
Czech: 
Řekneme si něco o entalpii vazeb
a o jejím využití pro výpočet
entalpie reakce.
Entalpie vazby představuje energii
potřebnou na rozbití jednoho molu vazby.
Takže jeden mol vazby.
Různé druhy vazeb mají
různé vazebné entalpie.
Například se podívejme
na vazbu uhlík-vodík,
což je jednoduchá vazba
mezi uhlíkem a vodíkem.
Tento uhlík je zřejmě navázán
ještě na další věci,
protože uhlík má obvykle více než
jednu jednoduchou vazbu.
Ale prozatím ignorujme všechno ostatní
navázané na tento uhlík,
jen si to znázorníme jako
velkou kaňku nebo jako popcorn.
Možná je to bílkovina,
možná je to molekula cukru,
může to být cokoli.
Tuhle kaňku zatím zanedbejme.
A ještě jedna věc,
na kterou jsem zapomněla

Bulgarian: 
Ще говорим за енталпията на връзките
и как чрез нея можем да
изчислим
енталпията на една реакция.
Енталпията на връзката е
енергията, която е необходима
на един мол от тази връзка.
Значи един мол от тази връзка.
Различните видове връзки
ще имат различни енталпии.
Можем да разгледаме връзката
въглерод-водород
или единична връзка
въглерод-водород.
Този въглерод може да
е свързан с други неща,
защото обикновено въглеродът
има повече от една единична връзка.
Но ние ще игнорираме всичко
друго, свързано с въглерода,
ще го представим като 
един голям балон или пуканка,
това може да е белтък,
или захарна молекула,
може да е много неща.
Но ние ще пренебрегнем
този балон.
Забравих да кажа по-рано,

Korean: 
우리는 결합엔탈피에 대해 알아보도록 하겠습니다
그리고  반응 엔탈피를  계산하기위하여
어떻게 그것을 여러분이 사용할수있는지도 알아보겠습니다
결합엔탈피는  어떤물질  1몰의 결합을
끊는데 필요로되는 에너지입니다
( 1몰의 결합)
즉 그래서 다른형태의  결합은 다른
결합에너지를 갖을 것입니다
예를 들어, 우리는 탄소와수소의 결합,또는 그들의 단일결합에 대하여
논해 볼수 있습니다
탄소는 주로 단일결합 보다 그이상을 가지고 있기 때문에
이 탄소는 아마도 다른 물질에 붙어져 있을것입니다
하지만 우리는 여기서 탄소에 붙어져 있는 다른것들을
무시한채 설명하겠습니다
우리는 그것을 팝콘같은 큰 방울로써 그것을 단지 표현할것이며
어쩌면 그것은 단백질일수도
당 분자가 될 수도,
그외에 많은 것일수도 있겠습니다
그러나 우리는 그 방울을 무시하고 설명하겠습니다
그리고  제가 그 이전에 미리 언급했어야할점은

English: 
- [Voiceover] We're gonna be
talking about bond enthalpy
and how you can use it to calculate
the enthalpy of reaction.
Bond enthalpy is the energy that it takes
to break one mole of a bond.
So one mole of a bond.
So different types of bonds will have
different bond enthalpies.
So as an example, we can talk about
a carbon hydrogen bond, or a
carbon hydrogen single bond.
So this carbon is probably
attached to some other stuff,
because carbons usually have
more than one single bond.
But we're gonna ignore everything else
attached to the carbon,
we're just gonna represent it
as a big blob, like popcorn,
maybe it's a protein, it could be,
it could be a sugar molecule,
it could be a lot of things.
But we're ignoring that blob.
And one other thing I
forgot to say earlier

Thai: 
เราจะพูดถึงเอนธาลปีพันธะ
และวิธีใช้มันคำนวณ
เอนธาลปีของปฏิกิริยากัน
เอนธาลปีพันธะคือพลังงานที่ใช้
ทำลายพันธะ 1 โมล
พันธะ 1 โมล
พันธะแบบต่างๆ จะมี
เอนธาลปีพันธะต่างกัน
ตัวอย่างเช่น เราพูดถึง
พันธะคาร์บอนไฮโดรเจน 
หรือพันธะเดี่ยวคาร์บอนไฮโดรเจน
คาร์บอนนี้น่าจะต่อกับอย่างอื่น
เพราะคาร์บอนมักมีพันธะเดี่ยวมากกว่าหนึ่งอัน
แต่เราจะไม่สนใจอย่างอื่น
ที่ต่อกับคาร์บอน
เราจะแทนมันด้วยก้อนใหญ่ๆ อันนี้เหมือนป๊อปคอร์น
มันอาจเป็นโปรตีน มันอาจ
เป็นโมเลกุลน้ำตาล มันอาจเป็นอย่างอื่นก็ได้
แต่เราจะไม่สนใจก้อนนั้น
อีกอย่างที่ผมลืมบอกก่อนหน้านี้

Thai: 
คือว่าพลังงานที่มันใช้
แตกพันธะ 1 โมลในสถานะแก๊ส
มันเป็นนิยามที่เจาะจงทีเดียว
ในกรณีของพันธะคาร์บอนไฮโดรเจน
เอนธาลปีพันธะของพันธะนี้
ถ้าเราแตกพันธะนี้ออกมา --
ลองวาดด้วยเส้นประกัน
ถ้าเราแตกพันธะนี้ --
เราต้องเพิ่มพลังงาน และสิ่งที่เราได้
เป็นผลิตภัณฑ์คือเราจะได้ป๊อบคอร์น
สิ่งที่เกิดขึ้นคือว่า เมื่อเราแตกพันธะนี้
อิเล็กตรอนสองตัวที่เดิมประกอบเป็นพันธะ
อิเล็กตรอนตัวหนึ่งจะไปอยู่กับคาร์บอน
และอีกตัวจะไปอยู่กับไฮโดรเจน
และเรามักแทนอิเล็กตรอนเดี่ยว
อย่างนั้นโดยใช้จุดเดี่ยว
เหมือนกับตอนคุณเขียนโครงสร้างลิวอิส
คุณเขียนอิเล็กตรอนคู่โดดเดี่ยวด้วยจุดสองจุด
ตรงนี้คือคาร์บอนที่มีหนึ่งจุด หรืออิเล็กตรอนหนึ่งตัว

Korean: 
이것은 기체 상태에서 물질 1몰의 결합을 끊는데
필요로되는 에너지라는 점입니다
그래서 그것은 꽤 구체적인 정의입니다
여기서 탄소와 수소결합 경우,
이 결합엔탈피는
만약 우리가 이결합을 끊는다면,
(여기에 점선을 긋겠습니다)
우리가 이 결합을 끊는다면
우리는 에너지를 추가해야 하며, 우리가 생성물질로서 얻게 되는것은
여기있는 팝콘 이겠습니다
우리가 이 둘사이의 결합을 끊을때  발생하는 현상은
원래 이 결합을 이루고 있는 두 전자들이,
전자들중 하나는 탄소로 갈것이며,
나머지 다른 하나의 전자는 수소로 갈것입니다
그리고 우리는 대개 이와 같은 한점을 이용하여
전자를 표현합니다
루이스의 전자점식을 적을때처럼,
여러분은 두개의 비공유 전자쌍을 찍을수 있겠습니다
이제 여기에 전자 한개를 가진 탄소가 있고

