How To Calculate Theoretical Yield and Percent Yield

[@TheOrganicChemistryTutor]

Stoichiometry Formula Sheet: bit.ly/3Z7uMw8 Stoichiometry - Video Lessons: www.video-tutor.net/stoichiometry.html

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Not only did you saved me in high school, but now your videos continue to help me in university. Thanks for sharing the knowledge!

[@persephone9307]

Thank you. You and Melissa Maribel really helped me in Chem this year. It's been killing me, hell it's been my worst class, but your making it somewhat bearable. Thank you again.

[@jasminekoala4826]

This video just helped me SO much with my lab report, I tried asking my teacher about this and she wasn't being very clear

[@theteacherbm2914]

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Hope i can get a great mark in the chemistry exam on coming Monday

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[@lanremoses5291]

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[@ricaelastieben1911]

This helped me so much!! THANK YOU!!

[@georgesadler7830]

Professor Organic Chemistry Tutor, thank you for showing How to Calculate the Theoretical and Percent Yield in AP/General Chemistry. From the video and other reasons, the Actual Yield in a reaction is ordinarily less than the Theoretical Yield. Putting it another way, the Percent Yield is expected to be less than 100. This is an error free video/lecture on KZbin TV with the Organic Chemistry Tutor.

[@JCEurovisionFan1996]

This is *very* confusing. Can you do some more examples?

[@yungwells6549]

He basically found the no. of moles for the limiting reagent. Then multiplied by the number of limiting reagent moles by the molar ratio (for this question it was 1:3, my question was 1:1 to so it remained the same) then multiply by the molar mass of the product to give you the mass. He basically joined all the steps which confused me too. But I did it in 1,3 parts (2 part question) and it was easy for me. 1)Find no of moles of limiting reagent n = m/Mr 2)Check the molar ratio (1:1 it remains the same, if not multiple or divide according to the ratio) which gives you the number of moles of the product. 3)Find the molar mass of the product 4)Mass = no. of moles x molar mass, so multiple them to get your theoretical yield. 5)Calculate % Yield using the formula. You probably know by now but this may help someone else.

[@basharibrahim2193]

Thanks a lot bro 😊 I have exams tomorrow I was just told to learn this wish you success

[@utzilsho5757]

Hi your videos really helped me from my freshman year to now my senior year, however i was wondering if there's a video that could help me solving this question : If 250 ml of 0.54 M HCl produced 1.01g H2O, what is the percentage yield of the reaction? CaCO3 + 2HCl --> CaCL2 + CO2 + H2O

[@DomBrungardtCubing]

Anyone else have chem exam tomorrow and are cooked?

[@violet-rj3cz]

me fr

[@DomBrungardtCubing]

@violet-rj3cz i have the ACS final this Wednesday. I'm cooked again

[@DomBrungardtCubing]

The average score on that test is a 50%

[@nb8982]

Got my chem final Wednesday kinda nervous but this help

[@ShyneApas]

how did you identify the limiting reactant and excess reactant? like the solving process???

[@matiasignaciorocco3667]

say you have A+B=C, A is 15 and B is 10, there B would be the limiting reactant and A the excess reactant, I am not sure I was completly clear but hope it helped

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God bless you❤

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[@kaiwoodlen730]

Hello, can you please solve this question because I can’t understand how to solve it. The overall equation for one method of manufacturing hydrogen from methane is: CH4 + 2H20 -> 4H2 + CO2 In one batch, 5.12 tonnes of hydrogen is obtained from 13.6 tonnes of methane. What is the percentage yield of hydrogen for this batch? A)37.6 B)42.5 C)54.4 D)75.3

[@RLN579]

Are you sure it's the percentage yield they're asking for, and not the Theorectical Yield? If its the latter, the perc yield is 13.72%, and the theoretical yield is answer choice A.

[@kaiwoodlen730]

@@RLN579 it word for word on the text book

[@jaeshiki]

the answer is D

[@azca.]

5:35

[@joseescobar549]

Good video

[@XarenyAnva]

Great analysis, thank you! A bit off-topic, but I wanted to ask: I have a SafePal wallet with USDT, and I have the seed phrase. (behave today finger ski upon boy assault summer exhaust beauty stereo over). What's the best way to send them to Binance?

[@DAG4RBAGE_EDITZ]

is it 30g c3h8/1 because it has one mole?

