chem

If an ideal gas is allowed to expand into a vacuum, this means that the external pressure is 0. This doesn't affect the internal pressure though, correct?

For example:
I have a problem in which one mole of an ideal gas at 300. K and at a volume of 10.0 L expands isothermally into a vacuum, which doubles its volume. If I plugged these values into an equation, I would have:
0.00 atm x 10.0 L= 1.00 x .08206 x 300. L
Which doesn't work. So the pressure used in this equation is not 0, correct?

well the volume doubles, so it's now 20L. Since the problem provided you with everything but the correct pressure, you would be able to calculate the pressure by using PV=nRT. I calculated 1.24 atm or 936 torr.

you might want to double check me though. It's been a while since I've done ideal gases. :)

  1. 👍 0
  2. 👎 0
  3. 👁 142
asked by Chris

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    A sample of an ideal gas at 15.0 atm and 10.0 L is allowed to expand against a constant external pressure of 2.00 atm at a constant temperature. Calculate the work in units of kJ for the gas expansion. (Hint: Boyle's law applies)

    asked by Jack on October 4, 2010
  2. Chemistry

    A sample of an ideal gas at 15.0 atm and 10.0 L is allowed to expand against a constant external pressure of 2.00 atm at a constant temperature. Calculate the work in units of kJ for the gas expansion. (Hint: Boyle's law applies)

    asked by Jack on October 3, 2010
  3. thermodynamics and kinetics

    One mole of an ideal gas at 25C and 1 bar is allowed to expand adiabatically against a constant external pressure of 1.00 bar from 1.00 dm^3 to 10.00 dm^3. Calculate the final temperature, q, w, delta_U and delta_H.

    asked by Dorota on October 12, 2012
  4. Chemistry

    You have 1L of an ideal gas at 0 degree celsius and 10 atm pressure. You allow the gas to expand against a constant external pressure of 1 atm, while the temperature remains constant. Assuming, 101.3 J/liter-atm, find q,w,delta E,

    asked by John on November 25, 2011
  5. Chemistry

    Consider an ideal gas encloesd in a 1.00 L container at an internal pressure of 10.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 20.0 L. w = ____ J now

    asked by Eric on February 9, 2012
  6. chemistry

    An ideal gas is allowed to expand isothermally from 2.00 L at 5.00 atm in two steps: a) against a constant external pressure of 3.00 atm, followed by b) against a constant external pressure of 2.00 atm. Calculate q and w. (101.33

    asked by ace on November 14, 2012
  7. Chemistry

    Consider an ideal gas encloesd in a 1.00 L container at an internal pressure of 10.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 20.0 L. w = ____ J now

    asked by Lauren on February 10, 2012
  8. Physical Chemistry

    5. Assume you have a 45°C 100g block of gold (cp=0.129J/g°C) and a 150°C , 150g block of silver (cp=0.240J/g°C)(1). You place these blocks into an adiabatic container in thermal contact. a. Calculate the final temperature b.

    asked by Anonymous on September 10, 2016
  9. Chemistry

    By what factor does the volume increase when An ideal gas is allowed to expand from 3.80 L to 32.3 L at constant temperature

    asked by Dust on October 29, 2014
  10. chemistry

    An ideal gas is allowed to expand from 7.40 L to 55.5 L at constant temperature. By what factor does the volume increase?

    asked by Twon on October 27, 2011

More Similar Questions