Explore BrainMass

Explore BrainMass

    Ideal gas problem

    This content was COPIED from BrainMass.com - View the original, and get the already-completed solution here!

    A certain gas cylinder A has a volume of 4.78 L and contains O2(g) at 927 mm Hg and a temperature of 25°C. A second gas cylinder B, with an unknown volume, contains Ne(g) at 25°C and a pressure of 898 mmHg. When the two cylinders are connected and the two gases are allowed to completely mix, the pressure in each cylinder becomes 907 mmHg. What is the volume of cylinder B in liters?

    © BrainMass Inc. brainmass.com October 9, 2019, 7:06 pm ad1c9bdddf

    Solution Preview

    We can solve this problem by using the ideal gas law. First we must convert the pressures to Pascals:

    760 mm Hg corresponds to 1 atmosphere and:

    1 atmosphere = 101325 Pa

    Converting the pressures to pascal gives:

    P_{O2} = 123.59*10^3 Pa

    P_{Ne} = 119.72*10^3 Pa

    P_{mixture} = 120.92*10^3 Pa

    The ideal gas law states:

    PV = N k T

    Here N is the number of molecules in the gas and k is Boltzmann's constant:

    k = 1.38065*10^(-23)J/K

    T is the ...

    Solution Summary

    A detailed solution is given.