How To: Find Limiting Reagent (Easy steps w/practice problem)
HTML-код
- Опубликовано: 30 сен 2024
- A video made by a student, for a student. Showing how to find the limiting reagent of a reaction.
Kansas University. Rock Chalk Jayhawk, KU!!!!!!!!!
IGNORE:
Stoichiometry. Biology. Chemistry. How to work practice problem. How to convert. moles to grams
. grams to moles. how to. doing chemistry practice problems. science. how. to. do. science. intro college chemistry level. problems. molecular weight. neutrality. acid. base. calculations. molar. mole. molar unit. grams. weight. chemical. formula. empirical. molecular. science equations. easy problems worked. made easier. made easy. density. mass. volume. how to find them. finding density. finding volume. finding mass. how to find molarity. how to find molecular weight of anything! all chemistry equations keywords
![NOSFERATU - Official Trailer [HD] - Only In Theaters December 25](http://i.ytimg.com/vi/nulvWqYUM8k/mqdefault.jpg)
How did you get the 1.75 moles you never explained that part
you're basically, instead of saying, for every 4 moles of NH3 you need 7 Moles of O2. your dividing 4 by 4 to make it 1 and whatever you do to one side of the equation you have to do the other, so you divide 7 by 4 aswell to get 1.75. therefore for every 1 mole of NH3 you will need 1.75 Moles of O2
@@sciencemadeeasier7100 but why by 4? why not by 7?
@@ej4458 I think it's because if you divide by 7, you would get a recurring decimal if you divided by 7, thus making your life harder for no reason
@@ej4458 @Bakhshi Zulfiqar Manzur you are dividing 7 by 4 so that you can find out how many moles of O2 reacts with 1 mole of NH3
@blip trip in math generally, you want to get to 1 as your least common factor, so to get 7:4 is the same as 1.75:1 since 7/4=1.75, and 4/4=1. Hope this helps! :D
u saved my ass bro thanks
i gotchu bro
huntsman knife....xd
this teflon from h1z1?
I'm a senior in engineering and i needed to review how to do this stuff. You made this video short, straightforward, and easy to understand. thank you
Thank you very much Alex, glad I could be of assistance.Good luck, finish strong. I have a good friend in his junior year now..shit looks nasty
I have watched at LEAST a dozen L.R. vids, trying to understand this (including all the best known Chem people on here) and this is THE ONLY ONE I GET. Thank god I get it now!
+Alexandra “North Star” Wilson Thank you so much! Thats exactly what I thought before I made my chemistry tutorials.. I couldn't find a good video online to teach me so I made my own videos to basically teach myself but others find them very useful :) Glad I could be of assistance and thank you for the compliment!
Yeah
your marker works perfectly well lol
Exam tomorrow wish me luck!!!
Mine is today and i woke up 5 hours early to study 🤣
I got one tomorrow
mine is tomorrow
@@ammaarquraishi2398 sammee
Tomato Llama mine is tomorrow 😂😂
You're telling me that my university professor took an entire class to explain this, while I learned it in 3 minutes?
yes
Your doing this in uni??
@@te1327 lol i was wondering the same cuz i m doing this in junior year of high school
@@abhya12 yeah in the UK we did this in year 10 which I believe is freshman year in the us (14-15)
@@te1327 sophomore it is, and yea same, we did it in year 10 too!
exams tomorrow wish me luck lol, and yes this video helped thanks
He got that 1.75 by dividing the no of moles by the stoichometry of the reaction. Like 8/7
how do u get 1.75??
+Akash Kumar 4 moles of NH3 require 7 moles 02. Therefore, Each mole of NH3 requires 7/4 of a mole of O2. Understand?
+ScienceMade Easier no
Onalenna Moeti
So basically it's,
So 4/4 = 1
So 7/4 = 1.75
Onalenna Moeti you have 4 mol NH3 and 7 mol O2. So when you take one mol NH3, you divided the original 4 mol NH3 by 4. (4/4 =1) So to keep the ratio the same, you also need to divide the original 7 mol O2 by 4 also (7/4 =1.75) . So that’s where the 7/4 mol O2 comes from.
you're basically, instead of saying, for every 4 moles of NH3 you need 7 Moles of O2. your dividing 4 by 4 to make it 1 and whatever you do to one side of the equation you have to do the other, so you divide 7 by 4 aswell to get 1.75. therefore for every 1 mole of NH3 you will need 1.75 Moles of O2
1. Quick vdo
2. Simply understand.
3. Tysm
😄ok bie.
at 1:45 - end I don't understand could you explain that more
Where did the 1.75 come from?
What if it moles instead of grams like 43.9g
Why not 2,58/4 and 8/7 instead of the 1,75 thing?
Simple, straight to the point videos like this are hard to find these days on here, thank you.
thanks a ton #2019
what if the coefficient for both reactants is just 1?
same
Divide the grams given by the molar mass for both compounds and which ever one has less is the LR
This is the most helpful video I’ve found so far, thank you so much
Nice dude👍
Thank you
1:57 where did 1.75 come from?
Ratio of the coefficients on the reactant side of the equation. 4/7=1.75
All other videos made me confused!......but this is too helpful.............
Amazing!! With the easiest explanation possible.Thanks a lot.
