Percent Yield Made Easy: Stoichiometry Tutorial Part 4

[@rachaelcruz2847]

Thank you for taking your time in breaking it down in a way that I can understand. It makes it easier to understand when you use everyday products as visual learning tools. Chemistry can be so abstract at times.

[@ketzbook]

You're very welcome!

[@TooManyPetsAndStuff]

This series helped me to understand what 3 months of classes couldn't. Cheers!

[@graciebowman5137]

Saved me, my exam's tomorrow and i forgot everything about this unit, thank you!

[@alamusleh1610]

how'd you do? lol

[@michaeldonatelli7166]

@@alamusleh1610 i got one tmrw and will provide updates haha

[@awokenajin6620]

@@michaeldonatelli7166 you did not provide updates

[@michaeldonatelli7166]

@@awokenajin6620 got a fuckin C but that’s bc I studied two days before. Got another one next week but starting now

[@oliviagrace3952]

thank you sooo much for this! my teacher didn't explain how to do this very well so i was basically relying on videos to get this assignment done. no other website was helping, thanks for being so thorough!

[@kyliejw8811]

Thank you!!! My teacher explained this just as well as a squirrel teaches calculus. You are much appreciated my friend!!!

[@ketzbook]

You're welcome!

[@AlysonFox-cy5tw]

THANK YOU ive been blankly staring at my lab report for hours you saved my life lol

[@willisilikefood9492]

TOP G thank you, I bout to pass my Chem test now.

[@moresalad221]

Dang that was awesome!! Onto limited reactions!!

[@سيفمجدالرمحي]

Mr you are a very tallent teacher Your explains is more than great

[@tapiwamutasa9295]

I’m writing in 2 hours. Thank you so much

[@panasiia2221]

So helpful, wish they explained it this way in my lectures.

[@mathyre232]

This guy has the best handwriting ever

[@1nick339]

ngl, I use khan academy but when I found your channel I was blown away how you made it sound a lot more easier. Even though this has been made 6 years ago, I want to say thank you!!!!!!!!!!!!!!!!!!!!

[@ketzbook]

Happy to help!

[@shanialenae1008]

percent yield is normally less than 100% because different side reactions may occur or the products may get lost | 00805 |

[@Park-zv8tf]

Just finished the chem final!! 🙌

[@story-time-message]

Mines tomorrow. 😬

[@luvsharma1627]

watching from India....nice work sir

[@ketzbook]

thanks!

[@244244cc]

It's normally less than 100% because the reaction might be incomplete, there may be side reactions, product loss when purifying or may be spilled or blown away

[@Silembr]

Thank you for this video. I went from wtf is this to fully understanding 😋

[@Knight_Igris]

Thank God a simple video to explain it

[@jonathan_kim]

Thanks for the helpful video!

[@Samosa-l7d]

Wow ❤❤❤ nice 👍 explanation ❤keep it up 👍

[@rjwarrior10118]

GOOD LUCK FOR YOUR EXAM TOMORROW!

[@cierrasouthard6532]

the percent yield is normally less than 100% because the reaction could be incomplete and different side reactions going on as well. product could be lost through the reaction and could affect the percent yield. 00823

[@Ilyff]

saving me before my exam tmmrw

[@rebeccaarpie9184]

ID:00404 If the percent yield is 250%, that means that there is a mistake and needs to be fix. This results form the actual yield being larger than the theoretical yield and this physically cannot happen. A calculation or measuring mistake must have occurred.

[@shivikamittal8664]

Very good explanation:)

[@meganperdue2865]

Percent Yield tells you how well the reaction worked; the actual yield divided by the theoretical yield times 100; 00415

[@DoplerEffect]

00803] Percent yield tells how much a specific chemical reaction actually yields compared to it's theoretical potential.

[@itsjustme.7059]

This finally makes sense. Thank you.

[@patriciachabala3190]

Well explained 😍

[@Mustangg]

This video is so good! Thank you for the help :)

[@dequinox7089]

Thanks for this excellent video!

[@rainymc]

OMG THANKS SO MUCH U MADE THIS SO CLEAR NOW I UNDERSTAND

[@miguelboisvert7375]

Thanks this made it so much easier

[@mekdev3319]

A lot helpful i loved it as i am a student pleas do more

[@ketzbook]

thanks!

[@luzzacariaz7021]

the percent yield is normally less than 100% because the reaction might be incomplete, there may be side reactions, product loss when purifying or may be spilled or blown away, 00611

[@Grace-li6ts]

really great!

[@alanafox7866]

It's recoiling to compare what you do vs the institutions. Being sincere & generous to "the system", I estimate 1 of your minutes is more valuable than 1 of their hours. At this point I'm nerding out and watching for fun, though it's put a thorn in my side... where could I be if such clean and clear content were available in my youth... The Kurzgurzat (spelling this wrong) channel gives me a similar feeling. Anyway, just venting a Well Done to the void. Cheers!

[@ketzbook]

Thanks, I'm glad this helped! And it's an honor to be compared with Kurzgesagt; I love Kurzgesagt!

[@hueyt3323]

Percent yield conveys the accuracy of the reaction. Actual yield/theoretical yield x100 = percent yield.

