22:00 this part has been overcomplicated - Just write the Mass and Mr and Moles on the left side of the equation and work your way toward - simply using mol = M/Mr by rearranging Everything else is great thanks
It looks like it. The spec he put at the beginning links with the current OCR A one. Obviously note that the Gas Constant which he uses is wrong for OCR A, it is meant to be 8.314Jmol−1K−1 as stated in the OCR A Data sheet
I know this is late but for anyone wondering: A mole is 6.02 x10^23 atoms/molecules; in this case molecules. 1 mole of CO2 means that there are 6.02 x10^23 molecules. And as there’s only 1 C atom in a molecule there’s 6.02 x10^23 C atoms. For oxygen there would be 12.04x10^23 atoms because there’s O2 in CO2
30:40, I don't understand how C can have the same number of moles as CO2- if they do, wouldn't that mean O has no value? Since C has taken all the moles? As the Mr of CO2 was used. I'm confused and if someone could clear this up for me, I would be grateful.
i know this was posted 2 years ago, but just for anyone reading this and who is also confused: this is because a mole is just 6.022 × 10^23 numbers of particles. so since we have a mole amount of CO2, which is CO2 x (6.022 × 10^23), that means we've multiplied 1 particle of C by (6.022 × 10^23) and also 1 particle of O2 by (6.022 × 10^23), hence we have a mole of C and a mole of O2. I hope it makes sense.
because then the number of S particles would need to be split in half too, leaving you with K S0.5 O2, I hope it now makes sense why K2 S O4 is the simplest way to write it :D
Just me or anyone else just really sucks at converting to m3 for the ideal gas equation? Im pretty good at everything maths related but i just always get confused with it
I'm a bit confused I thought atom economy was the mass of atoms in the desired product over the mass of atoms in the reactants. Do both formulas work? Can you please clarify.
He explained in 36 minutes and yet my teacher spent 3 weeks and nothing went inside my brain
absolutely precise
YESS
Literally
I’m not even gonna lie.. you helped me at A-Level & now im watching your videos in Pharmacy school for a refresh 🎉
2.1.2 0:00-11:07
2.1.3 11:07 onwards
these revision vids are so helpful.. many thanks Chris
You're welcome!
I cannot thank you enough sir, you've made the lives the of many.
You are very welcome
mate, these are bloody brilliant! clear and easy to follow, best tutorials I've ever watched!
Helping me pass chemistry one video at a time, thanks Chris!
actually getting me through chemistry during this quarentine, thank you
You're welcome!
I was revising when I realized the date. HAPPY 5TH ANNIVERSARY OF THIS VIDEOOO!!! Thank you for all your help :'))))))
Thank you so much one mental breakdown later this video has helped calm me down. I think I can actually pass. :)
If I get an A in chemistry, it will be because of these videos
Did you get an A?
Thank you so much this video was super helpful!!!
Really great video, thanks a lot!
I salute you Allery best for final quick straight to the point revision, Chem paper 1 8th June wish me luck
Thanks. Hope the exam goes well on the 8th 👍
22:00 this part has been overcomplicated - Just write the Mass and Mr and Moles on the left side of the equation and work your way toward - simply using mol = M/Mr by rearranging
Everything else is great thanks
23:50 we could've also found out the number of moles and went from there right?
Is this the new spec? Thanks c:
It looks like it. The spec he put at the beginning links with the current OCR A one. Obviously note that the Gas Constant which he uses is wrong for OCR A, it is meant to be 8.314Jmol−1K−1 as stated in the OCR A Data sheet
Great stuff sir!
To convert g/dm-3 into mol/dm- 3, do you just divide by the Mr?
Ben Vincent, Yes, if it isn't too late lol.
Ben Vincent yepp
Yes, you divide by the Mr of the substance ( a bit late but it might help others )
i love u to bits man
@ 30:00 isn't the mol which is 0.019 spread across the whole CO2, not just the C.
I know this is late but for anyone wondering: A mole is 6.02 x10^23 atoms/molecules; in this case molecules. 1 mole of CO2 means that there are 6.02 x10^23 molecules. And as there’s only 1 C atom in a molecule there’s 6.02 x10^23 C atoms.
For oxygen there would be 12.04x10^23 atoms because there’s O2 in CO2
Thank you for this really informative video , it really helped in my revision
Glad it was helpful!
you are amazing!!
30:40, I don't understand how C can have the same number of moles as CO2- if they do, wouldn't that mean O has no value? Since C has taken all the moles? As the Mr of CO2 was used. I'm confused and if someone could clear this up for me, I would be grateful.
I'm guessing that its because the oxygen has no mass, hence all of the moles would come from the C atom in the C02 compound
i know this was posted 2 years ago, but just for anyone reading this and who is also confused: this is because a mole is just 6.022 × 10^23 numbers of particles. so since we have a mole amount of CO2, which is CO2 x (6.022 × 10^23), that means we've multiplied 1 particle of C by (6.022 × 10^23) and also 1 particle of O2 by (6.022 × 10^23), hence we have a mole of C and a mole of O2. I hope it makes sense.
wait so all those coke cans i got with my burger meals were cans of carbon?
at 18:26, for the question in the purple box, why don't you use the equation mol = vol/24 given the question tells us we're at room temp and pressure?
i have my exam tomorrow ill come back when I get my results!
Hope it goes well 👍
Bro did not come back
When calculating the moles and goimg through esch stage of calculations do we have to roujd or can we use exact values until final answer
Would the Ca2O2 simplify to 2CaO or just CaO?
I may be a bit late here, but is % yield always in grams and the mass, or can you do it with moles too? Thanks
i've seen loads of past questions that does it with moles too.
Hey Chris or anyone who sees this comment, time stamp 21:41
I still don't really understand, is anyone able to reexplain?
why is this different from the textbook, in the textbook 2.1.2 is atomic structure and 2.1.3 is atomic masses
Different exam boards?
MY GOATTTTT
Question: potassium sulphate has the formula K2SO4 - why cant you simplify this down to KSO2
because then the number of S particles would need to be split in half too, leaving you with K S0.5 O2, I hope it now makes sense why K2 S O4 is the simplest way to write it :D
the goat
Just me or anyone else just really sucks at converting to m3 for the ideal gas equation? Im pretty good at everything maths related but i just always get confused with it
when do you do 100/x or x/100
I'm a bit confused I thought atom economy was the mass of atoms in the desired product over the mass of atoms in the reactants. Do both formulas work? Can you please clarify.
Why you coming fast?