# At conditions of 785.0 torr of pressure and 15.0 °C temperature, a gas occupies a volume of 45.5 mL. What will be the volume of the same gas at 745.0 torr and 30.0 °C?

Jun 18, 2017

50.0ml

#### Explanation:

${P}_{1} = 785.0 \text{Torr}$ => ${P}_{2} = 745.0 \text{Torr}$
Decreasing Pressure => Increasing Volume (Boyles Law) => Use ratio of pressure values that decrease ${V}_{1}$. => (785.0/745.0)

${T}_{1} = \left(15 + 273\right) K = 288 K$ => ${T}_{2} = \left(30 + 273\right) K = 303 K$
Increasing Temperature (Charles Law) => Increasing Volume => Use ratio of temperature values that increase ${V}_{1}$. => (303/288)

${V}_{1} = 45.0 m l$ => V_2=?

${V}_{2} = 45.0 m l \times \left(785.0 \text{Torr")/(745.0"Torr}\right) \times \frac{303 K}{288 K}$ = $49.9 m l \implies 50.0 m l$