[@hueyt3323]

00421

[@immsnghidi4871]

This is useful. Thanks a lot

[@shelovesRH]

the percent yield is basically the mass of the actual yield over the mass of the theoretical yield multiplied by 100

[@rebeccamerritt6001]

Percent yield is how well the reaction worked, it is the actual yield divided by the theoretical yield multiplied by 100 00115

[@daejahjackson-powell7096]

Percent yield is normally less than 100% because it could be an incomplete reaction, a side reaction, product could've been blown away or spilled, product sticks to the container, or product was lost when purifying., 00811

[@brookeparker7332]

theoretical yield is the amount of product that could be made if the reaction worked perfectly with what it has, 00214

[@Thatgueropaul]

Thank you soooo much

[@danez199]

00123, percent yield is usually less then 100% because the theoretical amount is usually more then the actual yield

[@CYBERSONIC-80]

A different method we always use to calculate theoretical yield gave me 3.84g and now I'm all confused

[@MAndy-sw8rb]

Compares the actual yield and the theoretical yield to show how well the experiment worked in a percent don't forget to times by 100, 00403

[@y2k68]

How much of the product that is made without any thing added or changed, 00707

[@ELARSGEEZ25]

Thank you

[@joehogue8415]

This was dope

[@christianrothermel6487]

Actual yield is the amount that is actually collected during a reaction, 00607

[@jordin407]

00815: The percent yield tells you how successful your work has been at producing the desired product

[@rileynobles7146]

Nice job

[@erykbluto2468]

Theoretical yield is taken from what you have and made with the most amount, 00702

[@okpala1586]

SO HELPFUL OMG

[@RYanimayyyyy31]

Theoretical yield is simply the greatest possible amount of what you can make with what you have. 00814

[@organic2840]

how to write organic reactions in video scribe? please guide me

[@ketzbook]

There are some Videoscribe instructional videos on youtube to get you started. If you want to do something like a reaction mechanism, you will have to draw it in ChemDraw or some similar program, then save the individual parts as tiff, png, or jpg, and import them into your Videoscribe. If you want to get a better drawing effect, you will need to convert it to svg, but that may not be worth the effort. It is a long process.

[@onyeagusimarycynthia3138]

Can the actual yield be equal to the theoretical yield

[@asdf7711]

Yes, but unlikely. It's theoretically possible to get 100% yield if actual yield = theoretical yield.

[@shaunkelly6224]

There is no actual yield on my question. Can we find it out of scratch?

[@ketzbook]

is it a lab question?

[@AMysteryGhost]

Nothing can save me now. This video was my last shot

[@sierrahfindeison3092]

The percent yield should be less than 100% if it is 250% an error has occurred and you should re-do the problem, 00110

[@leakheme648]

THANK YOUU SOO MUCH

[@rat_coder]

because there are usually impurities and undesirable reactions 00205

[@justinalloway1405]

Actual yield is the amount of a product that can be made of an isolated chemical

[@tariqmasih6986]

Please make video on soda glass and opal glass

[@rachaelbreneman8572]

a percent yield shows how good or efficient your reaction is

[@toptop1618]

When 3.59 g of nitrogen monoxide, 9.34 g of ammonia, and 2.38 g of oxygen were allowed to react, only 1.27 g of nitrogen can be obtained. What is the percent yield of nitrogen? I don't know about this😭😭😭

[@ashleymartinez2466]

Theoretical yield is the most of something that you can make with however much you have. 00114

[@ELARSGEEZ25]

God bless you

[@hannahohara5969]

Actual yield is what is physically made or product produced, 00213

[@kaylynndick9344]

Percent yield tells me how well the solution was effective, 00409.

[@alisawarren2096]

The ratio of the actual yield to the theoretical yield. How close you are to the 100% mark. 00609

[@marisoldeleon3735]

Actual yield is the amount of product that is actually made, 00801

[@rajatpandey4213]

Thankyou

[@kaitlinhitchens679]

percent yield is normally less then 100% because the theoretical amount is usually more then the actual yield. 00111

[@makaylaleigh7729]

Actual yield is the amount of product that is actually made and/or produced ; 00101

[@amycraft6993]

Theoretical yield is the most amount of product you can make with however much you have. 00108

[@Rubester11]

00414 Theoretical yield is the most amount you can make

[@colehatton9784]

the percent yield should be less then 100% if its over 100% then side reactions and other things might occur so you might want to go over your calculations again #008334

[@rhyno17]

Actual yield is amount of product actually made in a reaction

[@clairetrimble8439]

Actual yield is the amount that's actually produced, 00419

[@tiapersolio322]

Check your calculations/measurements and make sure your product is pure, 00416

[@kaiyahall6934]

Theoretical yield is how much the product is when its combined

[@sandwichson4532]

taking my test right now lmao

[@chizzo8347]

THANKS

[@GoatGaming-tr4ff]

You can't get the full amount out normally of what you put in, 00217

[@michaelbarr9426]

the amounts of proucts calculated from a complete reaction

[@angelalara2950]

so who wants to do some homework for me for some money?

[@JoseGonzalez-ed4hq]

U got a cool high school if u learning this stuff mime sucked

[@deniserobles9253]

a calculation or a measurement error has occurred within the process, 00216

[@karapowell4359]

The actual yield is the amount of what is produced, 00719

[@dylanarmiger6643]

the actual yield is the amount of product that actually produced and isolated from a chemical reaction. 50678

[@kumatatas9512]

It's exam season boys and girls

[@dustinbeideman9168]

Percent yield tells me how well the solution worked, 00103

[@johnriovelasco5617]

molar mass of 3O2 is 32.0? I thought it was 35

[@ChemSimplified]

It's 32.0 since there are 2 oxygen atoms, so 2 x 16.00 = 32.00 g/mol

[@yaritssaparada7881]

actual yield is the amount of product that is actually made, 00119

[@savannahfaulkner5874]

re-do the problem because the percent yield should be less then 100 00410

[@calistawaddell512]

because the theoretical yield is usually more than the actual yield 00723

[@jakekart55]

If the reaction worked perfectly with no errors it's the product that could be made. 00420

[@shanialenae1008]

percent yield tell me how much a actual yield compare to a theoretical yield. 00809