# Ideal gas problem

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?

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#### 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.