This video saved me and I'm doing AS chemistry! My teacher is rubbish but you explained it very well!! Thanks so much!
Amina Ahsan bruh I'm doing this at igcse lmao
Amina Ahsan same my chem teacher sucks 😂
@Jia Dittman that is the molecular mass of NH3.
Molecular mass of N= 14
Molecular mass of 1 hydrogen = 1.
There are 3 hydrogen out there are so there are a total of 3 .
Now 14+3=17
why do you need 1.75 moles???
+Neza G The ratio of 4NH3 + 7O2 is 4:7 (leading coefficients) but he just reduced it by doing 7 divided by 4 which equals 1.75
+Blueberry OaC can't you just leave it as it is though without doing that??
midterm tomorrow, yet another life saved by this
Glad to be of assistance, Diego
Ugh. 15 in AP Chemistry - You saved me from failing a midterm. Tysm
Thanks this video is helpful
I've BEEEEN struggling with this! Great video, thanks a million :)
Nice explanation brother 😉
last sec chem bang out
Skipped a year, needed this man. Thanks!
Wow thank u so much for summarising two classes into 3 min
wait, how is it 2.58 x 1.75, isn't is supposed to be 258? im kinda confuse
Thanku very much sir..
Cheerssss got my chemistry exam in one hour!
SAME
same lol
Where did the dude get 1.75. He can't teach lol
Bro i really like the way you write 6..BTW very well explanation..
Where did you get 17 from'?????
you're not very thorough. you'd make a good college professor
This was insanely helpful, thank you!!!
This is Perfect!
Can you tell me please how the NH3 is the limiting reagent?
Great video! I looked at 3-4 other sources and your explanation was by far the best. Keep up the good work!
What if the limiting turned out to be the O2 how would it turned out to be
Thankyou so much! This video really helped
@Lizzy Reese they make really confusing things in the text but conversion of moles is really easy , all you have to remember is
No. Of moles = given mass / molecular mass or atomic mass of compound
you r osm thankyu 😊😊
This confused me , my teacher taught it different
i have a chemistry test in less than 5 hours and this saved my life tytyty
Can we use this method in all limiting re agent problem
bro I think u have to divide mass of oxygen by its Ar value which I's 16 ..
this is was so helpful thanks so much brother
thanks
Where did u get 17 for NH3 and 32 for O2?
Thanks man... Really helped Me.
How do you get 17 when dividing I keep getting 16
That's not the balanced equation though
Sir finding molecular weight is difficult for many complex compounds (unknown atomic number in periodic table)please tell any way without involving in moles🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻🙏🏻
Terimo kaseh banyok
Where did you get 1.75 from?
kiefer weber that's what I was wondering
He basically divided the NH3 and O2 by the smallest coefficient, which was 4. So 4 NH3 / 4 = 1 and 7 O2 / 4 = 1.75.
@T. Tib do you have to always divide with the least number?
Just divide no of molss of o2 by nh3 simple
kiefer weber I don't know either
He divided 7/2 to get the 1.75 but why?
Exam today wish me luck
Awesome
we have to divide no of moles by co efficent
good idea
How'd you know whether to multiply 1.75 by 2.57moles rather than 8.06 moles of oxygen
What are you doing on my Seneca?
why you multiply 2.58 moles * 1.75 what is this 1.75 ?
Mole ratio,
Since there are 7 moles of O2 per 4 moles of NH3, you divide 7/3 =1.75
Then you take that number and multiply it by 2.58 to get excess agent.
You just saved my ass thx so much
How the 1.75 is came
THIS VIDEO WAS EXTREMELY HELPFUL. You literally saved me bro!!!
thank you thank you thank you
I really needed this, thanks a lot helped me very much!
Anybody here in syiem lol
How did you get the 43.4
Woooooowwwwwwwww thank youuu
Why do you do moles of NH3 x moles of O2 needed? I thought you did 8.06/2.58 to get the ratio then compare it to the ratio from the formula to see which one's in excess
My doubt clear
bro i looovvveeee yooouuu
u dont explain clearly how how u know 1.7moles of O2 needed
wait what if it's 1 to 1
Thankyou guy💝💝
you should do stoichiometry
Absolutely fantastic. Had to watch it twice, though, but the result is what matters! Cheers, ScienceMade Easier!
edit: who disliked this video?!
Literally the only video i have found on youtube that explains it so simple and easy to understand. The rest is just a bunch of confusing bullshit
Thank you so much
what a lifesaver
Why are u multiplying only NH3 moles ? Please elaborate!
Thanks bro!
1:23 yo your molar mass is 2 significant figures so you moles should be 2 significant figures since 2 is the fewest amount of sig figs used ( for accuracy). but it is not you used more when writing the amount of moles.
why did you multiply 2.58 with 1.75? like how do you know what to do by multiplying
U r osm....thank u so much... Ur video Help me alot 💫💫☺☺☺
thank you!
thank you!
Audio is low
Ive been stressing all week because my teacher sucks at teaching and I have to resort to RUclips as a replacement for my teacher. I finally found a video that made finding limiting reactants simple that also showed how you find the actual mole ratios. Thank you!
should use dimensional analysis. this way is just confusing.
Thanks for video. This really helps!!! Please make more.