Question

A sample of N2O gas has a density of 2.697 g/L at 298 K. What must be the pressure of the gas (in mmHg)?

Answer 1

Answer:

$P=1139.16384mmHg$

Explanation:

Given data

$R=0.08206(\frac{L.Atm}{mol.K} )\\Density=2.697g/L\\Temperature=298K\\f.wt=44(g/mol)$

To find

Pressure

Solution

From Ideal gas law we know that

$PV=nRT\\P=(nR\frac{T}{V} )=(R(\frac{mass}{f.wt} )(\frac{T}{V} ))\\P=R(\frac{mass}{volume}) (\frac{T}{f.wt} )=R(Density)(\frac{T}{f.wt} )$

Substitute the given values to find pressure

So

$P=(0.08206\frac{L.Atm}{mol.K} )(2.697g/L)(298K)(44g/mol)^{-1}\\ P=1.4989Atm$

Convert Atm to mmHg

Multiply the pressure values by 760

So

$P=1139.16384mmHg$