English: 
is that this is the energy it takes
to break one mole of a
bond in the gas phase.
So it's a pretty specific definition.
So in the case of our
carbon hydrogen bond,
the bond enthalpy of this bond,
so if we break this bond...
Let's do a sort of dotted line.
If we break this bond...
We have to add energy, and what we'll get
as our products is we'll get our popcorn,
and what happens is,
when we break this bond,
the two electrons that
originally made up the bond,
one of the electrons
will go to the carbon,
and the other electron'll
go to the hydrogen.
And we usually represent single electrons
like that using a single dot,
sort of like when you
write Lewis structures,
you can write lone pairs with two dots.
So here's our carbon with
one dot, or one electron,

Bulgarian: 
че ще говорим за енергията,
необходима за разкъсване
на един мол от връзката 
в газообразно състояние.
Това е много конкретна
дефиниция.
При тази въглерод-водородна
връзка
енталпията на връзката,
т.е. ако разкъсаме тази връзка...
Ще направя една прекъсната линия.
Ако разкъсаме тази връзка...
Трябва да внесем енергия
и ще получим
като продукти нашата пуканка и
какво ще имаме, след като
разкъсаме връзката?
Двата електрона, 
които образуват тази връзка,
единият от тях остава
при въглерода,
а другият отива с водорода.
Обикновено представяме
единичните електрони
като използваме една точка,
също като при Люисовите
структури,
можеш да запишеш една
електронна двойка като две точки.
Ето го въглерода с една точка
или един електрон,

Czech: 
je, že toto je energie potřebná
na rozbití jednoho molu vazby
v plynném skupenství.
Jde o poměrně konkrétní definice.
V případě vazby mezi
uhlíkem a vodíkem
je entalpie této vazby,
tedy když ji rozbijeme...
K rozbití této vazby
musíme dodat energii.
Jako produkt zůstane
náš popcorn,
a když zrušíme tuto vazbu,
tak se dva elektrony, které
původně tvořili tu vazbu, rozdělí.
Jeden z elektronů
půjde na uhlík,
a ten druhý
se přidá k vodíku.
Obvykle znázorňujeme
nepárový elektron pomocí jedné tečky,
podobně jako když zapisujete
Lewisovu strukturu,
tak můžete zapsat volné páry
pomocí dvou teček.
Tady je náš uhlík s jednou tečkou.,
tedy s jedním elektronem,

Korean: 
하나의 전자를 가진 수소가 있습니다
탄소 수소 모두 여전히 기체상태입니다
그래서 이 반응의 델타H 는 결합엔탈피입니다
BE로 축약하여 쓰겠습니다
이 결합엔탈피에 대해 유념해야할  중요한 점들은
결합 엔탈피는 항상 양의 의미라는것입니다
그것은 항상 에너지를 취할것이고
여러분이 결합을 끊기 위해서는 항상 에너지를 더해야할것입니다
만약 우리가 결합의 역을 취한경우는
만약 우리가 이 결합엔탈피의 역을 취한다면,
다시말해 우리가  여기 있는 이 반응을 뒤집는다면,
그래서 만약 우리가 이 반응의 역을 취한다면,
물론 그것은 우리가 결합을 할것이란 의미입니다
우리는 결합을 끊는다는것은 항상 에너지를 취한다는 것을 알고 있으므로,
결합시킨다는것은 에너지를 발산한다는 의미입니다

Czech: 
a náš vodík s jedním elektronem,
a oba jsou stále v plynném skupenství.
Takže delta H této reakce
je vazebná entalpie,
kterou zkrátím jako BE
(bond enthalpy).
Důležitá věc k zapamatování
ohledně entalpie vazeb je,
že entalpie vazby je vždy kladná.
Vždy potřebujete dodat energii.
abyste rozbili vazbu.
Pokud si vezmeme opačný děj,
neboli opak vazebné entalpie...
To znamená otočení této reakce.
Pokud vezmeme zpětnou reakci,
ve které vazbu vytváříme,
a protože víme, že rozbití vazby
vždy vyžaduje energii,
znamená to, že tvorba vazby
energii vždy uvolňuje.

Thai: 
และไฮโดรเจนของเรามีอิเล็กตรอนหนึ่งตัว
พวกมันอยู่ในสถานะแก๊สทั้งคู่
แล้วเดลต้า H ของปฏิกิริยานี้คือเอนธาลปีพันธะ
ซึ่งฉันจะย่อว่า BE
สิ่งสำคัญที่ต้องจำเรื่องเอนธาลปีพันธะ
คือว่าเอนธาลปีพันธะเป็นบวกเสมอ
มันจะต้องใช้พลังงาน
คุณจะต้องเพิ่มพลังงานเพื่อทำลายพันธะเสมอ
ถ้าเรากลับค่าพันธะ
ถ้าเรากลับค่าเอนธาลปีพันธะ
คิดอีกอย่างคือว่า เราพลิกปฏิกิริยานี้
ถ้าเราย้อนปฏิกิริยานี้
หมายความว่าเราจะสร้างพันธะ
เนื่องจากเรารู้ว่าการทำลายพันธะต้องใช้พลังงาน
การสร้างพันธะจึงปล่อยพลังงานเสมอ

English: 
and our hydrogen with one electron,
and these are both still in the gas phase.
So the delta H of this
reaction is the bond enthalpy,
which I will abbreviate as BE.
So some important things to
remember about bond enthalpy
are that bond enthalpy is always positive.
So it's always going to take energy,
you're always gonna have to
add energy to break a bond.
If we take the reverse of the bond,
if we take the reverse
of the bond enthalpy,
so another way to think about
this is to flip this reaction,
so if we take the
reverse of this reaction,
that means we're making a bond.
And since we know that breaking
a bond always takes energy,
that means making a bond
always releases energy.

Bulgarian: 
и водорода с един електрон.
Като те и двата са 
в газообразно състояние.
ΔН на тази реакция е 
енталпията на връзката,
която ще запиша съкратено като ЕВ.
Много важно е да запомниш
за енталпията на връзката,
че тя е винаги положителна.
За разкъсването ѝ винаги ще
е необходима енергия,
винаги ще използваш енергия,
за да разкъсаш една връзка.
Обратното на енталпията на връзката,
ако вземем обратната стойност,
това е все едно да обърнем
реакцията тук,
ако вземем обратното
на тази реакция,
това означава 
да създадем връзка.
И понеже разкъсването на връзка
винаги изисква енергия,
създаването на връзка
винаги ще отделя енергия.

