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Bulb A is 100mL and contains Helium at 1atm.
Bulb B is 500ml and contains Argon at 2atm
The bulbs are connected together by a valve.
(assume constant temperature).

What is the total pressure of the system after the valves are opened?

  • Chemistry -

    The long way to do this, but the easier way to explain, is this.
    Use PV = nRT for bulb A and solve for n = mols He.
    Then use PV = nRT for bulb B and solve for n = mols Ar.
    Add n He + n Ar = total n
    Then PV = nRT. Use total n and solve for P. (Note: you don't have a T listed so just use a convenient one but don't change it)

  • Chemistry -

    Would the total pressure be 2.19985 atm? Could you possibly help me with this one?

  • Chemistry -

    No, that isn't right.
    What's the problem with plugging in the numbers? For example, for He, you can use
    PV = nRT.
    n = PV/RT
    n = 1*0.1/(0.08206*300)
    n = 0.00406

    For Ar.
    n = PV/RT = 2*0.500/(0.08206*300)
    n = 0.406
    Total n = 0.0406+0.00406 = 0.0446

    Then p = nRT/V = 0.41*0.08206*300/0.600
    P = ?

    You can also do this a much shorter way by using P1V1 = P2V2
    For He that is P2 = P1V1/V2
    P2 He = 1*(100/600) = 0.167
    P2 Ar = 2*(500/600) = 1.67
    Total P = 0.167+1.67 = ?

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