Question

A sample of argon gas occupies a volume of 950 mL at 25°C. What volume will the gas occupy at 50°C if the pressure remains constant?

Answer 1

I fond: `1029.7ml`

Explanation:

Considering the gas as ideal we can use:
`PV=nRT`
Where:
`P=` pressure;
`V=` volume;
`n=` number of moles;
`R=` universal gas constant;
`T=` temperature.
So pasically our gas undergo a transformation from equilibrium state 1 to equilibrium state 2 where we have:
from:
`P_1V_1=nRT_1`
to:
`P_2V_2=nRT_2`

But `n` and `P` remain unchanged so we have that:
`(V_1)/T_1=nR/(P_1)`
`(V_2)/T_2=nR/(P_1)`
and so:
`(V_1)/T_1=(V_2)/T_2`

But:
`T_1=273+25=298K`
`T_2=273+50=323K`
and:
`V_2=(950*323)/298=1029.7ml`