English: 
So it will always be
negative to make a bond.
And that's another way of saying,
it will always release energy.
And then the third thing
that we're gonna discuss
about bond enthalpy is
that you can use it,
you can use bond enthalpy to
estimate delta H of reaction.
And delta H of reaction is,
or the enthalpy of reaction,
is something that chemists
are often interested in.
We wanna know if it's
exothermic or endothermic.
You might know that
there's lots of other ways
of calculating delta H of reaction,
such as using Hess's law...
Or another way is using
delta H of formation.
And then there are other ways too.
So this is just another
way that we can use
to calculate delta H of
reaction using bond enthalpies.

Bulgarian: 
Образуването на връзка
е винаги отрицателно.
Това е друг начин да кажем,
че винаги се освобождава енергия.
И третото нещо, което трябва
да кажа за енталпията на връзката, е,
че може да се използва за 
намиране на ΔН на реакцията.
ΔН на реакцията или 
енталпията на реакцията е
нещо, от което химиците
обикновено се интересуват.
Искаме да знаем дали един процес
е екзотермичен или ендотермичен.
Има много други начини
за изчисляване на ΔН на реакцията,
като Закона на Хес...
Или може да се използва
ΔН на образуване.
Има и други начини.
Това е просто един от начините
за изчисляване
на ΔН на една реакция
чрез енталпиите на връзките.

Czech: 
Tím pádem bude vždy
záporné při tvorbě vazby.
Jinými slovy, vždy uvolní energii.
A třetí věc, které se budeme věnovat
ohledně entalpie vazby, je
její využití pro odhad delta H reakce.
A delta H reakce, neboli
entalpie reakce,
je něco, co chemiky často zajímá.
Chceme vědět, zda je
exotermická nebo endotermická.
Možná víte, že je mnoho způsobů
jak vypočítat delta H reakce,
například použitím Hessová zákona.
Jiný způsob je použití
slučovacích entalpií.
A další jiné způsoby.
Takže toto je jeden
ze způsobů, jak
vypočítat delta H reakce,
použitím entalpií vazeb.

Korean: 
그러므로 결합은 항상 음의 의미를 가지고 있습니다
또 다른 표현으로는
항상 에너지를 방출할것입니다
결합에너지에 대해 우리가 살펴봐야할  3번째것은
여러분은 반응엔탈피를 측정하기 위하여
결합엔탈피를 이용할수 있다는것입니다
화학자들이 자주 관심을 갖고있는
이 반응엔탈피라는것은 이러합니다
만약 우리가 발열반응 인지 흡열반응인지 알고 싶을때
반응 엔탈피를 구하는 많은 다양한 방법이 있다는것을
여러분은 알고 있을것입니다
헤스의 법칙,
형성엔탈피를 사용하는것도 또다른 방법입니다
그리고 다른 방법도 있습니다
그러므로  이 결합엔탈피를 이용하여 반응엔탈피를 계산하는 것도
또하나의 방법입니다

Thai: 
มันจะต้องเป็นลบเพื่อสร้างพันธะ
มันก็คือการบอกว่า
มันจะปล่อยพลังงานเสมอ
แล้วเรื่องที่สามที่เราจะพูดถึง
เกี่ยวกับเอนธาลปีพันธะคือว่า คุณใช้มัน
คุณใช้เอนธาลปีพันธะเพื่อประมาณค่า
เดลต้า H ของปฏิกิริยาได้
และเดลต้า H ของปฏิกิริยาคือ
หรือเอนธาลปีของปฏิกิริยา
คือสิ่งที่นักเคมีมักสนใจ
เราอยากรู้ว่ามันเป็นแบบคายความร้อน
หรือดูดความร้อน
คุณอาจรู้ว่ามันมีวิธีอื่นๆ
เพื่อคำนวณเดลต้า H ของปฏิกิริยา
เช่นการใช้กฎของเฮส --
หรืออีกวิธีคือการใช้เดลต้า H ของการเกิด
แล้วมันยังมีวิธีอื่นๆ ด้วย
นี่เป็นเพียงวิธีอีกอย่างที่เราใช้
คำนวณเดลต้า H ของปฏิกิริยาโดยใช้
เอนธาลปีพันธะ

Thai: 
เราจะทำตัวอย่างเป็นอย่างต่อไป
ปฏิกิริยาตัวอย่างคือการนำโพรไพน์ (propine)
ซึ่งก็คือแก๊ส C3H4 --
และทำปฏิกิริยากับไฮโดรเจน  แก๊สไฮโดรเจน
ได้เป็นโพรเพน (propane) คือแก๊ส C3H8
ฉันไม่รู้ว่าคุณคิดยังไง
แต่เวลาดูสูตรเคมีอย่างนี้
ฉันไม่รู้ว่าโมเลกุลหน้าตาเป็นอย่างไร
งั้นฉันจะวาดโครงสร้างลิวอิสนะ
โครงสร้างลิวอิสของโพรไพน์
โพรไพน์มีคาร์บอน 3 ตัวและพันธะสาม
พันธะสามระหว่างคาร์บอนกับคาร์บอน
แล้วมันมีไฮโดรเจน 4 ตัว
นั่นคือโพรไพน์
และเรายังมีแก๊สไฮโดรเจน
ผลิตภัณฑ์ของเราก็คือโพรเพน
โพรเพนมีพันธะเดี่ยวหมด

English: 
So we're gonna go through
an example of that next.
So the example reaction is taking propyne,
which is C3H4 gas...
And reacting it with
hydrogen, so hydrogen gas,
to get propane, C3H8 gas.
And I don't know about you,
I'm pretty bad at looking at
a chemical formula like this
and knowing exactly what
the molecule looks like,
so I'm gonna draw out
the Lewis structures.
So the Lewis structure for propyne,
propyne has three carbons, and one triple,
one carbon carbon triple bond,
and then it has four hydrogens.
So that's propyne.
And we also have hydrogen gas.
And our product is propane, so
propane has all single bonds.

Czech: 
Teď si ukážeme příklad.
Jako příklad si vezmeme
reakci propynu,
což je plynný C₃H₄,
který zreaguje s plynným vodíkem.
Produktem je plynný propan,
C₃H₈.
A nevím jak vy,
ale nejsem moc dobrá v odhadu
struktury molekuly jen z molekulového vzorce.
Uděláme se strukturní vzorec.
Strukturní vzorec propynu.
Propyn má tři uhlíky,
a jednu trojnou vazbu
mezi uhlíkem a uhlíkem,
a ještě má čtyři vodíky.
Tohle je propyn.
A dále máme plynný vodík.
A náš produkt je propan,
který má všechny vazby jednoduché.

Bulgarian: 
Нека да видим един пример.
В тази примерна реакция
имаме пропин (метилацетилен),
който е газ с формула С3Н4.
Той реагира с водород,
значи плюс газообразен водород,
и се получава газообразен
пропан С3Н8.
Не знам за теб,
но на мен ми е трудно 
да погледна една такава формула
и да разбера как точно
изглежда молекулата,
затова ще направя 
Люисовата структура.
Люисовата структура 
на пропина е...
имаме три въглеродни атома,
една тройна въглерод-въглерод връзка,
и след това имаме четири
водородни атома.
Това е пропина.
Имаме също 
газообразен водород.
Получаваме пропан, който 
има само единични връзки.

