An airplane is pressurized with air to 660 mmHg . If air is 21% oxygen, what is the partial pressure of oxygen on the plane?

The partial pressure of oxygen on the plane is 138.6 mmHg

Explanation:

To calculate the partial pressure of the gas, we use the equation given by Raoult's law, which is:

where,

= partial pressure of oxygen gas = ?

= total pressure = 660 mmHg

= mole fraction of oxygen gas = 21 % = 0.21

Putting values in above equation, we get:

Hence, the partial pressure of oxygen on the plane is 138.6 mmHg

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.