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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?

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sebassandin

Answer:

[tex]V=39.914L[/tex]

Explanation:

Hello,

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

[tex]PV=nRT[/tex]

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

[tex]n=\frac{PV}{RT}= \frac{830torr*\frac{1atm}{760torr} *2.3L}{0.082\frac{atm*L}{mol*K} *(-7.4+273.15)K}=0.1153mol[/tex]

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

[tex]V=\frac{nRT}{P}=\frac{0.082\frac{atm*L}{mol*K} *377.35K}{78.55kPa*\frac{1atm}{101.325kPa}} =39.914L[/tex]

Best regards.

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