Bond Energy Calculations & Enthalpy Change Problems, Basic Introduction, Chemistry

[@TheOrganicChemistryTutor]

Final Exams and Video Playlists: www.video-tutor.net/

[@wildsharkstudio9705]

this video deserves millions of views and subscribers. thank you for explaining this to us perfectly.

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[@georgesadler7830]

Professor Organic Chemistry Tutor, thank you for showing how to calculate the enthalpy of reaction by using the Average Bond Dissociation Energies listed in a table.The examples/practice problems are simple to follow and understand from top to bottom. I really enjoy this short video. This is an error free video/lecture on KZbin TV with the Organic Chemistry Tutor.

[@gdog556]

well said

[@PulpFrancis]

chatgpt type shit

[@abemckay1447]

You are the reason why I did well in AP chem last semester

[@Morpheus-zw4px]

Why is deltaH here defined as H(reactants) - H(products) whereas in other cases we take H(products) - H(reactants) to find the enthaply of the reaction?

[@supremepizza2267]

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[@RicJiang]

0:00 Question 1 3:19 Question 2 8:03 Question 3 Final results 3:17 Question 1 7:57 Question 2 11:13 Question 3

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@@weteaman1498 they died i guess

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[@denissemitchell9891]

Thank you for simplifying this subject! My textbook freaked me out.

[@farawayfaerie8829]

i stressed about this topic so hard but you made it so easy, THANK YOU!

[@SayedOwais1234]

thank you so much, I knew everything about this topic but I got confused if I have to multiply this number by 1, 2, 3 or something, you made it crustal clear. God bless you

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[@andrewswehla1694]

I agree

[@craftyle1201]

Thank you so, so, so much! I got an A on my chemistry topic ab bond enthalpy and Hess's law because of you!! please keep making videos so I can also pass my exam lol. Also u have a rlly nice voice

[@mahdiasiddika]

Kinda right about the last statement!

[@denka7292]

U re like the most perfect thing in the world thank u this was soooo helpful

[@monenga]

It is a perfect explanation. Only CORRECTION is that the last two examples are not kJ/mol but kJ/entire reaction, so the unit in the answer is simply kJ. The first problem is indeed kJ/mol. Thank you so much!

[@FreestyleEditz_]

Bro knows everything 😂

[@MegaShiney99]

r-p only for bond energys because breaking bonds requires energy (endo) + and making releases (exo) -

[@Celery32]

ok thank you for this I was trying to figure out why it wasn't p-r as usual

[@arjaydeleon5996]

3:59 I found it funny and cute HAHAHA

[@avanirai2516]

i learned smth i didn't know before this video, ty !!!

[@PritomAhad]

Isn’t it supposed to bd del h product minus reactant del H instead of the other way around done in the question?

[@ubongabasigeorge2704]

bond enthalpy is bonds broken- bonds formed. in this case it is reactants-products

[@ChillFlows]

@@ubongabasigeorge2704 Is this only because it is endothermic? So when we do [bonds broken - bonds formed] it becomes [reactants - products]? Or does it always stay [reactants- products] even when exothermic or do we switch it around for exothermic [products-reactants]

[@someperson3549]

Yeah I need an answer to this as well.

[@ubongabasigeorge2704]

@@ChillFlows yes, enthalpy of formation is products-reactants while bond enthalpy is reactants-product. be aware of your balanced equation and know exactly what you’re looking for

[@yang_er]

Man, you're a blessing. I just read this on my book. I decided to take a break but I was kinda feeling guilty lol, so I searched this up. And it became a lot clearer. Thanks man!

[@vcj8096]

Thank you so much for taking the time to share knowledge calmly with understanding. Liked and subscribed

[@chloe-marguerite]

You're a lifesaver!!! Thanks so much JG

[@shriyaasingh4932]

Mannn thank you🫶 you just saved my Cambridge exam

[@missfly4406]

Hey I'm still confused with this part. Is the enthalpy of formation of defined as difference of the sum of bond energies of the reactants from the products or the products from the reactants?

