Answered: For the reversible isobaric expansion… | bartleby

Related questions

Question

2)
For the reversible isobaric expansion from V, to V2 of an ideal gas inside a frictionless piston-cylinder
system with heat-conductive walls: (AU)sys = q + w = CPAT - pAV. This process can be performed by
slowly raising the temperature of the surroundings from T1 to T2 while holding the pressure of the
surroundings constant. Show that for this type of process, AU can also be given as: (AU)sys=CvAT.

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Blurred answer

Similar questions

The temperature at state A is 20.0ºC, that is 293 K. During the last test, you have found the temperature at state D is 73.0 K and n = 164 moles for this monatomic ideal gas. What is the work done by the gas for process D to B, in MJ (MegaJoules)? 1.0 atm = 1.00 × 105 Pa.
In a constant-volume process, 208 J of energy is transferred by heat to 1.07 mol of an ideal monatomic gas initially at 303 K. (a) Find the work done on the gas. (b) Find the increase in internal energy of the gas. (c) Find its final temperature. K
The molar heat capacities at constant volume of Ne and N2 at 298 K are 12.47 J mol-1 K1 and 20.79 J mol-1 K-1 respectively. Give an explanation of these values based on statistical mechanics.
In an isochoric process, one mole of an ideal gas of rigid diatomic molecules at volume V is taken from an initial temperature T to a final temperature 4T. Using the convention that heat is positive when it is absorbed by the system, what is the heat transfer in terms of R and T?
A cylinder containing n mol of an ideal gas undergoes an adibatic process. Starting with dW = pdV and using the condition pVY = constant, show that the work done by the gas: 1 W × (p;V; - PfV¢) %3D Starting from the first law of thermodynamics in differential form, prove that the work done by the gas is n×Cy(T; - Tf).
Combustion products in a gas turbine expand adiabatically from a pressure of 4 bar and a temperature of 880ºC to a pressure of 1 bar and a temperature of 550ºC. Assuming the reversible path 1-b-2 and that the process 1-b is adiabatic, determine the ∆s. Consider the value of Cp = 1 J / g K
A flexible box contains 5.60 grams of nitrogen gas (N2) which is maintained at a constant pressure of 1.35 x 10$ Pa. The box is placed over a fire, causing the volume to increase from 0.00200 m3 to 0.00300 m³. Find the increase in temperature of the gas. (For N2 molar mass M = 28 grams.)
One mole of an ideal gas, for which CV,m = 3/2R, initially at 298 K and 1.00 × 10^5 Pa undergoes a reversible adiabatic compression. At the end of the process, the pressure is 1.00 × 10^6 Pa. Calculate the final temperature of the gas. Calculate q, w, ΔU, and ΔH for this process.
A cylinder with a piston contains 0.150 mol ofnitrogen at 1.80 * 105 Pa and 300 K. The nitrogen may be treated as anideal gas. The gas is first compressed isobarically to half its originalvolume. It then expands adiabatically back to its original volume, andfinally, it is heated isochorically to its original pressure. (a) Show theseries of processes in a pV-diagram. (b) Compute the temperatures atthe beginning and end of the adiabatic expansion. (c) Compute theminimum pressure. Use the conditions and processes of the problem above tocompute (a) the work done by the gas, the heat added to it, and its internal energy change during the initial compression; (b) the work done by the gas, the heat added to it, and its internal energy change during the adiabatic expansion; (c) the work done, the heat added, and the internal energy change during the final heating.