Example 1
Determine the volume of `1.00\ mol` of any gas, assuming it behaves like an ideal gas, at `STP`.
Given:
`n = 1.00\ mol`
`T = 273 K`
`P = 1.013 times 10^5\ N//m^2`
Known: `R = 8.314\ J//mol•K`
Equation: `PV = nRT`
Solutions:
`V = (nRT)/P = ((1.00\ mol)(8.314\ J//mol•K)(273 K))/(1.013 times 10^5\ N//m^2)`
`V = 22.4 times 10^(-3)\ m^3`
Almost `1\ mol` of any gas has a volume of
`22.4\ L (22.4 times 10^(-3)\ m^3)`
at STP