9 FOR A THERMODYNAMIC CYCLE TO BE REVERSIBLE, THE FOLLOWING MUST BE SATISFIED: For a thermodynamic cycle to be reversible, the following must be satisfied: when heat is being absorbed, temperature of hot source and working sub-stance should be same free expansion or friction resisted expansion/compression process should not be encountered when beat is being rejected, temperature of cold source and working sub-stance should be same none of the above. all of the above 00000

9 FOR A THERMODYNAMIC CYCLE TO BE REVERSIBLE, THE FOLLOWING MUST BE SATISFIED: For a thermodynamic cycle to be reversible, the following must be satisfied: when heat is being absorbed, temperature of hot source and working sub-stance should be same free expansion or friction resisted expansion/compression process should not be encountered when beat is being rejected, temperature of cold source and working sub-stance should be same none of the above. all of the above 00000

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

Chapter13: Spontaneous Processes And Thermodynamic Equilibrium

Section: Chapter Questions

Problem 39P

See similar textbooks

Similar questions

For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
Explain why the statement No process is 100 efficient is not the best statement of the second law of thermodynamics.
Calculate rS for each substance when the quantity of thermal energy indicated is transferred reversibly to the system at the temperature specified. Assume that youhave enough of each substance so that its temperatureremains constant as the thermal energy is transferred. (a) H2(g), 0.775 kJ/mol, 295 K (b) KCl(s), 500. kJ/mol, 500. K (c) N2(g), 2.45 kJ/mol, 1000. K
Explain why absolute entropies can be measured.
Liquid water at 25C is introduced into an evacuated, insulated vessel. Identify the signs of the following thermodynamic functions for the process that occurs: H, S, Twater, Ssurr,, Suniv.
What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?
The enthalpy of vaporization for water is 40.65 kJ mol-1. As a design engineer for a project in a desert climate, you are exploring the option of using evaporative cooling. (a) If the air has an average volumetric heat capacity of 0.00130 J cm-3 K-1, what is the minimum mass of water that would need to evaporate in order to cool a 5 m? 5 m room with a 3 m ceiling by 5°F using this method? (b) Is this a spontaneous or nonspontaneous process?
at if Hess’s law were not true? What are some possible repercussions this would have?
The standard enthalpy of formation of H2O(l) at 298 K is 285.8 kJ/mol. Calculate the change in internal energy for the following process at 298 K and 1 atm: H2O(l)H2(g)+12O2(g)E=? (Hint: Using the ideal gas equation, derive an expression for work in terms of n, R, and T.)
Under what conditions will U be exactly zero for a process whose initial conditions are not thesame as its final conditions?
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.