# To what temperature does 1.36 L of hydrogen originally at 25.0°C need to be heated in order to bring the volume to 2.5 L?

May 7, 2018

${T}_{2}$ = ~45.96C

#### Explanation:

$\left({V}_{1} / {T}_{1}\right) = \left({V}_{2} / {T}_{2}\right)$

$\left(\frac{1.36}{25}\right)$ = $\left(\frac{2.5}{T} _ 2\right)$

Cross-multiply.

1.36${T}_{2}$ = 62.5

Divide by 1.36 to isolate for ${T}_{2}$.

$\frac{62.5}{1.36}$ = ${T}_{2}$

${T}_{2}$ = 45.95588235294C