[@kcocrekcus8760]

Same😑

[@febronyao.3407]

Because that’s the formula for broken and formed bonds. It’s Delta H=summation of bond disassociation energy BROKEN BOND- summation bond disassociation energy of FORMED BONDS. So basically its energy absorbed-energy released Because energy is absorbed into breaking bonds and energy is released in forming bonds. That formula is specific to bond energy. So just remember it doesn’t follow the rule of products-reactants because that’s for heat formation.

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[@Edenchungkhoan]

I missed one class when my professor discussed abt this topic. Then I tryna look over and find the way out yet totally lost due to the complexity out of the way textbook explaining. 😖 This video really pulls me out though. Thank you!!!

[@khalidhuseyn7086]

Professor? Im in ks3 and im learning this bullshit

[@luiavalos92]

Man you got this on lock!

[@pickledmushrooms9720]

Correct me if I'm wrong, but in the first question the isn't the enthalpy change of formation supposed to be positive since it is an endothermic reaction?

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[@vanisethi5090]

To find the energy change can we also subtract the bonds formed from the bonds broken?

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DOUBT : DONE AND DUSTED

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[@temimafahrner428]

What happens when I need to calculate the enthalpy based on the Bond energy, but there are several different bonds in each molecule? Do I sum them up or multiply them by one another?

[@hmudisalam]

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[@scoobydoobydoo777]

You save my life 😭

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This video help me a lot

[@claraishungry501]

i wish i could thank you enough man

[@jamesyarbrough1248]

Saving my ap chem grade

[@arastheriver4421]

I'm a bit confused now. Didn't we have to put 0 for the energy of pure elements in their natural state?

[@psycho9554]

This is for bond diassociation enthalpy NOT for enthalpy formation

[@mikaelawriter6021]

Was perfectly explained and extremely helpful thanks so much

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Um I will be happy if u will teach the solution cycle topic properly on it own, I want to have a full concept on it not just solving it but wanna understand what I'm doing

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[@malcolmorrall8338]

Thanks for your clean and direct videos. Really nicely done. Glad to see in the comments you are getting the appreciation you deserve.

[@mahasaleh]

I thought delta h of the reaction was the sum of the product - the sum of the reactants and you have it the opposite way if I am not mistaken?!

[@himansutiwari6154]

Thank you sir your video is very useful i.e my concept is clear,thanks alot sir...

[@thegreatestofalltime9848]

My god I love ur work god bless u

[@samho2137]

why my note include the energy for condensation of water for calculation of enthalpy of combustion using bond energy?

[@lanirelano3180]

Thank you so much for this. It really is a big help.

[@nishikabagchi8799]

This was very helpful thank you

[@nadiakamran769]

Thanks.. it's helping me alot

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Hey King! I love you

[@maryamfatima7569]

can anyone explain me why he multiplied with 4 instead of 8? at 9:29 ??

[@brownbiriyani]

thank you so much :)

[@aminat_kelzbling5925]

Great video

[@JosephMillion-u4o]

Please may someone clarify because we used to be taught that it should be: enthalpy change =sum of enthalpy of products - sum of enthalpy of reactants

[@melissarainchild]

Thanks for posting. I looked up some data,at the first problem, I read an H-H disociation of 436, Cl-Cl of 242 and H-Cl of 432... I assume your sources are differnt...otherwise, I do get the drift, thanks for posting. I need your vids to get me through the exams :)

[@bigilpandi7722]

Dai jp for bde only reactant minus product for enthalpy product minus reactant

[@fredweker9106]

At what Bond disscociation Energy is a bond considered stable? Is 40 kJ/mol a stable bond?

[@EricaLwesha-cm4ri]

Example 2 answered my question

[@curtpiazza1688]

Wow....now I get it!!

[@CRYSTAL-dn5bk]

Thank you very much❤️❤️❤️❤️

[@duwarkaparsad4667]

Thanks sir you cleared my doubts

[@hakimusacca2781]

2:09 how did u come up with the equation

[@claraishungry501]

thats the formula, r-p

[@strictlyedits_123]

@@claraishungry501 for this formula,do we take the values from the list regardless of the sign? Like, for ex, product is -ve (exo)but the given value is +432, so should we take -432 or 432?

