A community for students.
Here's the question you clicked on:
 0 viewing
anonymous
 3 years ago
If a pressure of gas is suddenly reduced and we let the gas to expand again until it reaches equilibrium. What is final volume, work done and heat in this process? and what would be change in internal energy?
Again the pressure is suddenly increased back to initial pressure and gas is compressed to initial volume. What would be work done heat and change in internal energy?
Temperature is same throughout all process
anonymous
 3 years ago
If a pressure of gas is suddenly reduced and we let the gas to expand again until it reaches equilibrium. What is final volume, work done and heat in this process? and what would be change in internal energy? Again the pressure is suddenly increased back to initial pressure and gas is compressed to initial volume. What would be work done heat and change in internal energy? Temperature is same throughout all process

This Question is Open

anonymous
 3 years ago
Best ResponseYou've already chosen the best response.0The attempt at a solution Here All the process is done at isothermal condition so Boyles law apply P1V1=P2V2 where V2 is volume after the gas comes to equilibrium, so, V2=P1V1/P2 since the process is carried in isothermal condition ΔU=0 w=p*ΔV 0=q+p*ΔV > q=p*ΔV Now when the pressure is increased back to initial condition ΔU=0 ( since process is still isothermal) ΔU=q+p*ΔV > q=p*ΔV, here change in volume is volume after decreasing pressure  initial volume I am not sure if I am correct or not? Help
Ask your own question
Sign UpFind more explanations on OpenStudy
Your question is ready. Sign up for free to start getting answers.
spraguer
(Moderator)
5
→ View Detailed Profile
is replying to Can someone tell me what button the professor is hitting...
23
 Teamwork 19 Teammate
 Problem Solving 19 Hero
 Engagement 19 Mad Hatter
 You have blocked this person.
 ✔ You're a fan Checking fan status...
Thanks for being so helpful in mathematics. If you are getting quality help, make sure you spread the word about OpenStudy.