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?

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?

1 Answer

Impact of this question

12675 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2016-02-13T18:46:13

I fond: $1029.7 m l$ $1029.7ml$

Explanation:

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

But $n$ $n$ and $P$ $P$ remain unchanged so we have that:
$\frac{V_{1}}{T_{1}} = n \frac{R}{P_{1}}$ $(V_1)/T_1=nR/(P_1)$
$\frac{V_{2}}{T_{2}} = n \frac{R}{P_{1}}$ $(V_2)/T_2=nR/(P_1)$
and so:
$\frac{V_{1}}{T_{1}} = \frac{V_{2}}{T_{2}}$ $(V_1)/T_1=(V_2)/T_2$

But:
$T_{1} = 273 + 25 = 298 K$ $T_1=273+25=298K$
$T_{2} = 273 + 50 = 323 K$ $T_2=273+50=323K$
and:
$V_{2} = \frac{950 \cdot 323}{298} = 1029.7 m l$ $V_2=(950*323)/298=1029.7ml$

Science

Math

Humanities

... and beyond

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?

1 Answer

Explanation:

Related questions

Impact of this question