[@Hussaineditz]

Thanks very very helpful

[@wasabi4389]

heyyo this is super cool so thankyou but i have a doubt. If its supposed to be 1 mol then shouldn't the equation for combustion of methane be- 1/2CH4+O2=1/2CO2+2H20 ?

[@Trippify]

Isn't the first one Products-Reactants instead of other way round?

[@Lasted843]

Normally, yes, but for this equation, it'll be reactants - products.

[@mahdi2913]

StoeneWeala why would it be reactants - products? I’m not sure why it’s not products-reactants

[@doctoranon177]

For some reason, college textbooks and professors are useless at teaching this stuff. You either have to youtube it or already know it.

[@sccm100]

What about when you have products/reactants in the condensed phases yet you are asked to use bond enthalpies along with other enthalpies

[@SibahleMajiya]

How to find bond energy

[@evanr.battallio1115]

why is enthalpy for a reaction sum of [products]-sum of [reactants], but enthalpy of bonds is sum of [reactants]-sum of [products]

[@thabisombingo9649]

You didn't treat O2 the way u treated H2O and CO2

[@raheemsiddique3531]

Thanx bro..😉

[@overlordprincekhan]

Now I need yo know how to find that enthalpy energy. I mean how can I know that 'H-H' bond has only 427KJ/mole and not any other digits?

[@susa9786]

That's constant, in other words it's "a given" number.

[@quriositysquared1028]

Thanks a bunch

[@Harinijayasri_345]

Heyyy can you explain this with another example CH3-CH=CH2 +HBr ---> CH3-CHBr-CH3

[@Harinijayasri_345]

Like the values are c-c --> -348kj C=C ---> -612kj C-Br --->-276kj C-H --->-412kj H-Br --->-366kj

[@bisharofarah4431]

if there is 4 h-cl bond wouldn’t that give us 16 bonds for the hydrogen chlorine bond since we have to count each bond from 4 of the hydrogen chlorine bonds. I am really confused because that is how we did it in class.

[@jabtechnologies873]

exactly, last minute going through and i hit a brick wall😢

[@jabtechnologies873]

sorry just realised the 4 is a mole not the number of atoms of H therefore there was only 1 H - Cl bond

[@ahmadkhaled272]

What the different between reactant minus product and product minus reactant.Some1 plz help

[@Jaybee921]

So I thought it was products- reactants but you did it the other way?

[@johnlaux9378]

that works using this the Heat of Formation chart, in this case, the equation is different for bonding energies.

[@auriffarooq2740]

@@johnlaux9378 could u explain it further

[@Shorty50]

Basically when your working out the enthalpy of formation its products - reactants When your doing enthalpy of combustion it’s reactants - products Same with bond enthalpys it’s reactants - products

[@ojukwuifunanya3872]

THANK YOU

[@shirou.6243]

Anabolic reactions require an input of energy, and form larger molecules. But the formation of bonds release energy. While catabolic reactions form energy, but breaking bonds require energy. Can someone clarify this for me?

[@sweetie1208]

Thank youuuu

[@masteriq9787]

THANK YOU!

[@ShadNex]

You think someone solving 3 problem “normally” wouldnt be cool or something worth more then 100 views but by the views you can tell how many have so bad teachers thats you have to resort to someone solving a problem for knowledge, quite sad honestly

[@sweetsparkles6014]

Not necessarily bad teachers , maybe they r getting ready for summative assessments as me

[@jumiroy1853]

Thanks 🥰

[@akramat6586]

thanks a lot

[@LindiweMbewe-f9e]

Why was he adding 4 bonds instead of 2 for chlorine 11:38 11:38

[@shaheenkamal8925]

O=O bond is 498

[@haileyhung2694]

Thx so much

[@riteshrathwa7974]

what if i want to calculate enthalpy of formation of CO2, reaction is C+ O2 ---> CO2 and in this condition what is the value for Carbon?

[@Ikechickken458]

They will give you a table where there will be a energy change for carbon only and oxygen only

[@wengeance8962]

isnt the first problem exothermic because the resultant is negative?

[@melboo1179]

Correct. Positive is endothermic when energy is absorbed and negative is exothermic when energy is released.