# Question #9dcb3

Mar 24, 2017

No

#### Explanation:

The law that explains the relationship between Volume and Temperature is Charles's Law.

$\textcolor{w h i t e}{a a a a a a a a a a a a a a a a a} \frac{{V}_{1}}{{T}_{1}}$ = $\frac{{V}_{2}}{{T}_{2}}$

Another law, The Ideal Gas Law** is the condensed version of all the gas laws.

PV = nRT

$P = \text{pressure (atm)}$
$V = \text{volume (L)}$
$n = \text{moles}$
$R = \text{Gas constant 0.082 (L*atm)/(mol*K)}$
$T = \text{temperature (K)}$

If all else stays same, pressure and mass, then if Volumes increases, so will Temperature.

First convert Celsius to Kelvin

${T}_{1} = {25}^{\circ} \to 298 K$
${T}_{2} = {50}^{\circ} \to 323 K$

• ${T}_{2} / {T}_{1} = \left(323 \cancel{\text{K")/(298 cancel"K}}\right) \to 1.08$

Since the Temperature increased by a factor of $1.08$, the Volume will also increase by the same factor.

The volume won't double because we have to convert Celsius to Kelvin first. Be careful on that as you may have been tempted to say the volume doubled, but keep in mind the Ideal Gas Law uses Kelvin and not Celsius in its equation.