Physics ideal gases

posted by .

If 2 samples of nitrogen (different PVTs) are separated by a conductive barrier, they will eventually achieve equilibrium, I believe.

Am I right to assume that the final T and P at equilibrium in this case would be the SAME T and P if the barrier was highly insulated, then removed allowing equilibrium to happen.


  • Physics ideal gases -

    In one case the process is at equilibrium at every step and reversible.
    In the other case you have a sudden mixing. I would not assume the same U change for both cases.

  • Physics ideal gases -

    But I would if the gases do no work in case 1. If no work is done and the system is totally isolated from the surroundings so that no heat can pass in or out, then the initial and final states will be the same.

  • Physics ideal gases -

    If the pressures are not the same then when the barrier is removed, you get a free expansion of the gasses. When equilibrium is reached, the total internal energy will be the same as in the original state.

    It follows from this that the final pressure is given by

    P = (P1 V1 + P2 V2)/(V1+V2)

    Here P is the final pressure, P1 and P2 are the initial pressures, V1 and V2 are the volumes of the two parts.

    In case of a conductive barrier, only the temperatures will equalize. The total internal energy also stays the same. Equal final temperatures means that the final pressures are related according to:

    P_fin1 V1 = P_fin2 V2

    Conservation of energy then implies:

    P1 V1 + P2 V2 = 2 P_fin1 V1 --->

    P_fin1 = 1/2 (P1 V1 + P2 V2)/V1

    P_fin2 = 1/2 (P1 V1 + P2 V2)/V2

  • Physics ideal gases -

    Thank you both.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Econ MC

    Externalities cause markets to a. fail to allocate resources efficiently. b. cause price to be different than the equilibrium price. c. benefit producers at the expense of consumers. d. cause markets to operate more equitably. I think …
  2. Physics ideal gases

    Would someone check my thinking please. PVT of an ideal gas (nitrogen) are all given. I've used PV=nRT rearranged to get the number of moles. Then, U= 3/2nRT to get the internal energy of the sample. Am I on the right track?
  3. chemistry

    The gas phase reaction between nitrogen gas and oxygen gas to give NO gas is an endothermic process since 180.8 kJ of heat energy is absorbed when 1 mol of nitrogen reacts with 1 mol of oxygen. In which direction will the equilibrium …
  4. AP Chemistry- Equilibrium

    If 10.0 mL of 0.18 M MgCl2 are mixed with 20.1 mL of 0.56 M NaOH, what will be the final concentration of Mg2+ in solution when equilibrium is established?
  5. chemistry calculations

    At 25 deg C, Kc is 5.84x10-3 for the dissociation of dinitrogen tetraoxide to nitrogen dioxide. N2O4(g) ==== 2NO2(g) a) Calculate the equilibrium concentration of both gases when 4.00 grams of N2O4 is placed at 2.00-liter flask at …
  6. a level chemistry

    two most abundant atmospheric gases react to a small extent at 298K in the presence of a catalyst to achieve dynamic equilibrium: N2(g) + O2(g) ->/<- 2NO(g) Kp= 0.30 Partial pressure of N2 and O2 = 0.78atm 1dm3 flask and equilibrium …
  7. Physics

    A container is initially partitioned by a wall into two compartments. The left compartment has volume V1 and the right compartment has volume V2. Both compartments are filled with identical ideal gases at the same temperature T and …
  8. chem12

    for the equilibrium 2HI(g)--- H2(g) + I2 k eq = 8.0 2.0 mol of HI are placed in a 4.0 L container, and the system is allowed to reach equilibrium. Calculate the equilibrium concentration of all three gases. Inital 2HI 0.5mol/l H2 =0 …
  9. Chemistry

    The equilibrium constant, K, for the following reaction is 1.54×10-2 at 506 K: PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 15.7 L container at 506 K contains 0.207 M PCl5, 5.64×10-2 M PCl3 and 5.64×10-2 …
  10. Chemistry

    The equilibrium constant is equal to 5.00 at 1300K for the reaction 2SO2(g) + O2(g) <--> 2SO3(g) if initial concentrations are [SO2] = 6.00M, [O2] = 0.45M, [SO3]= 9.00M, the system is a/. At equilibrium b/. Not at equilibrium …

More Similar Questions