Question

In a gas cylinder a mixture of 40 % n2 ,35 % o2 and rest co2 produces a pressure of 700 mm hg. Calculate partial pressure of each gas .

Answer 1

finding the number of moles of each compound,

N2=40/28=1.43

O2=35/32=1.09

Co2=25/44=0.568

Now finding the mole fraction of each compound ,

for nitrogen---->

N2=nN2/nN2+nO2+nco2

$1.43 \div 1.43 + 1.09 + .568$

1.43/3.088=0.463

for oxygen--->

O2=nO2/nO2+nN2+nco2

=1.09/3.088=0.353

for carbon dioxide--->

co2=nco2/no2+nN2+nco2

=0.568/3.088.

=0.184

now using the formula,

partial pressure =mole fraction *total pressure

for N2----->

partial pressure =0.463*700

=324.1 mmhg

for O2------>

partial pressure =0.353*700

=247.1 mmhg

for co2----->

partial pressure =0.184*70.

=128.8 mmhg