How does temperature and pressure effect concentration?

Question

revircs · Answer

https://gyazo.com/6adcdfe7e83a015a8681cb2548fffa7e I really dont see how temperature and pressure can change concentrations...

photon336 · Answer

Yeah , you notice that there are more moles on the reactant side right? than the product side. so if you increased the pressure the reaction is going to go to the side with fewer number of moles i.e. the products. @Revircs

photon336 · Answer

The concentration of the products would go up, concentration of reactants down.

kainui · Answer

I think it might help to look at the equation of an ideal gas since after all we're dealing with gasses!

$$pV=nRT$$

Now we see that temperature and pressure are coming into play, but where is the concentration?

What is concentration? Well usually it's recorded in Molarity, which is moles per liter. $ M = \frac{ mol}{L}$. If you look carefully you'll notice that $n$ is number of moles and $V$ is liters, so by dividing both sides of our ideal gas equation by V we get:

$$p=\frac{n}{V} RT$$

We could just write the concentration as $C=\frac{n}{V}$ (C for concentration. I just made it up to make it clearer which part is the concentration, it's not some standard thing as far as I know but it might be) to get:

$$p=CRT$$

So now you can answer questions about how changing temperature and pressures affect concentration if you want that equality to remain the same I hope!