For Le Chatelier and Kc, no you don't have to learn all the industrial examples. There are some that you need to know conditions for from other topics that they might tie in to an equilibrium point of view. But mostly the industrial aspect of this will come in the form of an unfamiliar situation, and you'll have to work out what would happen and justify it
Glad it's useful! This isn't meant for a specific syllabus. I teach AQA at my school and I've made sure it fully meets that. There may be a tiny bit of difference between exam boards but not much
Yes indeed. Optical Isomers is coming out soon. I have question walkthroughs for a lot of year 2 content as well, e.g. Thermodynamics, Arrhenius Equation etc
hello sir at 16:50 , there was a similar question im doing to this on a paper regarding the decrease in pressure, for that equilibrium what affect would SO3 have on the yield and why ? i thought it would increase even though i understand it shifts to the left but i do not understand why the mark scheme says that the yield of so3 would decrease!
If you decrease pressure eqm shifts to the side with more moles of gas in order to increase the pressure again. So I'd assume that in the exam question there were more moles on the left side?
@@chemistrytutor yes the left hand side has more moles (3) while the right hand side had less moles(2), im just confused on why then the yield of the right side would increase
@17:40 so wether or not the system will be actually shift to oppose change depends on the ratio of moles of reactants to moles of products? Or in other words if they're equal on both sides, the system won't be able to shift to oppose change? @20:20 does this mean that the side with less moles is automatically lower in pressure no matter the size of the molecules?
Well explained, and yes to both. 1) when pressure is changed, equilibrium will only shift if it can reverse the change by doing so (which depends on mole ratios) 2) we assume all gases behave ideally, so one mole of any gas at the same temp and volume will exert the same pressure
I am now starting to enjoy Chemistry because of your vids. Thank youu so muchhh
Thats so lovely to hear! Thank you for the feedback!
for real
I was wondering for AQA do we have to learn all the industrial examples or just one?
For Le Chatelier and Kc, no you don't have to learn all the industrial examples. There are some that you need to know conditions for from other topics that they might tie in to an equilibrium point of view. But mostly the industrial aspect of this will come in the form of an unfamiliar situation, and you'll have to work out what would happen and justify it
you're the best. thank u so muchhh! also, is this for the cie syllabus?
Glad it's useful! This isn't meant for a specific syllabus. I teach AQA at my school and I've made sure it fully meets that. There may be a tiny bit of difference between exam boards but not much
can you please make videos for all as topics and a2 please
Yes indeed. Optical Isomers is coming out soon. I have question walkthroughs for a lot of year 2 content as well, e.g. Thermodynamics, Arrhenius Equation etc
hello sir at 16:50 , there was a similar question im doing to this on a paper regarding the decrease in pressure, for that equilibrium what affect would SO3 have on the yield and why ? i thought it would increase even though i understand it shifts to the left but i do not understand why the mark scheme says that the yield of so3 would decrease!
If you decrease pressure eqm shifts to the side with more moles of gas in order to increase the pressure again. So I'd assume that in the exam question there were more moles on the left side?
@@chemistrytutor yes the left hand side has more moles (3) while the right hand side had less moles(2), im just confused on why then the yield of the right side would increase
@MariamNuhu-fc9vz It wouldn't. If eqm shift left, the yield of whatever is on the right goes down
@@chemistrytutor oops I understand now I made a silly mistake thanks sir!
@17:40 so wether or not the system will be actually shift to oppose change depends on the ratio of moles of reactants to moles of products?
Or in other words if they're equal on both sides, the system won't be able to shift to oppose change?
@20:20 does this mean that the side with less moles is automatically lower in pressure no matter the size of the molecules?
Well explained, and yes to both.
1) when pressure is changed, equilibrium will only shift if it can reverse the change by doing so (which depends on mole ratios)
2) we assume all gases behave ideally, so one mole of any gas at the same temp and volume will exert the same pressure