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Can someone help me understand why the side with more molecules necessarily refers to more pressure? Is it just because those molecules are taking up more space? I think i am just confused with the concept of pressure in general. Thank you!
According to the ideal gas law, PV = nRT, P = nRT/V = concentration (=n/V) * RT. So [partial pressure = concentration * RT].
Shutong Hou_1F wrote:According to the ideal gas law, PV = nRT, P = nRT/V = concentration (=n/V) * RT. So [partial pressure = concentration * RT].
The way I see it is concentration is moles per liter which means the more moles, the higher the Molarity or Concentration, and as said in the comment above, partial pressure = concentration * RT (R being a constant and T being the temperature) so the larger the concentration, the more partial pressure.
More molecules would essentially mean less volume. The more particles you add into an empty flask, the less empty space there is. Since there is less volume, the pressure in the flask will increase. This is demonstrated through the inverse relationship between pressure and volume and the equation P=nRT/V.
When there are more molecules, the particles collide with one another and the container more frequently, resulting in higher pressure. Thus, when applied to Le Chatelier's, if the pressure of the system is increased, the reaction will shift in a direction that will alleviate this added pressure, which would be in the direction that produces less moles of gas.
In lecture Professor Lavelle said that you can increase pressure by decreasing volume, but then he also said you can increase pressure in some other way. How else can you increase pressure in a system? Would increasing concentration achieve that based on the comments in this post. Thank you.
How does Le Chatliers Principle apply to the concept of pressure?
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