Find the Amount of Excess Reactant (+ Example)

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

[@normalhumanbeing6066]

This video has changed my life. My whole outlook on everything that exists in this world, in fact even in the entire universe. I can never look at anything I know the same way ever again. This video represents emotions most humans could never comprehend. But I can. Thanks to this video I have been awakened to many things previously thought unimaginable. Thank you.

[@chemistNATE]

Your comment changed my life.

[@idkdikdidkd]

bot or what

[@particleex6428]

Your video changed my life. I'm so glad that you make videos like these, I would not be alive otherwise. I hope your channel flourishes and you never need to work another day in your life
(from @Orion)

[@cucumberboi945]

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.

[@neeuqollav2224]

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?

[@ArnavThakur-dq8jl]

This was really helpful bro
Hats off

[@thingsb4sleep]

you saved my life, thank you so much

[@GodSahil]

Great video!

[@southafricannewsroom]

Please make another video about this 5opic

[@nolansebring6786]

Does this work for problems other than finding just grams? Such as finding the amount of moles?

[@atomicshards]

Very grateful for this clear explanation, thank you

[@birbhadrajha3988]

Can you share where to find your print out of periodic table please

[@g3jusfly497]

this still makes no sense

[@aishahvora]

ur so real

[@wh1681]

I’d pack you in a fight

[@arpitapanchal6129]

Are u dumb bruh?!

[@M.i192]

😂😂

[@notdaycrucial5179]

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!

[@cilar7002]

Thankkkk youuu mister

[@AtharvNatu18]

thank you sir🙏🙏🙏

[@user-qq2bx3mk5i]

Shoudnot we take hydrigen molarmass 4 because we have 2 moles of 2h

[@omarora9516]

Nope its a mistake lots of students make you need to ignrore any number b4 the reaction

[@jaskaran8339]

Thank you so much sir.

[@user-tg8yv2ox9f]

Thanks mate

[@user-sr3iy5rk7m]

❤

[@viperdio69420]

i have no brain
im traumatised
AAAAAAAAA

[@user-tp8dg9qv6w]

Guys how is h2 is limiting reactant
Its 1.5 its higher than 0.95 huh???

[@rekham2083]

After dividing by stoichiometry coefficients,it's 0.75, which is less than 0.90