How to Find How Much Excess Reactant Remains Examples, Practice Problems, Questions, Summary
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In this video, you'll learn how to find how much excess reactant is left by going through an example together.
The first step is to write a balanced chemical equation is one is not already given. Then, you'll have to figure out which reactant is limiting by convert both reactants into moles and dividing by the coefficients. Then you'll convert the limiting reactant into the grams of the excess reactant to figure out how much was consumed. Lastly, you'll subtract the amount consumed from how much was present initially.
By the end of this video, you'll know exactly how to find how much of the excess reactant remains.
If you liked my teaching style and are interested in tutoring, go to www.conquerchemistry.com/onlin...
Пікірлер: 70
Watching this during my chemistry unit test 🙏
@lolae.4562
2 жыл бұрын
same haha
@aniketdesale494
Жыл бұрын
Savage
@Joseph-hf9mi
Жыл бұрын
Exam*
@rod2662
Жыл бұрын
@Joseph they called it a unit test I wrote unit test
@heelylife
Жыл бұрын
How did you do
short, straight to the point video. helped me out within 5 mins
Wow. English is not even my language, and yet you're explaining way better than some french people💯thanks and good job👌🏽👍🏽
Dude! You are the freaking MAN! Thank you so much, helps like you wouldn't believe!
This was perfect. Understood it immediately
Love u sir o finally understood excess reagent
Thank you good sir, my chemistry teacher has been KZread and you are now one of many KZreadr teachers
a bit late but he got 1.49 by multiplying 3.5 g of O2 by 1 mol of O2 then dividing it by 32 g of O2 then repeat (remember to cancel out everything except the top right which is the 17.031 g of NH3 for you to come up with grams of NH3 in your final answer)
Can you pls explain gram to gram conversion properly
thank you for refreshing my memory!
Thankyou so much, you saved me 1 day before my test
Thank you very much, really appreciate it
How did you get 1.49 ?????I'm so lost there
@cakemonster3983
3 жыл бұрын
I was confused too but I found out that you should follow the formula. You multiply and divide the numbers regardless if it is grams or mol
Easy and helpful, thanks
How'd you get 1.49 g
omg bless this video is everything
Very helpful, thank you
How did u get 1.49 ?
thank youuuuu for this simple explanation ,
love you sir🥺 tomorrow will be my chemistry final test and you help me a lot!
@SI.COYG6
Жыл бұрын
how was it
THANK YOU SOOO MUCH!!!!
Watching this while doing my assignment due in the next hour. Tnx
amazing job i got the same chemical reaction 😂❤️❤️
How did you get the 1.49g, Please I dont know how?
thankyou sir you made it easy
ALL THE OTHER VIDEOS DO SOME WIERD SHIT AND DONT EXPLAIN< BUT YOU, YOUR A LEGENDDDD
How did you get the 1.49g
Explanation is just a quick but amazingly did it well and more informative than I expected!!
thanks this was easy to follow!
What if it’s in moles and not grams?
Thank youuuu
God bless you sir
Oh how did you get the 17.031?
From India🇮🇳
life saver
Is it possible to calculate for the excess amount of excess reagent if the problem only include the mass of only one reactant?
@jaysondebrah8359
2 жыл бұрын
Find the mass of the other one
U saved meeeeeeeee
1:02
Ty
I finawy figuwed out how to do dis
can I directly cut from their mols instead? I mean by the mol of excess minus the mol of limiting, to find the excess mass...?
@senthilpuliadi6599
2 жыл бұрын
No u can't
how do you calculate on the calculator to get 1.49 im lost
@carelessbear800
11 ай бұрын
multiply straight across and divide by the bottom 3.5g O2 / 32g O2 = 0.107 (0.107 x 4 )/ 5 = 0.0856 0.0856 x 12.031 = 1.49g NH3 how i remeber its like a zig zag. diviide given mass by its molar mass. Then multiple and divide by the mole ratio (multiple by numerator first then divide by denominator) and finally multiple by the grams. (dont really need to divde by 1. its a given what ur anwser would be) hope this helps anyone
30 minutes till my chemistry midterm
Thank you so much 🤍🌷
i wonder what youre up to these days? engineer? MD?
Everything in blue here is unnecessary. The only thing it can be used for is determining WHICH is the excess/limiting reactant. It gives no data of any real value later on. You can also determine WHICH is the excess reactant by just starting with everything that he wrote in purple. Compare the amount of NH3 "Consumed" when reacting with 3.5g O2 (1.49g NH3) to the amount of NH3 given in the experiment (3.25g NH3). The amount consumed is less than the amount given in the experiment, thus some of the NH3 would be left over. Thus it would be the excess reactant. This saves time because it identifies which reactant is in excess, as well as giving you real numbers that can be used to determine how much in excess the reactant actually is. Edit: I do realize that for someone being introduced to the topic, your way is probably better for them to learn. On a test however, especially a test on stoichiometry, this would be burning time that you really don't have.
watching 5 hrs before Chem exam fml
3.5 x 1/32 x 4 /5 x 12.031 / 1 = 1.053g NH3 am I wrong here?
@bendyaerial5940
4 жыл бұрын
sorry, 17.031 actually looks like 12.031
@meddlemedley740
4 жыл бұрын
@Bendyaerial he meant 17.031 but prob wrote the number like 2 on accident
@Manuxe
2 жыл бұрын
@@meddlemedley740 17.031 is a molar mass of what?
Goat
Great video. I was lost at the point where you had the 1.49g of NH3. That calculation is supposed to give 1.053g of NH3
@friendlytutor8891
2 жыл бұрын
I think you mistook 17.031 as 12.031. he was using 17.031 because that is that molar mass of NH3 :)
Very poor explanation
How did you get the 1.49g, Please I dont know how?