Korean: 
자 ,이제, 우리는 그러한 다음 예를 살펴보겠습니다
그 예는 프로핀입니다
이는 C3H4 기체입니다
그리고 그것이 수소기체와 반응하여
프로판, C3H8 기체를 얻을 수 있습니다
여러분들에 대해 제가 잘은 모르지만,
저는 이러한 화학적 수식을 보는것을 잘하지 못하지만
이 분자들이 어떤 모습인지는 정확히 알고 있습니다
그러므로, 저는 루이스 구조를 그리겠습니다
그러므로 프로핀에대한 루이스 구조식을 보면,
프로핀은 세 개의 탄소를 가지고 있으며, 트리플 하나,
다시말해,탄소-탄소의 삼중결합,
다음은 네 개의 수소들이 있습니다
저것이 프로 핀입니다
그리고 우리는 또한 수소 기체를 가지고 있습니다
그래서 프로판이 생성물질이 되고,프로판은 모두 단일 결합들입니다

Thai: 
คาร์บอน 3 ตัวที่มีพันธะเดี่ยว
และไฮโดรเจน 8 ตัวอยู่กับคาร์บอน
นั่นคือปกฏิกิริยาที่เราสนใจ
แล้วสิ่งที่เราอยากรู้ตรงนี้คือว่า 
เดลต้า H ของปฏิกิริยาเป็นเท่าใด?
และเราจะคำนวณมันโดยใช้
เอนธาลปีพันธะได้อย่างไร?
เราบอกไปก่อนหน้านี้ว่าเอนธาลปีพันธะ
เอนธาลปีพันธะคือพลังงานที่ใช้แตกพันธะ
สิ่งที่เราจะทำต่อไปคือดูปฏิกิริยา
ในแง่ที่ว่ามันทำลายพันธะอะไร
และสร้างพันธะอะไร
มันง่ายขึ้นมากเวลาใช้โครงสร้างลิวอิส
อย่างแรก ลองคุยกันก่อนว่าพันธะไหนแตกบ้าง
ถ้าเราเปรียบเทียบสารตั้งต้นกับผลิตภัณฑ์
เราจะแตกพันธะสามคาร์บอน-คาร์บอนนี้
ถ้าเราแตกพันธะสามคาร์บอน-คาร์บอนนี้
เราจะจะแตกพันธะไฮโดรเจน-ไฮโดรเจน
และสิ่งที่เราลืมทำ
ซึ่งสำคัญสุดๆ
คือเราต้องแน่ใจว่าปฏิกิริยาของเรานั้นดุลแล้ว

English: 
So three carbons with single bonds,
and eight hydrogens bound to the carbons.
So that's the reaction
we are interested in,
and what we wanna know here is
what is delta H of reaction?
And how can we calculate
it using bond enthalpies?
We said earlier that bond enthalpies,
a bond enthalpy is the energy
it takes to break a bond.
So what we're gonna do next
is look at our reaction
in terms of what bonds are
broken and what bonds are formed.
And this is a lot easier to
do using the Lewis structures.
First let's talk about
which bonds are broken.
We, if we compare our
reactants and our products,
we're breaking this
carbon carbon triple bond.
If we're breaking this
carbon carbon triple bond,
and we're also gonna break
this hydrogen hydrogen bond,
and one thing we forgot to do earlier
which is super important,
is we actually need to make
sure our reaction is balanced.

Bulgarian: 
Значи три въглерода
с единични връзки,
осем водорода,
свързани с въглеродите.
Това е реакцията, която 
ни интересува
и търсим ΔН за тази реакция.
Как можем да я намерим,
като използваме енталпиите на връзките?
По-рано казахме, че енталпиите
на връзките...
енталпията на връзката
е енергията за нейното разкъсване.
Затова ще разгледаме реакцията
от гледна точка на разкъсаните
и създадените връзки.
Това е много лесно
с Люисовите структури.
Първо да видим кои
връзки са разкъсани.
Ако  сравним изходните вещества
и продуктите,
разкъсва се тази тройна
 връзка въглерод-въглерод.
Ако разкъсаме тази тройна връзка,
ще разкъсаме и тази
връзка водород-водород...
но забравихме нещо много
важно,
трябва да се уверим,
че уравнението ни е изравнено.

Korean: 
그래서 단일 결합한 3개의 탄소,
탄소에 결합된 8개의 수소들이 여기에 있습니다
그래서  그것이 우리가 관심갖고 있는 반응입니다
그리고 우리가  여기서 알고자하는것은  "반응엔탈피는 무엇인가?"와
"결합엔탈피를 이용하여 어떻게 반응엔탈피를 계산할것인가? "입니다
우리는 앞에서 결합엔탈피란
어떤 결합을 끊는데 필요로 되는 에너지임을 언급했습니다
그래서 이 반응에서 우리가 다음으로 살펴봐야할것은
어떤결합이 끊어지고  어떤결합이 형성되는가라는 관점에서 봐야합니다
그리고 이것은 루이스구조를 이용하면 훨씬 쉽습니다
먼저, 어떤 결합이 끊어지는지를 보겠습니다
만약 우리가 반응물질과 생성물질을 비교해보면,
우리는 이 탄소 - 탄소 삼중 결합을  끊겠습니다
우리는 이 탄소 - 탄소 삼중 결합을 끊고
그리고 이  수소-수소 결합도 끊겠습니다
그리고 앞서서 미리 했어야할것중 우리가 망각한  한가지는,
(아주 중요한 것입니다)
우리는 이 반응이 균형을 이루어야함을 확실히 할 필요가 있습니다

Czech: 
Tři uhlíky s jednoduchými vazbami,
a osm vodíků navázaných na uhlíky.
Tak toto je reakce
která nás zajímá,
a chceme zjistit,
jaká je delta H reakce?
A jak ji můžeme vypočítat
pomocí vazebných entalpií?
Řekli jsme si, že entalpie vazby
je energie potřebná k rozbití vazby.
Teď se podíváme na naši reakci
a určíme,
které vazby se
ruší a které jsou tvořeny.
A to je mnohem jednodušší
za použití Lewisových struktur.
Nejprve si řekněme,
které vazby se přetrhnou.
porovnáním reaktantů a produktů.
Roztrhneme tuto trojnou vazbu uhlík-uhlík.
a také trháme tuto vazbu mezi vodíky.
Zapomněli jsme ale na jednu věc,
která je strašně důležitá.
Musíme si tu rovnici vyčíslit.

