Stoichiometry Tricks

[@mr.b6551]

"Here's 12 of these questions, you have 15 minutes to complete the quiz" -Chemistry teachers

[@PCgamerChannel]

Sounds like my Steel design professor but with problems way harder and longer

[@deniserobles9253]

top left and bottom right always have to have 1 mole bottom left goes the molar mass of what you start with and the top right has to have the molar mass of what your solving for in the middle section goes the coefficients of the chemicals from the balanced reaction

[@VKVK-bb8ql]

Thank you so much, We can even short down it. The above equation 2C8H18. Gives. 16CO2 then 228grams of 2C8H18. Gives 704 grams of 16CO2 THEN 2800 grams gives 2800×704÷228 Which gives 8600 grams of CO2

[@myraflores4608]

Anyways, your videos are always helpful! And your voice does not makes me feel sleepy.

[@altheagordon7183]

Thank you very, very much for your explanation on Stoichiometry. After weeks of trying everyone, I never knew I would find someone like you to help me. I am so happy because I have my exam coming up later today. Thank you.

[@calistawaddell512]

1) Write down the balanced chemical equation 2) Calculate the molar masses of the chemicals 3) Convert mass to moles of what you know 4) Convert moles of what you know to moles of what you want to know 5) Convert moles to mass of what you want to know 1 Mole This tells us the other part of the fraction is a molar mass conversion factor 00723

[@henryroa1729]

I learned more in 6 minutes than 2 hours worth of BS video lectures from my professor. you are a god send!

[@justinalloway1405]

A new trick I learned was that when a number in a balanced equation is not whole multiply the whole thing by 2 - 00401

[@meganperdue2865]

The balanced equation is used between two unit conversions of moles to grams, 00415

[@0nobody379]

the balanced reaction is used between the 2 unit conversions of mols and grams. The thing you're solving for is multiplied at the top and the thing you have is divided and the 2 numbers are used as coefficients. 00205

[@user-ut5nx6hm9d]

Ok I wish I'd found this videos earlier.

[@kirashort1895]

1 mol is always in the top left and bottom right. This figure reminds us that the other half of the fractions are molar masses. The number on the bottom left is the molar mass of what we're starting with, while the number on the top right is the molar mass of what we're solving for.

[@savannahfaulkner5874]

top left and bottom right always have to have 1 mole bottom left goes the molar mass of what you start with and the top right has to have the molar mass of what your solving for and the middle section is the coefficients of the chemicals from the balanced reaction 00410

[@rebeccamerritt6001]

The balanced reaction is used to convert the molar mass of the chemical we were starting with, in this example octane, to the chemical we were looking for, carbon dioxide. The balanced reaction is needed to take into consideration how many of each molecule is needed in the complete combustion. 00115

[@joeybfitness991]

The conversion factor between one chemical I another is the balanced chemical decided by the other chemical. A trick I learned from this is the mole divided by the molar mass of the chemical mirror each other on each side.

[@jakekart55]

It's used between the two unit conversions of moles and grams. The thing you are solving for is multiplied and the thing u have is divided.

[@drewd2696]

The middle fraction are the numbers from the balanced reaction the chemical we are solving for goes on top and the one we are starting with goes on the bottom 00802

[@MAndy-sw8rb]

00403: Bottom left- molar mass of what you are starting with, important because it corresponds to what you start with Top Right- molar mass of what you are solving for, important because numbers on top correspond to what you are solving for

[@jordin407]

00815: You use the balanced reaction in stoichiometry to determine the relative number of reactants and products

[@hueyt3323]

The chemical that you are solving for goes on top and the balanced reaction goes on the bottom, using numbers of elements, from a balanced reaction, 00421 (Elijah Tull)

[@sheilaescamilla4767]

It is used between the conversions of moles and grams, 00715

[@briannagrace182]

This is the reason I won’t fail my quiz tmr

[@cierrasouthard6532]

1 mole is always in the top left and the bottom right, this tells us that everything in between are molar masses. the fraction in the middle comes from the balanced equation itself. 00823

[@kokopium7761]

I absolutely love you

[@oliviaalloway6869]

the numbers from the balanced reaction, the chemical solving for goes on the top and the balanced reaction is on the bottom

[@atiqazubairi3382]

THANKYOU SO MUCH SIR THIS VIDEO HELP ME ALOT TO SOLVE SO MANY TRICKY QUESTIONS THANKYOU

[@ketzbook]

you're welcome!

