The ideal gas law describes the relationship between a gas’s pressure P, volume V, and temperature T. The Ideal Gas Law calculator helps you understand these relationships. Another name for The ideal gas law is the Perfect Gas Law.
An ideal gas has molecules that don’t attract or repel each other and don’t take up any volume. No gases in real life are exactly ideal, but some gases may behave close to an ideal gas at high temperatures and very low pressures.
So, the ideal gas law is used to solve stoichiometry problems in chemical reactions involving gases. It is also used to determine the densities of gases.
Using the ideal gas law calculator, you can calculate the pressure, volume, temperature, and also the amount of the gas.
The variables in the calculator include
Pressure (p) For the gas pressure, we specifically have to use Absolute Pressure for the calculation.
Volume (V) The volume occupied by the gas
Number of Moles (n) The number of moles of gas
Temperature (t) The absolute temperature of the gas, for the calculation, the unit should be in Kelvin
We can obtain The Ideal Gas Law relationship by the following formula
Where,
R = Ideal Gas Constant, its value is 8.31446261815324 J/mol K
The ideal gas law describes the relation between pressure, volume, temperature, and also the amount of gas.
As the name suggests, this law describes the behavior of ideal gases, which does not exist, but some gases exhibit quite closely the properties of an ideal gas at high temperatures and low pressures.
The assumptions made for the ideal gas are as follows.
Gases are made up of a large number of tiny particles approximated as point particles that can be considered to have negligible volume.
No forces interact on the gas particles, and they only interact with each other through elastic collisions.
When the gas particles collide with other gas particles for the walls of the container, the collisions are elastic collisions where there is no net loss of kinetic energy.
The gas particles are moving in random motion, and Newton’s laws of motion possess kinetic energy due to this motion.
The average kinetic energy of the gas particles depends upon the temperature of the gas.
Based on the experiments performed on various gases to understand their behavior led to these three relationships.
The volume V is proportional to the number of moles. So, if you double the number of moles (n), keeping the pressure and temperature constant, the volume doubles.
Volume V varies inversely with pressure. So, if we double the pressure while holding the temperature T and the number of moles n constant, the volume is halved.
The pressure is proportional to absolute temperature. So, if we double the temperature keeping the volume and number of moles constant, the pressure doubles.
The above three relationships are put together to give us the ideal gas law
Note: We have to use the absolute pressure, not the gauge pressure, for the calculation. Similarly, the temperature T is the absolute temperature Kelvin and not Celsius.
R here is the proportionality constant of the ideal gas equation.
The pressure of a gas can be calculated using the Ideal Gas Law and rearranging the terms shown below
The volume of a gas can be calculated using the Ideal Gas Law and rearranging the terms shown below
The temperature of a gas can be calculated using the Ideal Gas Law and by rearranging the terms shown below
The amount of a gas can be calculated using the Ideal Gas Law and rearranging the terms shown below
The ideal gas law is derived from the kinetic theory of gases, which describes the behavior of gases in terms of the motion and interactions of their particles. The ideal gas law is a generalization of both Boyle’s and Charles’ laws as special cases.
The ideal gas law assumes that the gases are composed of point particles that do not interact with each other except for perfectly elastic collisions. It also assumes that the volume of the particles themselves is negligible and that no forces are interacting with the gas particles, like attraction or repulsion.
According to the ideal gas law, an increase in temperature will cause an increase in the pressure and volume of a gas, assuming the number of particles and the volume of the container are held constant. This is due to the increased kinetic energy of the gas particles at higher temperatures.
If the temperature (T) is doubled, keeping the volume and number of moles constant, the pressure (p) doubles.
According to the ideal gas law, an increase in pressure will cause a decrease in the volume of a gas, assuming the temperature and number of particles are held constant. This is due to the increased force exerted by the gas.
If the pressure (p) is doubled, keeping the temperature (T) and the number of moles (n) constant, The volume is halved.