Bulgarian: 
Имаме четири плюс две,
шест водорода от страната на
изходните вещества,
а имаме осем водорода
при продуктите.
Това не е изравнено.
Затова ни трябват две молекули водород
при изходните вещества.
Ще нарисувам още една.
Казахме, че разкъсваме
връзката водород-водород,
но ние всъщност разкъсваме
две такива водородни връзки.
Важно е да следим
колко връзки от всеки вид разкъсваме,
защото енталпията на връзката
е за мол,
така че ако тук имаме два мола,
ще ни е необходима два пъти повече енергия за разкъсване на тези връзки.
И сега да видим връзките,
които се образуват.
Имаме... тъй като разкъсахме
тази тройна връзка въглерод-въглерод,
това означава, че се образува 
нова връзка,
и тази нова връзка в нашия продукт
е единична връзка
въглерод-въглерод.
Не само образуваме
нова единична връзка
между тези два въглерода, но сега 
те са свързани с много водороди,

Czech: 
Máme čtyři plus dva,
šest vodíků na straně reaktantů,
a máme osm vodíků na straně produktů.
To není vyčisleno.
Potřebujeme dvě molekuly vodíku
na straně reaktantů.
Řekli jsme si, že trháme
vazbu vodík vodík,
ale ve skutečnosti trháme
dvě vazby vodík vodík.
Je důležité si hlídat,
kolik vazeb každého druhu rušíme,
protože entalpie vazby je na mol,
tedy pokud máte dvakrát tolik molů,
je nutná dvojnásobná energie
na rozbití všech těch vazeb.
Teď se můžeme podívat
na všechny vazby, které vznikají.
Jelikož jsme rozbili tuto
trojnou vazbu uhlík uhlík,
museli jsme také vytvořit
novou vazbu mezi uhlíky.
A ta nová vazba v molekule produktu
je tato jednoduchá vazba uhlík uhlík.
Kromě nové jednoduché
vazby mezi těmito dvěma uhlíky,
je na uhlíky také navázáno několik vodíků.

Korean: 
우리는 4더하기 2
즉 6개의 수소를  반응물측에 가지고 있고
그리고 8개의 수소를 생성물측에 가지고 있습니다
즉, 균형을 이루지 못한상태입니다
그래서 우리는 실제로 두 개의 수소를
반응물측에 더해야 합니다
그럼, 하나 더 그려 보겠습니다
우리는 수소-수소 결합을 깨고 있습니다
우리는 실제로 2개의 수소- 수소 결합을 깨고 있습니다
우리가 몇개의 각 결합을 끊고 있는지를
잘 기억하는것은 중요합니다
왜냐하면 결합엔탈피는 1몰의 결합을 끊는데 필요한 에너지이기 때문입니다
만약 여러분이 2배의 몰을 끊는다면,
그 결합들을 끊기위해서는 2배 만큼 많은양의 에너지가 필요할것입니다
우리는 이제 끊어진 결합을 볼수 있습니다
그래서 우리는
이 탄소 - 탄소 삼중 결합을 끊었기 때문에
그 의미는 우리는 새로운 결합을 만들필요가 있었고
생성물측면에 우리가 만든 새로운 결합은
이 탄소 - 탄소 단일 결합입니다
우리는 이 2 탄소들 사이에 새로운 단일 결합을 형성했을 뿐만 아니라,
또한 이제 이 탄소들은
수소의 무리에 연결되어

Thai: 
เรามี 4 บวก 2
ไฮโดรเจน 6 ตัวทางด้านสารตั้งต้น
และเรามีไฮโดรเจน 8 ตัวสำหรับด้านผลิตภัณฑ์
มันไม่สมดุล
เราต้องการโมเลกุลไฮโดรเจน 2 ตัว
ทางด้านสารตั้งต้น
ลองวาดอีกตัวลงไป
ใช่ เราบอกว่าเราจะแตกพันธะไฮโดรเจน-ไฮโดรเจน
เราจะแตกพันธะไฮโดรเจน-ไฮโดรเจน 2 ตัว
เราต้องติดตาม
จำนวนของพันธะแต่ละอันที่เราแตก
เพราะเอนธาลปีพันธะมีค่าเป็นต่อโมล
ถ้าคุณมีโมลมากเป็นสองเท่า
มันจะใช้พลังงานมากเป็นสองเท่า
เพื่อแตกพันธะเหล่านั้น
แล้วเราก็ไปดูพันธะที่สร้างขึ้นได้
เนื่องจากเราได้แตก
พันธะสามคาร์บอน-คาร์บอนนี้แล้ว
นั่นหมายความว่าเราต้องการพันธะใหม่
และพันธะใหม่ที่เราสร้างในโมเลกุลผลิตภัณฑ์
คือพันธะเดี่ยวคาร์บอน-คาร์บอนนี้
ไม่ใช่แค่เราสร้างพันธะเดี่ยวใหม่
ระหว่างคาร์บอนสองตัวนี้ แต่คาร์บอนเหล่านี้
ยังติดกับไฮโดรเจนอีกหลายตัว

English: 
And we have four plus two,
six hydrogens on our reactant side,
and we have eight hydrogens
on our product side.
That's not balanced.
So we actually need two hydrogen molecules
on the reactant side.
So let's draw one more in.
So yes, we said we are breaking
a hydrogen hydrogen bond,
we're actually breaking two
hydrogen hydrogen bonds.
It's important to keep track of
how many of each type
of bond we're breaking
because the bond enthalpy is per mole,
so if you have twice as many moles
it'll take twice as much energy
to break all of those bonds.
And then we can look at
the bonds that are formed.
So we have, not, since we broke
this carbon carbon triple bond,
that means we needed to make a new bond,
and the new bond we made
in our product molecule
is this carbon carbon single bond.
Not only did we form a new single bond
between these two carbons,
but now these carbons
are attached to a bunch of hydrogens,

Bulgarian: 
така че тук имаме четири нови
въглерод-водород връзки.
Нека го запиша, 
за да можем да го следим,
когато правим окончателната
калкулация на ΔН на реакцията.
Ако само погледнем
разкъсаните връзки...
Връзките, които разкъсахме...
Имаме тройна връзка
въглерод-въглерод
и две връзки водород-водород.
Нека само да запишем
по колко имаме от вид,
тъй като това ще ни трябва
за изчисленията.
Имаме една тройна връзка
въглерод-въглерод,
и имаме две връзки
водород-водород, които се разкъсват.
И сега можем да видим
техните енталпии,
които са в килоджаули на мол.
Енталпиите на връзките
можеш да намериш
в учебника или онлайн,
и те обикновено са като таблици.
Единиците са обикновено
килоджаули на мол,

Korean: 
그래서 우리는 4개의 새로운 탄소 -수소 결합을 만들었습니다
그것들을 잘 기억할수 있도록 적겠습니다
우리가 우리의 최종 반응엔탈피 계산을 할때,
우리가 이 끊어진 결합만을 본다면,
우리가 끊은 결합,
우리는 탄소 - 탄소 삼중 결합을 가지고 있고
그리고 우리는 2개의 수소-수소결합을 가지고 있으며,
이곳에 우리가 가진 결합의 수를 적겠습니다
왜냐하면 우리는 우리의 계산과정에서 그것이 필요합니다
그래서 우리는 1개의 탄소- 탄소 삼중 결합을
그리고 2개의 수소-수소 결합을,
그리고 우리는 그 결합들의 엔탈피도 볼수 있습니다
즉 1몰당 킬로줄(kilojoules) 말입니다
결합 엔탈피는  온라인상이나 여러분의
교과서에서 찾아볼수 있습니다
일반적으로 결합엔탈피 표로 나와 있습니다
그리고 단위는 몰당 킬로쥴입니다

