Question

A sample of `N_2O` gas has a density of 2.85 g/L at 298 K. What must be the pressure of the gas (in mmHg)?

Answer 1

1.58 Atm

Explanation:

From Ideal Gas Law (PV = nRT)

`P = (nRT/V) = (R("mass"/"f.wt")(T/V))`

`P = R("mass"/"Volume")(T/"f.wt.")`= `R("Density")(T/"f.wt.")`

Given:
`R = 0.08206("L-Atm"/"mol-K")`
`"Density" = 2.85(g/L)`
`T = 298K`
`f.wt. = 44(g/"mol")`

`P = (0.08206"L-Atm"/"mol-K")(2.85g/L)(298K)(44g/"mol")^-1 = 1.58Atm`