[@onk215]

Thank You.

[@shaunkelly6224]

Tutorial for actual yield from scratch..? Please..! Thank you (if) in advance.

[@kgalalelonapo4588]

Can I ask isn't it suppose to be 4O2 not 5O2??

[@andrieguteza9573]

9:30

[@hangersan995]

If the problem includes a given value of temperature, do I disregard it or not?

[@zachseaman4335]

If this is gen chem, probably disregard it. Implications of temperature on reaction rates are in Analytical chem courses. In that case, one may use temperature to calculate a different theoretical yield.

[@jaegersbomb6706]

ok so i’m super confused and i don’t know how to do this question i got for homework... sodium reacts with chlorine to form sodium chlorine. calculate the theoretical yield of sodium chloride, in grams, when 28.4g of chlorine reacts completely with sodium.

[@haas9649]

Hi, I know this is like super late and you probably got the answer by now, but first you need to write the chemical equation of the sum (Na+ Cl2 -> NaCl) and then balance it (2Na +Cl2-> 2NaCl), after that you just need to find the moles of Cl on the reactant side (moles= given mass/ molar mass, so that would be moles=28.4/35.45= 0.801 moles of Cl2) now that you've found the moles. You just need to use the mole ratio and find the moles of NaCl (the balanced equations says that 1 mole of Cl reacts to give 2 moles of NaCl, so 0.801 moles of Cl gives 2(2 moles of NaCl in the balanced equation) x0.801 (moles of Cl that youve found) which gives 1.602 moles of NaCl, from there on its just finding the mass of NaCl which im sure you can do on your own. Note: You dont have to use the method i used for the mole ratio, use which ever method you know best.

[@nebulablitz1518]

@@haas9649 you didnt start if off with hello there, disgraceful if you ask me

[@haas9649]

@@nebulablitz1518 ah shit. I'm ashamed of myself. I shall do better from here on.

[@raniariffat8094]

@@haas9649 hey, won’t it be 28.4/71 instead of 28.4/35.45? since there is a two subscript with chlorine. 🤷‍♀️

[@veronicaflores5575]

Can a percent yield be more than 100?

[@ycremkiraguh8596]

No

[@mariakokomali]

Good

[@ThadRassin]

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[@oscarmalungo2754]

Hope I can get great marks in chemistry test tomorrow

[@sarimkhan2414]

how did he get h20 when making the reaction

[@rollaskaet]

it's combustion, combustion produces water and carbon dioxide

[@chourouk-gr9qg]

Ty

[@rodrigoflores8537]

Thanks for saving me from extra

[@dustincayron4640]

what is the theoretical yield of Zn(s) + 2 AgNO3(aq) --------------- 2 Ag(s) + Zn(NO3)2(aq) NEED HELP.

[@mohammedbadi3081]

do u still

[@dustincayron4640]

@@mohammedbadi3081 nahh but thank you bro

[@AnimeGIFfy]

*homework* something that teachers to kill us (if you sit in the back you can get away not doing it)

[@NestThermostat-y3j]

I hate when people explain something, you see adding things that are not in the verbiage. Where did H2O come from? That was not in the paragraph. Is H2O the common theory to solving the problem?

[@jonathanhight2942]

He saves me every test but bros mic is picking up to much sound I can hear every mouth movement

[@Koweenss]

Can someone answer my assignment When 1.87g of aluminum reacts with 9.65g of copper(II) sulfate ( CuSO4), 3.65g of Cu was produced what is the percent yield of Cu If anyone got an answer Find this Person Hamada Maruteru

[@pialikoya6507]

There’s no need for converting grams to moles in this particular question. The ratio of C₃H₈ to CO₂ is 1 : 3 so 30 g of C₃H₈ will produce a theoretical yield of 3 x30g or simply 90g. To calculate percent yield do (70/90) x 100% = 77.8%. Same answer

[@user-rk5hu5fh7y]

i have a gcse tm and this is on it #sendhelp

[@JRH2033]

When calculating you should say multiply by 100%, because mathematically that is incorrect. 0.50 x 100% = 0.50 instead 0.50 x 100. I say this because a lot of people will put the percent when multiplying and get the wrong answer because 100% is equivalent to 1.

[@J1zzy_]

Real shit

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This left me disoriented tbh

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