Midterm 1 Question 2

[106046096]

Hi! I just wanted to ask why the answer to question 2 on Midterm 1 would be false. If you are increasing the pressure of a system, wouldn't you favor the side with fewer moles to generate a lower pressure? Can someone please explain thank you!

[Andrew Rizk]

Since you are pumping in Helium, an inert gas, it does not affect the formation of products or reactants. Lavelle mentioned this during lecture that an inert gas won't affect it.

[Bryan Lee 2L]

Inert gases don't affect equilibrium. Since an inert gas doesn't react with the reactants or the products, it has nothing to do with the equilibrium. Equilibrium is simply just the ratio of the concentration of reactants and products, so any changes that don't affect the reactant/product whatsoever will do nothing.

[Lexi Brownsberger 2E]

To add on to this, when inert gases are pumped into a sealed container, they simply sit in the occupied area without interacting with products and reactants, acting as a bystander. Since they are not involved in any interaction, they will have no impact on pressure. Remember that this only applies if the gas is inert!