Це відео не доступне.
Перепрошуємо.
How To Calculate Theoretical Yield and Percent Yield
Вставка
- Опубліковано 24 кві 2015
- This video shows you how to calculate the theoretical and percent yield in chemistry. The theoretical yield is the maximum amount of product that can be produced in a reaction. The percent yield is equal to the actual yield divided by the theoretical yield times 100%.
Full-Length Math & Science Videos:
/ collections
___________________________________
Introduction to Moles:
• Introduction to Moles
How To Calculate The Molar Mass:
• How To Calculate The M...
How To Convert Grams to Moles:
• How To Convert Grams T...
How To Convert Moles to Grams:
• How To Convert Moles t...
Moles to Atoms Conversion:
• Moles To Atoms Convers...
Grams to Molecules Conversion:
• Grams to Molecules and...
_________________________________
Grams to Atoms:
• How To Convert Grams t...
Moles, Atoms, & Grams Conversions:
• How To Convert Between...
How To Balance Chemical Equations:
• How To Balance Chemica...
Stoichiometry - Basic Introduction:
• Stoichiometry Basic In...
Avogadro's Number:
• Avogadro's Number, The...
_________________________________
Limiting Reactant Problems:
• Limiting Reactant Prac...
Excess Reactant Problems:
• How To Find The Amount...
Theoretical & Percent Yield:
• How To Calculate Theor...
Percent Yield - More Examples:
• How To Calculate The P...
Percent Error:
• Percent Error Made Easy!
_________________________________
Percent Composition By Mass:
• Percent Composition By...
Empirical Formula Problems:
• Empirical Formula & Mo...
Empirical Formula - Hydrated Compounds:
• How To Find The Empiri...
Combustion Analysis:
• Introduction to Combus...
Stoichiometry Practice Test:
• How To Solve Stoichiom...
_______________________________________
Final Exams and Video Playlists:
www.video-tutor.net/
Final Exams and Video Playlists: www.video-tutor.net/
General Chemistry 1 Review: bit.ly/3DNmZqb
PDF Worksheet - 160 Questions: bit.ly/37SVLn6
Thanks😊
Prayers turn to God may everyone everywhere be blessed and healed and protected in Jesus name amen.
Good luck on your test tomorrow
My exam is actually tomorrow
how did you know? XD
@Jaiden Boren mine is today and tomorrow
Wtf
Nah just confused on a lab report
you've taught me more in a 6 minute video then my chem teacher has this entire year
Sairy Ortiz ikr
Same reason why I’m here
Sairy Ortiz Tell me about!
never heard that one before
Truer words have never been spoken
Thank you so much. I'm currently failing chemistry and have studied for 2-3 hours every night. This subject is super hard for me. I spent 5 hours studying this tonight, watching videos and reading guides and doing problems. Whatever you did differently, it helped. Something in my head clicked and I understand this now! Again, thank you SO much!
You're welcome
Did you pass?
@@earthchan7540???
Jherson Gutierrez Maybe you should stop trying to cause problems and watch the video.... it can help you focus.
Screaming Bullfrogs you know damn well you only studied the day before the test stop lying
I’m gonna fail this final exam dawg 😭
Naw me too I’m so cooked ☠️
i failed 😊.
Same bro same 😔
Real
oop
How is it that the education system could be so fucked that the majority of a class won't be able to properly grasp a concept through hours of "teaching" yet can develop a perfect understanding from this 6 and a half minute UA-cam video. Teacher incompetence should really be addressed in some schools...
I wasn't at school for 2 days I missed the entire lesson like a dumbass
Because schools don't check if the teachers are able to competently teach their students
@@lucipo_ Your ignorance is amusing.
