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)?

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Answer 1 · 2017-06-02T04:06:37

1.58 Atm

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

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

A sample of N_2ON_2O gas has a density of 2.85 g/L at 298 K. What must be the pressure of the gas (in mmHg)?