Question

A sample of fluorine has a volume of 2.3 L when the temperature is -7.4 degC and the pressure is 830 torr. What will be the volume when the pressure is 78.55 kPa and the temperature is 104.2 degrees Celsius?

Answer 1

`V=39.914L`

Step-by-step explanation:

Hello,

Starting by the ideal gas law which always involves absolute temperatures:

`PV=nRT`

At the initial given conditions, the moles are computed, assuming they are constant:

`n=(PV)/(RT)= (830torr*(1atm)/(760torr) *2.3L)/(0.082(atm*L)/(mol*K) *(-7.4+273.15)K)=0.1153mol`

Now, by solving for the volume at the new pressure and temperature we get:

`V=(nRT)/(P)=(0.082(atm*L)/(mol*K) *377.35K)/(78.55kPa*(1atm)/(101.325kPa)) =39.914L`

Best regards.