@@Sean_Orsborn OK taco bell lover
@@lucipo_ Say it like an insult. I I don't mind.
i love it when mark wahlberg teaches chemistry
i heard it too but after reading your comment i cant stop laughing during the video for some reason
im not gonna learn anything now because im laughing at this too hard
😂😂😂😂😂😂😂😂
OH MY GOD I HEAR ITTTT
😁😁😁
my method:
1.) balance the reaction
2.) find the ratio (how many moles of this make how many moles of that)
3.) find the mr(s) of the substances you want to work with
4.) just put the mass given into the ratio after converting mass into moles
brief version:
57 kg of aluminum oxide gave
17 kg of aluminum via electrolysis:
1.) 2Al²O³ ---> 4Al + 3O2 (balanced equation
2.)2 moles of Al²O³ give 4moles of Al so the ratio is 2:4 or 1:2
3.)Al²O³ Mr = 102
Al Mr = 27
4.) 57kg = 57000g
57000g ÷ 102(Al²O³ Mr) = 500
so 500 moles of Al²O³ were used
ratio = 1:2 (1mole of Al²O³ gives 2 moles of Al) so 500moles of Al²O³ gives 1000 moles of Al this
mass of Al= 1000 moles × 27(Mr of Al) mass = 27kg
actual mass / theoretical mass so:
17kg/27kg ×100% = 62.9 %
long explanation:
(sorry the numbers appear as powers)
57kg of aluminum oxide gave 17kg of aluminum via electrolysis
step1.)
balance the reaction
2Al²O³ ---> 4Al + 3O²
step2.)
find the ratio of the elements we want to work with
2 moles of aluminum oxide make 4 moles of aluminum so the ratio is 2:4 or 1:2
(look before the element/comound in the balanced reaction and use the numbers to figure this out)
step3.)
find the Mr(s)
Al²O³ has an Mr of 102
Al has an Mr of 27
(technically this is aluminums Ar since it is not a compound)
step 4.)
it says 57 kg of Al²O³ was used in electrolysis so we wanna convert this into moles:
57kg is the same as 57000g so 57000/ 102 (the Mr of Al²O³) gives us 500moles.
so we now know that 500 moles of aluminum was used. lets put this into our ratio that we found out in step 2.
ratio is 1:2 (for moles of aluminum oxide vs moles of the aluminum produced)
now just use this ratio to find how many moles of just aluminum were produced.
1:2 -----------> 500:1000
since the ratio states that 1 mole of aluminum oxide gives 2 moles of aluminum. so 500 moles of aluminum oxide should theoretically give 1000 moles of alumimun.
now we now that 57kg of aluminum oxide was used and that this equates to 500 moles of it
so now lets just find out how much aluminim was produced in mass
convert moles into mass ----> 1000×27(mr of just aluminum) gives 27kg (theoretical mass)
we were told that 17kg of aluminum was produced so niw what we do to find %yield is divide 17kg(actual mass given) by 27kg and we turn that into a percent to get the percebt yield which should be 62.9 percent.
Are u kidding me what is this man ???!!! Its a comment not a your chemistry period to explain all this😵😵😵
No wrong af
What time did u finish writing this all huh
Thank you for the free help!
I use this it’s much simpler one u know it
I know I'm like 4 years overdue but THANK YOU! Isn't it weird that UA-cam videos are MUCH better than our actual teachers in school? Like all of the lessons I learned was from UA-cam😅
5 years overdue lmao
How come professors cannot explain these concepts this simply?
Because they understand the material so easily and so they perform shortcuts to look smart meanwhile half of the class is failing due to their pride and arrogance. They need to show full examples of how to do the material but they dont bother and expect you to learn it by your self. Some teachers were never meant to teach and they know it and i cant understand why they are there to begin with in the first place. Not ALL teachers can teach. BUT TOCT is my Hero and i respect his craft it all make so much sense.
Lauren bruh im learning this in 9th grade
@@jylee4582 same i'm pretty sure it's a requirement to learn this in 9th
Yeah I’m starting to want to just do virtual school because teachers at school are so bad at teaching I learn most stuff myself anyway. What’s the point of spending 8 hours if you can learn material better in less that 8 hours online🤷🏿♂️
Honestly, youtube has taught me more than school. Im in the 7th grade and i like learning about science for fun but school is just stressful. Thankfully, i have a good teacher this year and last year but my grade four teacher sucked ass. He was to arrogant to actually explain how multiplation worked and was trying to win an imaginary game of who can teach the fastest instead. I wish school focused more on teaching than grades and scores.
