R2.1.5 Atom economy
Mike Sugiyama Jones (MSJ Chem)
https://www.youtube.com/watch?v=Y9NVz7_9zw4

Transkript (automatisch erstellt)

0:00 this is msj CM in this video I'll be looking at atom economy here we have the equation for calculating percentage atom economy that appears in the IB data
0:11 booklet so that's percentage atom economy equals the molar mass of the desired product divided by the molar mass of all reactants multiplied by
0:22 100 there are other versions of the equation and they are atom economy equals mass of desired product divided by mass of all reactants multiplied by
0:32 100 and mass of desired product divided by mass of all products multiplied by 100 to calculate the atom economy for a reaction either one of these equations
0:45 can be used in this video I'll be using the top equation because this one appears in the IB data booklet next we look at an example ion
0:55 is produced by the reduction of ion oxide in a blast furnace Cal the atom economy of the reaction here we have the balanced
1:04 chemical equation for the reaction ion oxide reacts with carbon monoxide to form ion and carbon dioxide we'll start by finding the total
1:14 of all the molar masses of the atoms in the reactants so we have two atoms of ion so that's 2 multiplied by the molar mass of ion which is 55.8 5 we have six
1:26 atoms of oxygen so that's 6 multiplied by the mol mass of oxygen oygen which is 16. and we have three carbon atoms so that's 3 multiplied by the mol mass of
1:37 carbon which is 12.01 when we add these together we get a total of 243.166
2:00 us 11.7 next we'll use the equation to calculate the percentage atom economy
2:07 the total of the molar masses of our desired product which was ion is 11.7 the total of the molar masses of the reactants was
2:17 243.166 which I rounded to two significant figures this percentage atom economy
2:29 tells us that 54% by mass of the reactants do not end up in the desired product in other words they are wasted the higher the atom economy for a
2:40 chemical reaction the less waste is produced and the more efficient the reaction is