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Welcome to our Physics lesson on Relationship between the Volume of Ideal Gas and the Number of Molecules. The Avogadro's Law, this is the fourth lesson of our suite of physics lessons covering the topic of Gas Laws, you can find links to the other lessons within this tutorial and access additional physics learning resources below this lesson.
So far, we have assumed the amount of gas as constant in all processes discussed. Now, let's suppose we add some extra gas in the container by keeping both pressure and temperature constant.
If the gas is ideal, no collisions between particles occur. Therefore, an additional amount of gas (which means an extra number of molecules) simply brings an increase in volume of gas if no change in the other parameters does occur. This phenomenon was first explained by Avogadro, so the relationship between the volume of ideal gas and the number of its molecules is known as the Avogadro's Law. Its mathematical expression is
where n is the number of moles.
Avogadro's Law is intended for ideal gases but it is valid for real gases if the values of pressure and temperature are low.
From experiment, it has been found that one mole of an ideal gas occupies 22.4 L of volume at normal temperature and standard atmospheric conditions.
A balloon contains 0.125 moles of an ideal gas at normal conditions. If an additional amount of gas is added to the balloon, its volume becomes 11.2 L. How many moles of gas were added in the balloon?
First, we find the initial volume of gas given the conversion factor
We have
Thus,
Now, using the Avogadro's Law, we obtain for the final number of moles n2:
Thus, the amount of gas added in the balloon is
You have reached the end of Physics lesson 13.9.4 Relationship between the Volume of Ideal Gas and the Number of Molecules. The Avogadro's Law. There are 4 lessons in this physics tutorial covering Gas Laws, you can access all the lessons from this tutorial below.
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