Skip to content
Showing 1 to 2 of 2
Anyone fancy explaining the concept of equilibriums for Higher Chemistry? (The idea of equilibriums shifting to the right/left, etc ) I can't seem to get my head around it.
If the change that has occured means that there is more of one thing, the position of the equilibrium will move to oppose the change. So it will use up more of the thing there is now more of and make more of the other thing. So if we had A + B in equilibrium with C + D + E and we increased the concentration of C, the equilibrium would move to make more of C, D and E because the C will be more likely to react and produce more of the A + B . Or if we increased the pressure, the equilibrium would try to reduce the pressure by moving to the side with fewer moles of gas. Lets assume all of A, B, C, D, and E are gaseous. The equilibrium would move to make more of A + B because that would reduce the overall nuber of moles and therefore reduce the pressure. Basically, the equilibrium wants to keep the same conditions and concentrations of reactants and products if possible, so when a change occurs, it moves to wherever will leave the smallest difference to the origional conditions. If you are still unsure, there is quite a good youtube video on this topic http://www.youtube.com/watch?v=4-fEvpVNTlE Try that too.
Hope that isn't too confusing and it helps.