Draw the graphs and explain both positive deviations from ideal behaviours?
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hiiii mate ☺️☺️
your solution is attached with the picture.....
We already know the Ideal Gas Equation pV= nRT. It defines the relationship between Temperature, pressure, and volume of gases. For checking the reliability of this relationship we first plot a graph between pV and p. Now we know that at a constant temperature, as the Boyle’s law states, pV shall be a constant. Therefore the graphs between the two (p and pV) shall be a straight line. But the case is not so! At temperature 273 K the data for several gases is shown in the graph below:
From the graph plotted in the figure we can easily conclude that despite the constant temperature, the real gases do not show behaviour as predicted by the Boyle’s law. These gases show a significant deviation from the predicted ideal behaviour as per the Boyle’s law. The plot in the graph signifies the deviating behaviour of real gases like Dihydrogen, Helium, Carbon monoxide and Methane from the behaviour of ideal gas. In faact we see, from the graph that real gases do not show any signs of similar to Ideal gas’s behaviour.
From our next graph that plots the volume to pressure data of gases, we find an apparent deviation from the theoretical prediction of gases in changed conditions. From the graph, we can figure out that at very high pressures the value of volume we calculated is less than the actual practical volume. Hence from the above two graphs, it is clear that generally real gases, under all conditions do not follow The Ideal Gas Behaviour or equation.
hope it helps you ✌️✌️
Qᴜᴇsᴛɪᴏɴ♧︎︎︎
Draw the graphs and explain both positive deviations from ideal behaviours?
Aɴsᴡᴇʀ♧︎︎︎
Your answer is in ☝︎ pictures
Exᴘʟᴀɴᴀᴛɪᴏɴ☘︎
Ideal Gas Equation pV= nRT. It defines the relationship between Temperature, pressure, and volume of gases. For checking the reliability of this relationship we first plot a graph between pV and p. Now we know that at a constant temperature, as the Boyle’s law states, pV shall be a constant. Therefore the graphs between the two (p and pV) shall be a straight line. But the case is not so! At temperature 273 K the data for several gases.
Hope it helps you ✌️