You got a nice ass voice. It's comforting before a chem exam.
Nou Thao u can flirt later
its so dead, he doesnt give any expression
I ship you and Tyler. NEVER GIVE UP ON LOVE!!!
Oh wrong channel. I thought I was on a Tyler Dewitt vid lololol I MEANT I ship you and JG.
Dude, bless your soul. You just saved me from failing an assignment big time
his voice is such a comfort
yeah i’m done w chemistry i still don’t know what i’m doing💀🙏
Absolute life saver, my chem lab professor works multiple chapters ahead of lecture and did not want to read more than necessary for my upcoming lab. Thank you! I should ace this quiz now.
This dude works wonders. My prof teaches for 3 hours every lecture, and somehow makes the topic more confusing then it needs to be. Thank you for making things clear and organized.
I've watched so many videos on this and yours is the only one that makes sense. Thank you!!
"you know". Nah but out of all honesty you're teaching me better then my chem teacher can/has since the start of the semester
Thank you so much! I passed and got a perfect score in the computation part in our inorg chem lab (I'm taking pharmacy course). I don't get that topic before but due to watching this for two times, I get it now. KEEP INSPIRING
My professor with a PhD in chemistry cannot explain any mathematical processes in laymen's terms. He makes everything SO difficult and hard to understand.
Thank you, stranger on the internet, for doing this for all struggling chemistry students.
Thanks so much man.. you taught me more than my chem teacher did this whole year.. thanks bro keep it up
Y all these comments are soo old😭
Beautifully explained as always! You're the only UA-cam channel I can understand so clearly.
You explain these concepts so simply and smoothly much better than my current teacher, also your voice is really calming and its making me less anxious for my final, thank you so much!
Kinda complicated method... simply put;
[[Mol = Mass(g) ÷ Molar Mass]]
∴ 30 / 44 = (30/44) [= Moles of C3H8]
3(30/44) = 90/44 [= Moles of CO2 since there is a 1:3 ratio]
90/44 * 44 = 90g [Theoretical yield since molar mass of CO2 = 44]
It was just coincidence that the molar mass of Both C3H8 and CO2 are the same
UR ACTUALLY THE GOAT WTF
bruhh i still dont understand a thing i suckkk at chemistry
this is what i do everytime
That's what I was thinking
what if the ratio was 4:3 then??
You explain it so well and your voice is very pleasent unlike my proffessor :)
Thank youuuu Organic Chemistry Tutor!!! I have an exam about this topic in Chemistry and I easily understood everything you're saying 😭 what a lifesaver
That is amazing. Understood a concept I’ve been struggling for weeks on in six minutes. Thank you!!!
Literally 2 mins into the video and I get it already...Hope you hit 1 million .
This helped me more than my chem teacher, really good stuff man.
Very good video, paced just right for me to understand what's going on and not lose focus, thank you!
Thank you so much, as a maths lover it irritated me that I could not work out complex percentage yield and now, a day before my GCSEs, your video has saved me. Much appreciated.
How did it go?? Been 5 fcking years 😂😂
@@Lightningod7🤣🤣🤣🤣🤣🤣 got them in a few months bro
What would’ve we done without your videos 😭😭😭 thank you so much ❤️❤️❤️
It's a great explanation but you could get the theoretical yield by just using the molar ratio in grams. 30g of C3H8 and the molar ratio is 1, x grams of CO2 and the molar ratio is 3. Cross multiply and you'll get 90. it's way more simple
Thank you. You have made my chemistry work easier for me. Keep up the good work.
Thank you!! Sometimes it just helps hearing it explained just a slightly different way to get the concept. This'll really help with my exam tomorrow!
