1.50 mol of an ideal gas with a constant ratio of heat capacities at constant pressure and volume y == 1.40 is taken through the (reversible) cycle shown in the figure below. The process A → B is an expansion at constant temperature, whereas B → C and C → A are constant-pressure compression and constant-volume processes, respectively. a) What is the temperature TA of the gas at A? P (atm) For the cycle as a whole, Isothermal b) calculate the (net) work done W (by the gas), process c) calculate the (total) heat transfer Q,

1.50 mol of an ideal gas with a constant ratio of heat capacities at constant pressure and volume y == 1.40 is taken through the (reversible) cycle shown in the figure below. The process A → B is an expansion at constant temperature, whereas B → C and C → A are constant-pressure compression and constant-volume processes, respectively. a) What is the temperature TA of the gas at A? P (atm) For the cycle as a whole, Isothermal b) calculate the (net) work done W (by the gas), process c) calculate the (total) heat transfer Q,

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 22P

See similar textbooks

Similar questions

Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special cart to move them around. An80.0-Ltank ofnitrogen gas pressurized to 172 atm is left in the sun and heats from its normal temperature of 20.0C to 140.0C. Determine a the final pressureinsidethe tank and b the work, heat, and U of the process. Assume that behavior is ideal and the heatcapacity of diatomic nitrogenis 21.0J/mol.K.
The Dieterici equation of state for one mole of gas is p=RTe-aVRTV-b Where a and b are constants determined experimentally. For NH3g, a = 10.91 atm. L2 and b = 0.0401 L. Plot the pressure of the gas as the volume of 1.00 mol of NH3g expands from 22.4 L to 50.0 L at 273 K, and numerically determine the work done by the gas by measuring the area under the curve.
A 5-mmdiameter hailstone has a terminal velocity of10.0m/s. Assuming its mass is6.031025 kg and all of its kinetic energy turns into heat, calculate the temperaturechangeof the hailstone when it hits the ground and stops. The heat capacity of ice is 2.06J/g.K.
Benzoic acid, C6H5COOH, is a common standard used in bomb calorimeters, which maintain a constant volume. If 1.20 g of benzoic acid gives off 31, 723 J of energy when burned in the presence of excess oxygen and in a water bath having a temperature of 24.6 C, calculate q, w, H, and U for the reaction.
Use the two appropriate values of R to determine a conversion between L. atm and J.
Assume that 1.20 g of benzoicacid, C6H5COOH, is burned in a porcelain dish exposed to the air.If 31, 723 J of energy is givenoff andthe surrounding temperature is 24.6C, calculate q, w, H,and U. Compare your answers to those from the previousproblem.
What are the numerical values of the heat capacities c-v and c-p of a monatomic ideal gas,in units of cal/mol.K and L.atm/mol.K?
What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?
If the heat capacity varies withtemperature, abetter form ofequation 2.9 isto solve q=TiTfnCT-t A 50.0-g sample of white phosphorus is heated from 298 K to 350K. If its molar heat capacity is CT- = 56.990.1202T J/mol.K, how much heat is needed?
Show that = T/p for an ideal gas.
Explain why the high-temperature reservoir of a heat engine must, indeed, be higher in temperature than the low-temperature reservoir. Can it ever be the other way around?
Use the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions necessary.