English: 
so we made four new carbon hydrogen bonds.
So let's write that out so
that we can keep track of them
when we do our final calculation
of delta H of reaction.
So if we just look at the bonds broken...
The bonds we broke...
We have a carbon carbon triple bond,
and we have a couple
hydrogen hydrogen bonds.
Let's also just write down
how many of each we have,
because we'll need that
for our calculation.
So we have one carbon carbon triple bond,
and we have two hydrogen
hydrogen bonds that are broken.
And then we can also look
up their bond enthalpies,
which are in kilojoules per mole.
Bond enthalpies you can typically look up
in your textbook or online,
and they usually come in a
table of bond enthalpies.
And so the units can
be kilojoules per mole,

Czech: 
Vytvořily se čtyři nové
vazby uhlík-vodík.
Rozepíšme si to,
abychom na ně nezapomněli,
až budeme dělat výpočet reakční entalpie.
Podívejme se na rozbité vazby.
Roztrhli jsme trojnou vazbu uhlík uhlík,
a také pár vazeb vodík vodík.
Napišme si i kolik kterých
vazeb jsme rozbili.
Budeme to potřebovat pro výpočet.
Máme jednu trojnou vazbu uhlík uhlík,
a dvě vazby vodík vodík,
které byly roztrženy.
Nyní si můžeme vyhledat jejich entalpie,
které jsou udány v kilojoulech na mol.
Entalpie vazeb si můžete vyhledat
ve vaší učebnici nebo online.
Obvykle jsou uspořádány v tabulce.
Jednotky mohou být kilojouly na mol,

Thai: 
เราได้สร้างพันธะคาร์บอนไฮโดรเจนใหม่ 4 ตัว
ลองเขียนมันออกมา เราจะได้ติดตามพวกมันได้
เวลาคำนวณเดลต้า H ของปฏิกิริยาตอนจบ
ถ้าเราดูพันธะที่แตก --
พันธะที่เราทำลาย --
เรามีพันธะสามคาร์บอน-คาร์บอน 1 ตัว
เรามีพันธะไฮโดรเจน-ไฮโดรเจน 2 ตัว
ลองเขียนลงไปว่าเรามีแต่ละอันกี่ตัว
เพราะเราจะใช้ในการคำนวณ
เรามีพันธะสามคาร์บอน-คาร์บอน 1 ตัว
และเรามีพันธะไฮโดรเจน-ไฮโดรเจน 2 ตัวที่แตกออก
แล้วเราก็ดูเอนธาลปีพันธะได้เช่นกัน
ซึ่งมีหน่วยเป็นกิโลจูลต่อโมล
เอนธาลปีพันธะ คุณหาใน
หนังสือเรียนหรือออนไลน์ได้
พวกมันมากอยู่ในตารางเอนธาลปีพันธะ
และหน่วยเป็นกิโลจูลต่อโมล

Czech: 
někdy se můžete setkat
s kaloriemi nebo kilokaloriemi na mol.
Tyto hodnoty entalpií jsem si už vyhledala.
Trojitá vazba uhlík uhlík má entalpii
835 kilojoulů na mol,
Vazba vodík vodík má entalpii
436 kilojoulů na mol.
Teď se podívejme na vytvořené vazby.
Máme jednoduchou vazbu uhlík uhlík,
která je vytvořena právě jednou.
A entalpie této vazby,
také v kilojoulech na mol, je
346.
A v neposlední řadě
vytváříme vazbu uhlík vodík,
a takových máme čtyři.
Každá z nich má vazebnou entalpii
413 kilojoulů na mol.

Bulgarian: 
но понякога са калории
или килокалории на мол.
Вече съм проверила
енталпиите на тези връзки.
Тройната връзка 
въглерод-въглерод
има енталпия 835 килоджаула на мол,
а връзката водород-водород
има енталпия 
436 килоджаула на мол.
Като погледнем новите връзки,
имаме единична връзка
въгерод-въглерод.
Образува се една такава връзка.
Енталпията на тази връзка
е 346 килоджаула на мол.
И накрая имаме образуване
на връзки въглерод-водород.
Имаме четири такива връзки, като
енталпията за всяка от тях
е 413 килоджаула на мол.

English: 
sometimes you'll also see
calories or kilocalories per mole.
I already looked up these
bond enthalpy values.
So carbon carbon triple
bonds have a bond enthalpy
of 835 kilojoules per mole,
and hydrogen hydrogen
bonds have a bond enthalpy
of 800, sorry, 436 kilojoules per mole.
And then next, if we look at
the bonds that are broken,
we have a carbon carbon single bond.
And we have one of those bonds forming.
And the bond enthalpy for that,
which is also in terms of
kilojoules per mole, is 346.
And last but not least, we have the
carbon hydrogen bonds that we're forming,
and we have four of
those, and each of those,
the bond enthalpy is
413 kilojoules per mole.

Korean: 
때때로 여러분은 또한 몰당 칼로리나 몰당 킬로칼로리 단위도 볼수있습니다
저는 이미 이것들의 결합엔탈피를 조사해봤습니다
그래서 탄소- 탄소 삼중
결합은 결합 엔탈피를
몰당 835 킬로쥴 가지고 있고
수소-수소
결합은 결합 엔탈피가
800 ,죄송합니다 몰 당 436 킬로쥴입니다
그리고 다음 단계로 우리는 끊어진 결합들을 살펴봐야합니다
우리는 탄소 - 탄소 단일 결합을 가지고 있습니다
그리고 우리는 형성하고 있는 결합중 하나를 가지고 있고
그리고 그에 대한 결합엔탈피는
몰 당 킬로 줄 (346)입니다
그리고 마지막으로, 우리는
우리가 형성하고 있는 탄소 수소 결합
4개를 가지고 있고 ,각각 결합의 엔탈피는
몰 당 413 킬로쥴입니다

Thai: 
บางครั้ง คุณจะเห็นเป็นแคลอรี่ 
หรือกิโลแคลอรี่ต่อโมล
ผมหาค่าเอนธาลปีพันธะเหล่านี้ไว้แล้ว
พันธะสามคาร์บอน-คาร์บอนมีเอนธาลปีพันธะ
เท่ากับ 835 กิโลจูลต่อโมล
และพันธะไฮโดรเจน-ไฮโดรเจนมีเอนธาลปีพันธะ
เป็น 800 โทษที 436 กิโลจูลต่อโมล
แล้วต่อไป ถ้าเราดูพันธะที่สร้างใหม่
เรามีพันธะเดี่ยวคาร์บอน-คาร์บอนเกิดขึ้น
และเรามีพันธะหนึ่งในนั้นเกิดขึ้น
และเอนธาลปีพันธะสำหรับอันนั้น
อยู่ในรูปกิโลจูลต่อโมล เท่ากับ 346
และสุดท้ายแต่สำคัญยิ่ง เรามี
พันธะคาร์บอน-ไฮโดรเจนเกิดขึ้น
เรามีพันธะนั้น 4 ตัวและแต่ละตัว
เอนธาลปีพันธะเท่ากับ 413 กิโลจูลต่อโมล

