Find the Amount of Excess Reactant (+ Example)
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- เผยแพร่เมื่อ 23 ส.ค. 2024
- How much of the EXCESS reactant is left over?
* Find the limiting reactant. The OTHER reactants are in excess.
* Use mole ratio to see how much of the excess reactant is used up
* Subtract that from the original amount of excess reactant
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Your comment changed my life.
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OMG thank you so much watched three vids so far, with at least an hour of work, and this 5 min vid helped more than anything.
Bro...... What the heck! You made the formula looks so easier!
Calculating moles was a heck of a ride, not until I found different video giving the simplest formula.
Why can't we have this simple formulas instead of making a long and complicated one?
This was really helpful bro
Hats off
you saved my life, thank you so much
Great video!
Please make another video about this 5opic
Does this work for problems other than finding just grams? Such as finding the amount of moles?
Very grateful for this clear explanation, thank you
Can you share where to find your print out of periodic table please
this still makes no sense
ur so real
I’d pack you in a fight
Are u dumb bruh?!
😂😂
Just because this more of something doesn't mean it is in excess.
For example lets say you are making a cheese sandwich which needs 2 slices of bread and 1 slice of cheese. If you had something like 8 slices of bread and 5 slices of cheese you would only be able to make 4 sandwiches before running out of bread.
Even though we had more slices of bread it was the ingredient that caused us unable to make sandwiches.
Now apply the same idea to chemistry.
If for example you had 3 grams of hydrogen gas and 16 grams of oxygen gas let's see how much water we can make.
The balanced equation for water is 2H2 + O2 --> 2H2O
So if you convert that into moles
3g/2.0M = 1.5 mol of hydrogen
16g/32M = 0.5 mol of oxygen
Then divide by 1.5 by 2 because there are 2 moles of hydrogen reacting per mole of oxygen. This nets you 0.75 moles
Compared 0.75 to 0.5 the oxygen is lower which means it is the limiting reactant.
Even though we had much more grams of oxygen than hydrogen it was still the thing that limited the reaction!
I hope this comment helped you understand this concept more!
Thankkkk youuu mister
thank you sir🙏🙏🙏
Shoudnot we take hydrigen molarmass 4 because we have 2 moles of 2h
Nope its a mistake lots of students make you need to ignrore any number b4 the reaction
Thank you so much sir.
Thanks mate
❤
i have no brain
im traumatised
AAAAAAAAA
Guys how is h2 is limiting reactant
Its 1.5 its higher than 0.95 huh???
After dividing by stoichiometry coefficients,it's 0.75, which is less than 0.90