# 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?

Feb 13, 2016

I fond: $1029.7 m l$

#### Explanation:

Considering the gas as ideal we can use:
$P V = n R T$
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:
${P}_{1} {V}_{1} = n R {T}_{1}$
to:
${P}_{2} {V}_{2} = n R {T}_{2}$

But $n$ and $P$ remain unchanged so we have that:
$\frac{{V}_{1}}{T} _ 1 = n \frac{R}{{P}_{1}}$
$\frac{{V}_{2}}{T} _ 2 = n \frac{R}{{P}_{1}}$
and so:
$\frac{{V}_{1}}{T} _ 1 = \frac{{V}_{2}}{T} _ 2$

But:
${T}_{1} = 273 + 25 = 298 K$
${T}_{2} = 273 + 50 = 323 K$
and:
${V}_{2} = \frac{950 \cdot 323}{298} = 1029.7 m l$