ideal gas. p(Pax 105) 2.0 a b - V(m³) 0 0.010 0.040 a. What temperature is the gas at state c? b. What temperature is the gas at state a? c. How much heat is added/removed from the gas over the path c-to-a? d. What is the pressure of state a? e. What is the temperature of state b? f. Find the work and heat for path a-to-b. g. Find the work and heat of path b-to-c. h. Find the efficiency of the engine. i. Would the engine be more, or less efficient if the gas were diatomic?

A certain heat engine operates on the PV diagram below. It contains 3.21mol of a monatomic ideal gas. p(Pax 105) 2.0 a b - V(m³) 0 0.010 0.040 a. What temperature is the gas at state c? b. What temperature is the gas at state a? c. How much heat is added/removed from the gas over the path c-to-a? d. What is the pressure of state a? e. What is the temperature of state b? f. Find the work and heat for path a-to-b. g. Find the work and heat of path b-to-c. h. Find the efficiency of the engine. i. Would the engine be more, or less efficient if the gas were diatomic?

University Physics Volume 2

18th Edition

ISBN:9781938168161

Author:OpenStax

Publisher:OpenStax

Chapter2: The Kinetic Theory Of Gases

Section: Chapter Questions

Problem 34P: (a) What is the gauge pressure in a 25.0 cc car tire containing 3.60 mol of gas in a 30.0-L volume?...

See similar textbooks

Similar questions

(a) Calculate the work done by the gas along the closed path shown below. The curved section between R and S is semicircular. (b) If the process is carried out in the opposite direction, what is the work done by the gas?
In a cylinder of an automobile engine, immediately after combustion the gas is confined to a volume of 50.0 cm3 and has an initial pressure of 3.00 106 Pa. The piston moves outward to a final volume of 300 cm3, and the gas expands without energy transfer by heat, (a) What is the final pressure of the gas? (b) How much work is done by the gas in expanding?
(a) How much heat transfer occurs to the environment by an electrical power station that uses 1.251014J of heat transfer into the engine with an efficiency of 42.0%? (b) What is the ratio of heat transfer to the environment to work output? (c) How much work is done?
In a cylinder, a sample of an ideal gas with number of moles n undergoes an adiabatic process. (a) Starting with the expression W=PdV and using the condition PV = constant, show that the work done on the gas is W=(11)(PfVfPiVi) (b) Starting with the first law of thermodynamics, show that the work done on the gas is equal to nCV(Tf Ti). (c) Are these two results consistent with each other? Explain.
2 mole of a monotomic ideal gas is taken along the path abc as shown in the figure. If the gas was taken from a to c along the horizon dashed line instead (a) What is the work done by the gas?(b) How much heat is transferred into or out ofthe gas?(c) What is the internal energy change?
An ideal gas is enclosed in a cylinder with a movable piston on top of it. The piston has a mass of 8,000 g and an area of 5.00 cm2 and is free to slide up and down, keeping the pressure of the gas constant. (a) How much work is done on the gas as the temperature of 0.105 mol of the gas is raised from 30.0°C to 325°C?? J(b) What does the sign of your answer to part (a) indicate? The surroundings do positive work on the gas. There is no work done, by the gas or the surroundings. The gas does positive work on its surroundings.
Figure shows a pV-diagram for an ideal gas in which its absolute temperature at b is one-fourth of its absolute temperature at a. (a) What volume does this gas occupy at point b? (b) How many joules of work was done by or on the gas in this process? Was it done by or on the gas? (c) Did the internal energy of the gas increase or decrease from a to b? How do you know? (d) Did heat enter or leave the gas from a to b? How do you know?
In the pV diagram shown in the figure (Figure 1), 80.0 J of work was done by 0.0610 mole of ideal gas during an adiabatic process. a) How much heat entered or left this gas from a to b? Express your answer in joules. b) By how many joules did the internal energy of the gas change? Express your answer in joules. c) What is the temperature of the gas at b? Express your answer in kelvins.
An ideal gas is enclosed in a cylinder with a movable piston on top of it. The piston has a mass of 8,000 g and an area of 5.00 cm2 and is free to slide up and down, keeping the pressure of the gas constant. (a) How much work is done on the gas as the temperature of 0.280 mol of the gas is raised from 25.0°C to 260°C? J(b) What does the sign of your answer to part (a) indicate? The surroundings do positive work on the gas.There is no work done, by the gas or the surroundings. The gas does positive work on its surroundings.
After an isobaric process, the enthalpy of 28g of CO gas, increases by 2700 J. The initial temperature of the CO gas is 20◦C. Assume CO is an ideal gas. (a). What is the final temperature?(b). By how much did the thermal energy of CO change?