[@TheMan-cf9yf]

Thank You So much

[@khubaibuddinsimran4930]

He's sooo underrated

[@redlight7718]

you are the best thank you so much

[@kasiyahtatem7946]

1 mol always goes in the top left and the bottom right because it reminds us that the other portion is the molar mass, 00418

[@myraflores4608]

Why I get 8632 and something when I calculate it? What could be the problem?

[@manaloaaron7256]

Me to even the scientific calculator agreed

[@rhyno17]

1) Write down the balanced chemical equation 2) Calculate the molar masses of the chemicals 3) Convert mass to moles of what you know 4) Convert moles of what you know to moles of what you want to know 5) Convert moles to mass of what you want to know Grams to moles 00407

[@madankumarsingh1598]

Thank you for saving ma life

[@ketzbook]

you're welcome!

[@madankumarsingh1598]

@@ketzbook omg can't believe it's you. Thank you once again

[@hannahohara5969]

1 mole always goes in the top left and bottom right. This tells us the other part of the fraction is a molar mass conversion factor. 00213

[@rebeccaarpie9184]

ID:00404 The excess mass of the Carbon Dioxide came from the Oxygen; this is why its mass is larger than Octane's.

[@MiguelSantiago-tr4ff]

In the middle of the fraction, the Chemical we are going for goes on top, and chemical we start out with goes on bottom, 00217

[@mylezhudson7324]

Balanced reaction is in the middle of the three parentheses

[@sierrahfindeison3092]

You use the balanced reaction as your conversion factor, 00110

[@alexispascual8187]

1 mole is always in the top left and also the bottom right. This tells us that everything in between is considered the molar masses. 00818

[@rosingh8425]

The chemical that's getting solved goes on the top and the balanced reaction goes on the bottom right, 00608

[@amycraft6993]

1 mol goes in the top left and bottom right. This tells us that everything in between are molar masses - 00108

[@colehatton9784]

you put the balanced reaction into the middle of the three parentheses

[@colehatton9784]

008334

[@teganshockley2047]

we use the chemical we start with on the bottom and the chemical we are solving for goes on the top, 00417

[@lendyfuentes2082]

1mole is at the top left and the bottom right. Reminds us that the other half are molar masses

[@christianrothermel6487]

In the middle fraction, the chemical we are going for goes on the top and the chemical we have goes on the bottom, 00607

[@makaylaleigh7729]

I learned how to combine the three equations into one large conversion ; 00101

[@mssmiley85]

Thank youuuuuuuu

[@dustinbeideman9168]

1 mol. Reminds us the other half of the fractions are molar masses, 00103

[@daejahjackson-powell7096]

Instead of having three separate calculations, you can combine the three conversions., 00811

[@DoplerEffect]

00803] 1) 1 mol in TL and BR 2) this "reminds us that the other half of those fractions are molar masses"

[@tiapersolio322]

1 mol goes in top left and bottom right conversions, 00416

[@kaiblackwell2086]

You lost me at “welcome” lol

[@irhamf7636]

oh god oh god oh god oh god , this is so helpfulll !! i believe u can beat khan academy way more better ! u solv 6 yeas problemmssss. thanksssssss

[@stephaniedalit573]

Life saver

[@ketzbook]

:)

[@islerdonnesha]

Your balanced equation is the conversion factor in the moles to moles equation

[@bayleeketterman3620]

the coefficients of the chemicals from the balanced reaction. 00412

[@agustinjaysoncadag]

Sir, I think that should be 8, 632 and not 8, 600?

