Crap, last post 50 days ago! Doesn't vce go fast!!
Having a hard time getting my head around the effects of changing pressure in a reaction;
So apparently, with any change in pressure, the reaction will oppose it by moving to the side with less gas particles. Not sure what it means by 'moving to the side with less gas particles'. Does it mean just move to the side of the reaction with less coefficients?
Don't understand the whole theory of pressure vs reaction
So for the pressure factor (it's related to volume factor as well): according to Le..... (bleh, I never know how to spell his name, but whatever).
For eg, if I have PCl3 + Cl2 <=> PCl5
assume constant temperature, if we double the pressure, we halve the volume and hence we have increase the concentration of each gas (amount/volume). Think of it like the negative feed back system (since you did Bio
), the system will try to partially negate the "stimulus" by partially decrease the concentration of each gas/unit (i.e decrease the pressure). For this particular equation, the RHS only has 1 molecule and the LHS and 2 molecules. As a result, the system responds by favouring the forward reaction in an attempt to partially reduce the concentration of the LHS species until equilibrium is regained.
You can also think of it by using CF value:
CF = [PCl5] / ( [PCl3] x [Cl2] ) = Kc
when you introduce a change (halve volume => double concentration)
CF = 2[PCl5] / ( 2 [PCl3] x 2 [Cl2] ) = 1/2 [PCl5]/[PCl3]x[Cl2] => which is half of the original Kc value, hence CF < Kc. Hence, the system will try to equilibrate by increasing the CF value, by producing more PCl5 at the expense of PCl3 and Cl2. Hence, forward reaction is favoured.