Thai: 
ตอนนี้เราใช้ข้อมูลทั้งหมดนี้
นำมาคำนวณเดลต้า H ของปฏิกิริยาได้
เดลต้า H ของปฏิกิริยา ถ้าเราคิดถึงมัน
ในรูปของพันธะที่สร้างและทำลาย
มันคือการเปลี่ยนแปลงพลังงานทั้งหมด
ระหว่างที่มีปฏิกิริยา
มันก็แค่พลังงานที่ใช้
ทำลายพันธะทั้งหมดในสารตั้งต้น --
เพื่อทำลายพันธะสามคาร์บอน-คาร์บอนนี้
กับพันธะไฮโดรเจน-ไฮโดรเจน 2 ตัว
บวกพลังงานที่ใช้สร้างพันธะ
เพื่อสร้างพันธะผลิตภัณฑ์ใหม่
เราบอกไปก่อนหน้านี้ว่าคุณ
ต้องเพิ่มพลังงานเพื่อแตกพันธะเสมอ
เอนธาลปีพันธะจึงเป็นบวกเสมอ
เราจึงรู้ว่าการคำนวณส่วนนี้
ควรเป็นบวกเสมอ
ความหมายคือว่ามันปล่อย
พลังงานเวลาสร้างพันธะใหม่เสมอ

Czech: 
Nyní tedy vezmeme všechny tyto informace
a spojíme je na výpočet
reakční entalpie.
Delta H reakce, pokud se nad
tím zamyslíme
ve smyslu vazeb tvořených a rušených,
je celková změna energie
v průběhu reakce.
A tedy je to pouze energie potřebná
na rozbití všech našich
vazeb v reaktantů...
Takže na rozbití této
trojité vazby uhlík uhlík
a těchto dvou vazeb vodík vodík,
plus energie uvolněná
vytvořením vazeb.
Už jsme si řekli, že na rozbití vazeb
vždy musíte dodat energii,
tedy entalpie vazby je vždy kladná,
takže víme, že tato část našeho výpočtu
by měla být vždy kladné číslo.
To znamená, že se energie vždy
uvolní při tvorbě nových vazeb,

Korean: 
그래서 지금 우리는이 모든 정보를 가지고 있고
반응엔탈피를 구하기 위하여 합해보겠습니다
형성되고 끊어진다는 측면에서
반응 엔탈피는
그것은 반응하는 과정동안에 발생하는 에너지변화 총량입니다
그러므로 그것은 반응물측에서 모든결합들을
끊기위해 필요한 모든 에너지입니다
그래서 이 탄소 -탄소 삼중 결합과
두 수소- 수소 결합을 끊기 위하여
그리고 , 새로운 생성결합을 만들기위하여
필요한 에너지를 덧붙혀야 합니다
저는 앞에서부터 여러분게 항상 말씀드렸습니다
결합을 끊기위해서는 에너지를 추가해야 하므로
결합에너지는 항상 양수라고 말입니다
그래서 우리는 우리의 계산이
항상 양수이어야함을 알고 있습니다
그것은 이런 의미입니다
새로운 결합을 만들기위해선 에너지를 방출하고

English: 
So now we can take all of this information
and put it together to
calculate delta H of reaction.
So delta H of reaction,
if we're thinking about it
in terms of bonds made and broken,
it's a total energy
change during a reaction.
And so it's just the energy it takes
to break all of our
bonds in the reactants...
So to break this carbon carbon triple bond
and the two hydrogen hydrogen bonds,
plus the energy it
takes to make the bonds,
to make new product bonds.
We said earlier that you always
have to add energy to break bonds,
so bond enthalpy is always positive,
so we know this part of our calculation
should always be a positive number.
What that means is that it always
releases energy to make new bonds,

Bulgarian: 
Сега можем да вземем
цялата тази информация,
да я заместим и 
да изчислим ΔН на реакцията.
ΔН на реакцията 
от гледна точка на
разкъсани и създадени връзки,
е общата промяна
на енергията при реакцията.
Това е просто енергията, 
необходима
за разкъсване на връзките
в изходните вещества...
За разкъсване на тази
тройна връзка въглерод-въглерод
и две връзки
водород-водород,
плюс енергията от 
създаването на връзки,
за създаването на новите 
връзки в продуктите.
По-рано казах, че винаги
добавяме енергия, за да разкъсаме връзки,
така че енталпията на връзките 
е положителна,
така че знаем, че тази част 
от изчислението
винаги  ще бъде
положителна.
Това означава, че винаги
се освобождава енергия
при образуване на нови връзки,

Bulgarian: 
и тогава стойността на ΔН 
става по-отрицателна.
Така че тези числа тук,
когато говорим за
сбора на енергията, когато
имаме нови връзки,
те трябва да са със знак минус.
И сега да заместим стойностите, които имаме
за енталпия на връзките
за всички тези връзки,
които се  създават или разкъсват
в реакцията.
Да започнем с връзките,
които се разкъсват.
Имаме тройна връзка 
въглерод-въглерод,
за която са нужни
 835 килоджаула за мол,
и тя е само една.
Също така трябва да разкъсаме
две връзки водород-водород,
значи 2 по 436 килоджаула на мол,
което е енталпията на тази връзка.
Това са всички връзки, 
които разкъсваме.
Сега да прибавим енергията,
която се освобождава
при образуване на нови връзки.
Имаме единична връзка
въглерод-въглерод.
Това са 346 килоджаула на мол
със знак минус,
защото енергията се освобождава.

Korean: 
에너지가 방출되므로 반응엔탈피는 음수가 된다는 의미입니다
그래서 여기에서 우리가 에너지를 추가한다고 말할때는
그것은 새로운 결합을 만들때 이므로
이 수는 음수이어야 합니다
이제 우리의 반응에서 만들어지고 끊어진
이 모든 결합들을 위한 결합엔탈피를 구하기 위해
이 값들을 더해 보겠습니다
끊어진 결합들을 먼저 시작하겠습니다
그래서 우리는  탄소- 탄소 단일 결합은
즉, 몰 당 835 킬로줄이 필요할것이고
우리는 그 중 하나를 가지고 있습니다
그리고 우리는 또한 
2개의  수소- 수소 결합을 끊어야합니다
그래서 몰 당  436 킬로줄 에 2를  곱하면
즉 그 값이 그 결합의 결합 엔탈피입니다
그것이 우리가 끊은 모든 결합입니다
이제 우리는 새로운 결합을 만들때
방출된 에너지를 더해야 합니다
우리는  여기에  탄소 -탄소 단일 결합이 있습니다
그것은 몰당  346킬로쥴이며 음수가 되겠습니다
그 에너지가 방출되기 때문입니다

English: 
and when energy is released,
delta H becomes more negative.
So this number here,
when we're talking about
adding up the energy it
takes to make new bonds,
these should be negative numbers.
So now let's plug in the values
we have for bond enthalpy
for all of these bonds that are
made and broken in our reaction.
Let's start with the
bonds that are broken.
So we have our carbon carbon single bond,
that will require 835 kilojoules per mole,
and we have only one of them.
And we also have to break
two hydrogen hydrogen bonds,
so two times 436 kilojoules per mole,
which is the bond enthalpy of that bond.
So that's all of the bonds we break.
Now we have to add up the
energy that's released
when we make the new bonds.
So we have this carbon carbon single bond.
So that is 346 kilojoules per
mole, and that's negative,
because that energy is released.