[@briehagen1254]

I learned how to combine three equations into one big step, 00806

[@elianrodriguez6206]

because octane was being burned in excess air, the mass of oxygen made the mass of CO2 larger than Octane, 00824

[@erykbluto2468]

The numbers from the bottom reaction, 00702

[@johnwyck9482]

❤️ u........thank u soo much 🙏

[@rachaelbreneman8572]

1 mole it reminds us that the other half of the problems are molar masses, 00703

[@reaganlittle6431]

1 mol, this reminds us that the other half of those fractions are molar masses. 00813

[@abbyswearer5408]

the chemical you are solving for on top and the balanced reaction on the bottom,984311

[@ZioTrickz]

I learned how to put 3 fractions into one to make the problems easier., 00821

[@EternalSmite99]

The mass of CO2 is larger because when the 2 Octane molecules are burned it creates 16 CO2 molecules (a much larger amount) 00610

[@kaylynndick9344]

The mass of Co2 is larger than the mass of octane bc of the large amounts of oxygen compared to hydrogen in octane, 00409

[@kirbygedalanga4402]

Why the O becomes 25 please explain

[@ashleymartinez2466]

The mass of CO2 is larger than the mass of octane because of the excess air, O2, 00114

[@edgarfernandocortesespinoz3706]

did someone else solve the balance equation diffrent? Igot C8H8 + 10O2 = 8CO2 + 4H2O

[@kaitlinhitchens679]

the mass of carbon dioxide is larger than the mass of octane. 00111

[@johnkopp780]

The percent Yield is 0.8 percent, 00606

[@ricky-11]

Anyone else here cuz their teacher made them watch this vid then do notes?? Smfhhhhh😭💀😂😂

[@guadalupevasquez8859]

love the trick!! Too many steps makes me not want to do it. Much thanks! xoxo

[@ketzbook]

you're welcome!

[@alphatangowhiskey7600]

i learned to combine 3 equations into 1 big one, 00206

[@RYanimayyyyy31]

The mass of CO2 is larger than the mass of octane because of the large amount of oxygen compared to the hydrogen in Octane. 00814

[@princessjones5185]

It is more oxygen in octane than hydrogen, 00209

[@dylanarmiger6643]

i learned to combine 3 equations into 1 big one, 50678

[@y2k68]

Balanced reaction, 00707

[@gabrielgalaviz8398]

How he get 44.01 ?

[@brookeparker7332]

CO2 is larger due to the amount of oxygen which makes it 3 times bigger than the mass of octane, 00214

[@tarynwood7017]

because CO2 has the higher molar mass in the equation 00224

[@alisawarren2096]

Because octane is being burned in excess air, 00609

[@raynelawrence7546]

balanced reaction, 00812

[@yaritssaparada7881]

The mass of CO2 is larger than the mass of octane because the extra mass came from the oxygen, 00119

[@sabrinacardarelli6486]

Balanced Reaction 00107

[@jillianwharton1442]

Its larger becuase CO2 has such a bigger mass, which is why it overrules octane, 00724

[@JewBoiZ96]

00716 I learned to use 3 steps in one

[@trevorbowden7341]

oxygen makes the mass larger for carbon dioxide while octane is burned excess air. 00104

[@davinperez3194]

1 mole, and tells us that half of the other factors are moler mass

[@karnaejackson5136]

Balance reaction 00112

[@graysondoesgaming1330]

Chad 🧡

[@donnyconquest3085]

because of the oxygen in the carbon dioxide, 00204

[@sharvesh0369]

it is not 8600g co2 it is 8624g of co2

[@ketzbook]

significant figures my friend, significant figures. There are only 2 significant figures, so it is 8600.

[@waltersobchak7275]

@@ketzbook What's up with all the repetitive comments in this comment block?? Are they your students?? By the way nice videos, and website. You are a natural bro. 👨‍🎓👨‍💻🔬🔎📚✏👍💯🎓🤓

[@ketzbook]

@@waltersobchak7275 yes, some of these were my students answering a hw in the comments.

[@waltersobchak7275]

@@ketzbook Thanks Professor Ketz.

[@clairetrimble8439]

CO2 is larger than octane because of the excess air, 00419

[@Rubester11]

00414 Hydrogen weighs less than oxygen

[@shelovesRH]

Because CO2 has a larger molar mass 00709

[@karapowell4359]

CO2 is larger because of the amount of oxygen compared to octane. 00719

[@sanatani_manushy77]

Anyone from India!!

[@J_o_k_e_m_a_n]

FIRST!!!!

[@Omg.itsmonica]

Anyone else get 8632g of CO2??