I'm in college right now and I have a Chem test tomorrow. This whole day I have had people pulling up to me asking me if I made chemistry videos because this guy sounds like me. 😂
i’m a freshman in highschool and i have to learn this not even capping
@@gerardohernandez5572 what on earth has you being a freshman got to do with people thinking this guy is the guy making the videos because they have a similar voice
@@gerardohernandez5572 same
This was very helpful! So glad UA-cam exists, and people like this to makes these vids. Hope everyone understood!
I'm in seventh grade and you don't know how much this has helped me not fail my finals
why are you taking chem in the 7th grade dawg😭
Great video! My lab instructor is a new TA and he just gave us one example and turned us loose on solving a ton of unknowns. No one understood. Unfortunately, having a Dr. teach us in the lecture and his TA do our lab causes a huge disconnect. The TA does things differently than the Dr. who breaks things down in a great way. It is killing my grade! I am struggling to keep an A and that is not me! I have never made below 97% in a college course. Until now, I have pulled the grade up to 93% and that took more work than I am used to. Thanks for the great video, the theoretical yield is pretty simple, only he could make it hard! He NEVER mention the limiting reactant once! Pretty important information!
Thanks so much, this finally makes sense to me!
Aftab shaik how did u do
thank you it was very helpful .....thank you thousand times
Love this video! Easy and straight to the point! 👏🏻👏🏻👍🏻
Bruh. Thank you so much, I never understood this concept but after seeing this one video for whatever reason I have a way better understanding.
Ai...He deserves a noble prize in chemistry man!!!
to all of those wondering.
here's a quicker way to do this.
Actual Mass of C3H8 / molar mass (relative formula mass) of C3H8
using your answer
times that by the Molar ratio difference (Example. H20 and 2H20 = 1:2)
then time by that by the molar mass (relative formula mass) by the one you are comparing your molar mass to. as if it had a molar mass of 1.
Here's how you do it.
1C3H8 = 30g
compared to
3CO2
30 (g)/ 44 (relative mass of C3H8 12x3=36 + 1x8=44)= 0.681 (continuous)
molar ratio = 1:3 (1C3H8 3CO2)
0.681 (continuous) x 3 = 2.045 (continuous)
time that by the relative mass of the product (in this case 3C02 if it was 1CO2 which coincidently has the same relative mass as 1C3H8)
CO2 = 44 (12 + 16x2= 44)
2.045 x 44 =90g
90% theoretical yield.
the actual that we got is 70g/70%
so its
70/90 (the smaller number is first.)
x100% = 77.7% percentage yeild.
there you go. hope this helps.
(also I am not a teacher, I am a college student who just grasped this.)
Thank you so much!
@@scarlet5621 even though its a year later. Your very welcome
Thank you so much, I finally understand how to do this and I have my exam on Wednesday...I can’t believe how simple this actually, why can’t my teacher can’t explain it like this 😪
I’ve never been able to solve a percentage yield question until now. Thank you!
You've been my teacher for my whole chem course lol, my chem teacher can't teach.
Don't mind me, just taking notes because I slept in for my Ap Chem class and wasn't able to know what everyone was doing
THIS WAS SO HELPFUL I WAS IN THE MIDDLE OF PANICKING IN CHEM CLASS THANK YOU !!!!!!!!!!
Omg thank god for this video I needed so much help with my chem homework and you cleared everything up for me. Thank you so much
this video saved me lmao. my first AP chem test is tm and this finally made sense to me
Thank you! btw you sound soo much like Mark Wahlberg! lol
Thank you so much for this video. The Way you explained really helped me understand. Most teachers just tell you what to do with out telling you why.
You're welcome
Needed some clarification on this topic for my unit test tomorrow. Thanks once again OCT!
bro saved my chemistry exam
His voiceeeee 😍😂
It's something else isn't it?
The Organic Chemistry Tutor Are u from Nyc?
It’s cute
His voice gives me anxiety. He sounds like he's either nervous or right about to go into a panic attack.
Noelly Abreu the breathiingg
oh my god thank u so much I have a lab report due on Monday and I literally don't understand anything especially percentage yield but now I understand a lot better!!!