Czech: 
a když se uvolní energie,
delta H je záporná.
Takže když sčítáme energie
uvolněné tvorbou nových vazeb,
zde by měly být vždy záporná čísla.
Vložme nyní naše hodnoty
pro entalpie vazeb
pro všechny tyto vazby,
vytvořené a rozbité, do naší reakce.
Začněme s vazbami,
co se rozbily.
Máme tedy naši trojnou
vazbu uhlík uhlík,
která bude vyžadovat
835 kilojoulů na mol,
a je jen jedna.
A také musíme rozbít dvě
vazby vodík vodík,
tedy dva krát
436 kilojoulů na mol,
což je entalpie pro tu vazbu.
Tak to máme všechny vazby, co roztrhneme.
Nyní musíme sečíst veškerou
energii, která se uvolní,
když vytvoříme nové vazby.
Takže máme tuto jednoduchou
vazbu uhlík uhlík.
To je 346 kilojoulů na mol,
a je záporná
protože ta energie je uvolněná.

Thai: 
และเมื่อพลังงานถูกปล่อยออกมา
เดลต้า H จะกลายเป็นลบยิ่งขึ้น
เลขนี่ตรงนี้ เมื่อเราพูดถึง
การเพิ่มพลังงานที่ใช้สร้างพันธะใหม่
ค่าเหล่านี้ควรเป็นลบ
ทีนี้ ลองแทนค่าที่เรามี คือเอนธาลปีพันธะ
สำหรับพันธะทั้งหลายที่
สร้างและทำลายในปฏิกิริยาของเรา
ลองเริ่มด้วยพันธะที่แตกกัน
เรามีพันธะเดี่ยวคาร์บอน-คาร์บอน
ซึ่งใช้ 835 กิโลจูลต่อโมล
และเรามีแค่ตัวเดียว
เรายังต้องแตกพันธะไฮโดรเจน-ไฮโดรเจน 2 ตัว
2 คูณ 436 กิโลจูลต่อโมล
ซึ่งก็คือเอนธาลปีพันธะของพันธะนั้น
นั่นคือพันธะทั้งหมดที่เราแตก
ทีนี้เราต้องบวกพลังงานทั้งหมดที่ปล่อย
เวลาเราสร้างพันธะใหม่
เรามีพันธะเดี่ยวคาร์บอน-คาร์บอนนี้
มันคือ 346 กิโลจูลต่อโมล และมันเป็นลบ
เพราะพลังงานถูกปล่อยออกมา

Czech: 
Poslední vazba je
vazba uhlík vodík,
která je také záporná
protože se energie uvolňuje.
A tyto máme čtyři, a každá
uvolní 413 kilojoulů na mol.
Tohle všechno
hodíme do kalkulačky,
abychom dostali náš výsledek.
Mně vyšlo, že delta H
pro tuto hydrogenační reakci
mezi propynem a plynným vodíkem
je -291 kilojoulů na mol.
Vidíme, že celkově tato
reakce energii uvolňuje,
protože delta H je negativní,
tedy je exotermická.
Takto tedy můžeme použít vazebné entalpie
k výpočtu reakční entalpie.

English: 
And then, the last bond is
the carbon hydrogen bond,
also negative because
the energy is released,
and we have four of them, and each of them
will release 413 kilojoules per mole.
So if we still all of
this into our calculator
to get our final answer,
what I got was that the
delta H of reaction for this,
for this hydrogenation reaction
between propine and hydrogen gas,
is -291 kilojoules per mole.
We can see that this overall
reaction releases energy,
because delta H is negative,
so it's exothermic.
And that's how you can use bond enthalpies
to calculate delta H of reaction.

Thai: 
แล้ว พันธะสุดท้ายคือพันธะคาร์บอน-ไฮโดรเจน
เป็นลบเช่นกัน เพราะพลังงานถูกปล่อยออกมา
เรามี 4 ตัว แต่ละตัว
จะปล่อย 413 กิโลจูลต่อโมล
ถ้าเราใส่ทั้งหมดนี้ลงในเครื่องคิดเลข
หาคำตอบสุดท้าย
สิ่งที่ผมได้คือเดลต้า H ของปฏิกิริยาสำหรับอันนี้
สำหรับปฏิกิริยา hydrogenation
ระหว่างโพรไพน์กับแก๊สไฮโดรเจน
เท่ากับลบ 291 กิโลจูลต่อโมล
เราเห็นได้ว่าปฏิกิริยาโดยรวมปล่อยพลังงาน
เพราะเดลต้า H เป็นลบ 
มันจึงเป็นการคายความร้อน
นั่นคือวิธีใช้เอนธาลปีพันธะ
เพื่อคำนวณเดลต้า H ของปฏิกิริยา

Bulgarian: 
И след това последната връзка
е въглерод-водород,
също със знак минус,
защото се освобождава енергия,
имаме четири такива връзки, 
всяка от които
освобождава 413 килоджаула за мол.
Ако въведем всичко това в
калкулатора,
получаваме крайния отговор.
Получих, че ΔН за тази реакция
на хидрогениране на пропин
с газообразен водород
е –291 килоджаула за мол.
Като цяло при реакцията
се отделя енергия,
защото ΔН е отрицателно,
така че това е екзотермична реакция.
Ето как може да се използва
енталпията на връзките,
за изчисляване на ΔН 
на химичните реакции.

Korean: 
그리고 이제 마지막 결합은 탄소-수소 결합입니다
에너지가 방출되므로 음수이겠고
그러한 결합 4개가 있으며, 그들 각각은
몰 당 413 킬로쥴을 방출할것입니다
그래서 최종값을 얻기위하여 이 모든것들을
계산기에 입력하면,
우리가 얻게 되는것은  이것에 대한 반응 엔탈피입니다
프로핀과 수소기체 사이에
수소첨가 반응을 위한 엔탈피는
몰 당 -291 킬로입니다
우리는 여기에서 이 반응은 에너지를 방출했음을 볼수 있습니다
왜냐하면 반응엔탈피가 음수이므로 그것은 발열을 합니다
그것이 바로 여러분이 반응엔탈피를 계산하기 위하여 결합엔탈피를
사용할수 있는 방법입니다
