A vessel contains 1.60 g of oxygen and 2.80 g of nitrogen. The temperature is maintained at 300 K and the volume of the vessel is 0.166 m 3 . Find the pressure of the mixture.

Question

Philoid · Accepted Answer

Given

Mass of oxygen gas =1.60g

Mass of nitrogen gas =2.80g

Temperature of vessel=300K

Volume of vessel=0.166m³

We know that

Number of moles n=

Molar mass of oxygen= 32g/mol

Molar mass of nitrogen=28g/mol

Number of moles of oxygen n₁ =

Number of moles of nitrogen n₂=

We know ideal gas equation

PV=nRT

Where V= volume of gas

R=gas constant=8.31Jmol^-1K^-1

T=temperature

n=number of moles of gas

P=pressure of gas

In a mixture of non-interacting ideal gases, the pressure that a gas in a mixture of gases would exert if it occupied the same volume as the mixture at the same temperature is called the partial pressure of that gas.

Partial pressure of oxygen gas

Partial pressure of nitrogen gas

According to Dalton’s law of partial pressure, the total pressure of a mixture of ideal gas is the sum of partial pressures.

So, total pressure

P=P_o+P_N =750+1500=2250Pa

The pressure of the mixture of oxygen and nitrogen gas is 2250Pa.

A vessel contains 1.60 g of oxygen and 2.80 g of nitrogen. The temperature is maintained at 300 K and the volume of the vessel is 0.166 m3. Find the pressure of the mixture.

A vessel contains 1.60 g of oxygen and 2.80 g of nitrogen. The temperature is maintained at 300 K and the volume of the vessel is 0.166 m³. Find the pressure of the mixture.