# How would you find the number of grams of CO2 that exert a pressure of 785 torrs at a volume of 32.5 L and a temperature of 32 degrees C?

Jun 6, 2018

$\text{58.96 g}$

#### Explanation:

Use ideal gas equation

$\text{PV = nRT}$

$\text{n" = "PV"/"RT}$

color(white)("n") = "785 torr × 32.5 L"/"62.36 L torr / mol K × (32 + 273) K"

color(white)("n") = 1.34\ "mol"

Mass of ${\text{CO}}_{2}$ is

$\text{m" = 1.34 cancel"mol" × 44 "g"/cancel"mol" = "58.96 g}$