The gas in which every molecule behaves autonomous of every individual molecule and has no excluded volume is called an ideal gas. Ideal Gas Law Formula is arithmetically articulated as:
P= Pressure of the gas
V=Volume of the gas
n= Amount of substance
R =ideal gas constant
T = Temperature
from which simpler gas laws such as Avogadro’s, Charles’s and Boyle’s law were derived.
One must highlight that this gas law is based on the ideal situation. As chemists, instructors, and scholars, we from time to time need to comprehend the concepts in advance before we can use them, and to suppose, unaffected by the real-world conditions, the gases are in an ideal state; it will help us better comprehend the behaviour the gases. Gas’ behaviour must follow the Kinetic-Molecular Theory to be ideal, whereas the Non-Ideal Gases will deviate from this theory due to real-world situations.
Problem 1: What is the temperature of One mole of CH4 gas that occupies 20.0L at 1.00atm pressure in Kelvin?
Answer the ideal gas law for T and put in the given values.
T = [1.00atm][20.0L]/[1mol][0.082]
T = 244K
Remember that under these conditions we computed the temperature for 1.00 mol of CH4 gas. The solution would be similar for 1.00 mol of NH3, N2, CO2 or any other gas underneath these settings.