Question

a closed container contain 56 grams of N2 and 20 gram of helium if partial pressure of N2 is 1 ATM then find total pressure of the gas molecules in the container​

Answer 1

Answer:

Explanation:

The pressure exerted by the gasses is directly proportional to moles.

$\frac{PN2}{PHe}= \frac{number of moles of N2}{Number of moles of He}$

$\frac{1}{PHe}= \frac{\frac{56}{28} }{\frac{20}{4} }$

on solving, we get

Pressure exerted by Helium = 2.5 atm

Total pressure exerted by gasses = 1 atm + 2.5 atm = 3.5 atm

Answer 2

The total pressure exerted by gas molecules in the container=1.4 atm

Explanation:

Given mass of nitrogen=56 g

Given mass of helium=20 g

Partial pressure of nitrogen=1 atm

We know that

Partial pressure exerted by gas is directly proportional to number of moles.

Number of moles=$\frac{Given\;mass}{molar\;mass}$

Mass of nitroge($N_2$)=28 g

Mass of helium=4g

$\frac{P_{N_2}}{P_{He}}=\frac{\frac{56}{28}}{\frac{20}{4}}=0.4$

$\frac{1}{P_{He}}=0.4$

$P_{He}=0.4 atm$

By Dalton's law of partial pressure

$Total\;pressure=P=P_{N_2}+P_{He}$

$P=1+0.4=1.4 atm$

Hence, the total pressure exerted by gas molecules in the container=1.4 atm.

#Learns more:

State Dalton's law of partial pressure

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