In the previous post, we talked about partial pressures and the Dalton law. Today, we will see how the mole fraction and partial pressures of a gas are related. Remember, mole fraction (Χ) is the ratio of the moles of … Read more
To understand the partial pressures, let’s suppose a certain amount of gas “A” is added to a tank and exerts 5 atm pressure, and in another tank with gas “B” the pressure is 3 atm: Now, it turns … Read more
The mixing of different gas molecules by random molecular motion and frequent collisions is called diffusion. An example of this can be the raid odor spread of perfume when the stopper is removed. Effusion is a similar process in which … Read more
Density and molar mass are calculated by modifying the ideal gas law equation. What we do is first replace the moles (n) in PV = nRT with mass over the molar mass: … Read more
The combined gas law is obtained by rearranging the ideal gas law, from PV = nRT. From this, we obtain an expression for the R: \[{\rm{R}}\; = \;\frac{{{\rm{PV}}}}{{{\rm{nT}}}}\] Now, because R is constant, this expression is true for … Read more
The ideal gas laws show the correlation of the temperature, pressure, volume, and the amount of a gas. Although, this is not how the laws were determined, I found my students grasping the concepts a lot easier using the following … Read more