Your videos are amazing. Thank you for sharing the wealth!
Good luck on your tests everyone!!!!❤
why is it that you did not get the g of O2?? like you did in C3H8??
it's the excess reagent. We don't need it to calculate the percent yield. There's plenty of oxygen in the air. I hope that answers your question :)
wow you have taught me in 6 mins more than any teacher in history of the whole world
Thank you for the step by step. it was so very helpful.
I am sooo uncooked
who come here looking for yield calculation in finance? its like you entering a wrong class
This is amazing, good job and keep it up :D
Since online school is staring because of this virus I will be utilizing this channel! This was super helpful, thank you so much
My test us actually tomorrow
Mark Wahlberg knows his chemistry.
I swear i was looking for the video about percentage yeild and percentage purity i have test tomorrow of chemistry about this very good explanation i understand easier you are better than my teacher
God bless you, you help me through my suffering in chemistry
Stop flirting with me
another simpler method guys
C3H8:3CO2
44 : 132
30 : x
132×30/44= x
90=x
This is wrong and definitely isn't a simpler method
How I wish you were my teacher. I don't usually subscribe to educational channels but I did to yours. Big thumbs up 👍👍
First time i didn't get his video🥺idm but really thankful that he uploads:)
I understood from his other video and now i can do this question and all other yeild questions he is a REAL GOAT 🐐
mom can we get *khan academy* ?
“no we have *khan academy* at home
khan academy at home:
You can do it! FOR WITH GOD NOTHING IS IMPOSSIBLE IN JESUS MIGHTY NAME! May God bless you on your exam!!!!
Thanks bro
Thank you Julio, I owe you so much, 3rd year chemical engineering student here.
this saved my life before my chem exam tmr god bless
I am still so confused :'( Like... I understand percentage yield no problem. It's the calculating of TY I can't grasp. The whole... 30g over 1 and 1 over 44, and 3 over 1.... x g / mol... I'm so so lost. Help! Someone, anyone!
Simplest way to do it is (Moles = Mass x Mr- then use the stoichiometric equation to find the ratio. Then using the moles from the ratio, and the equation Mass = Mr x Moles, you can find your theoretical yield.
you need to learn dimensional analysis
Didn’t get a single damn thing and I’m running out of time
Don’t expect to get help with that attitude.
@@AKCman35 2 months ago
@@josh-qj2zu im in the same position rn
this video helped me lol now i get the concept
istg this is easy but also so hard at the same time,, it's easily confusing... but your explanation is extremely clear! hopefully i'll be able to actually do my assignments on my own from now on TT
Thank you so much! I had no idea how to do this, and you made it so simple!
Thanks
Thank you. To be funny: 0:40 8 hydrogen atoms, eight has five letters, 8-5= 3, 3 sides to a triangle. Illuminati confirmed!
He didn't put the correct molar mass of CO2...... He filled it in with the molar mass of C3H8
Alright kiddy. Before you go calling out our professor here,,,,,, c = 12 o = 16 h = 1, if we're rounding to whole numbers. (12+32) = (36 + 8)
32+12=44 numb nuts
lol
lmao!
Gretchen Sich if you didnt notice, the molar mass of CO2 and C3H8 happen to be the same
This was PERFECT! Thank you!!
I've deadass learned more from this than my chemistry teacher could teach in the last month
Thanks dude this was helpful, you teach better than my chem teacher
thank you. your explanation prepared me for my exam
Appreciate the quick video as review for my AP Chem clsss
Makes so much sense now!! Thank you!!!
Thank you so much you helped me understand this concept.
you are a god. i swear when i'm makin a little more money i'm jumpin all up on your patreon. you put college professors to shame
great vid, helped a lot
This was super helpful, thanks!!
youre a lifesaver dude thank you
Thank you! Chemistry is super hard when there’s all this maths.
I already watched this video back in highschool on the subject General Chemistry, and I'm back to rewatch it again on our Chemistry for Engineers now in college.
this person is carrying so many students on his back right now. THANK YOU!