Two one-liter containers each contain 10 moles of a gas. the temperature is the same in both containers. container a holds helium (molecular mass = 4 u), and container b holds oxygen (molecular mass = 16 u). which container has the higher pressure and by what factor?

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I18ntech I18ntech · Answer 1 · 2018-08-01T14:12:08+02:00

Using the Ideal gas equation,

[tex] PV=\frac{n}{m}RT [/tex]

Here, P is pressure of the gas

V is the volume of the gas,

n is number of moles,

R is universal gas constant, and

T is absolute temperature

As all the factors are the same for helium and oxygen gases except their molecular mass,

So, we can say that pressure exerted by the gases is inversely proportional to their molecular mass. That is,

[tex] \frac{P_{1}}{P_{2}}=\frac{m_{2}}{m_{1}} [/tex]

P₁= Pressure exerted by the helium gas

P₂= Pressure exerted by the oxygen gas

m₁= Molecular mass of helium gas = 4 u

m₂= Molecular mass of oxygen gas = 16 u

[tex] \frac{P_{1}}{P_{2}}=\frac{16}{4} [/tex]

[tex] \frac{P_{1}}{P_{2}} =4 [/tex]

The pressure exerted by the helium gas is more than that by oxygen gas by 4 times.