1. Not finding help here? Sign up for a free 30min tutor trial with Chegg Tutors
    Dismiss Notice
Dismiss Notice
Join Physics Forums Today!
The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

Yet another pressure/volume/temp question. (no fishes!)

  1. Dec 23, 2004 #1

    Mo

    User Avatar

    Hello all, looking for some expert guidance again please! ill just get straight into it;

    The Question
    A fixed mass of gas has an initial volume v0 (v subscript 0) and an initial pressure p0 .It is first compressed at a constant temperature of 27C until its volume is reduced to [tex]1/4 [/tex]v0 State the pressure of the gas, in terms of p0, at the end of this process. The temperature of the gas is now increased until its volume returns to v0. Throughout this process, the gas is allowed to expand in such a way that its pressure remain constant.Calculate the final temperature, in C of the gas.


    My answer (brace yourself!)

    a) Boyle's law states that

    [tex]p . v = c[/tex] So we can deduce that if the volume were to be reduced to a quarter of its original value, then the pressure will increase four-fold.

    i.e 4p0 . [tex]1/4 v0[/tex] (4p0 multiplied by one quarter of v0)

    b)For this part we know that the pressure = 4p . For the volume to return to its original value, it must be multiplied by 4. (and this is where i get it completely wrong .. well maybe a bit before this!) .so

    27 + 273 = 300 K

    300 X 4 = 1200.
    1200 -273 = 927 C

    Now that seems incredibly high to me.Im positive i have gone wrong somewhere.Please enlighten me!

    Regards,
    Mo

    ps: Should i have converted the temperature to kelvins? if not then the answer would be 108 C. i could be using the wrong forumla even ..
     
    Last edited: Dec 23, 2004
  2. jcsd
  3. Dec 23, 2004 #2

    dextercioby

    User Avatar
    Science Advisor
    Homework Helper

    If the gas is assumed to be ideal,note IDEAL,then it obeys certain simple laws.On of then states that,if a certain process is isobar,then:
    [tex] (\frac{V}{T})_{1}=(\frac{V}{T})_{2} [/tex]
    ,which includes the ABSOLUTE TEMPERATURE,MEASURED IN KELVINS.
    The tempertures will be 300K the first one,and 1200K the final one.
    Again,this is an IDEAL gas,at 1200K,a REAL gas will be partly ionized,and the laws of physics will be different.

    Daniel.
     
  4. Dec 23, 2004 #3

    Mo

    User Avatar

    Thank you for your response.

    I gather that this question is talking about ideal gases, since these are the question directly after that chapter.

    In an exam situation how would i know though? Would they tell me, or could i say .. "assuming the gas is an ideal gas .." (i doubt they would give me anything that is not an ideal gas since i have not yet learnt any formulas for REAL gases .. i dont think ..)

    So .. my answers were correct. 1200K ? So in Celsius this is 927 C .

    Thanks again for your reply.

    Regards,
    Mo
     
  5. Dec 23, 2004 #4

    dextercioby

    User Avatar
    Science Advisor
    Homework Helper

    You're welcome! :smile:


    If the problem does not specifically say:"ideal/real gas",then it would be smart to chose the simpler case and simply write on the paper:"Assuming the gas is ideal,then..." :tongue2:

    Yes.Again,u're welcome to post any problems u have.

    Daniel.
     
Know someone interested in this topic? Share this thread via Reddit, Google+, Twitter, or Facebook

Have something to add?



Similar Discussions: Yet another pressure/volume/temp question. (no fishes!)
  1. Pressure temp volume (Replies: 3)

Loading...