I don't suppose many people are still following this course now, but in case anyone is reading this and doing the problem sets on the ocw website: the solutions posted for the problem set for Lecture 18 are either incorrect or misleading. In the decomposition of phosgene question, the question provides an equilibrium constant as K, implying you might have to calculate the partial pressures to solve the problem, but the solution just uses that K value as Kc, the equilibrium constant expressed in terms of molar concentrations. In equations with a change in the total number of moles from products to reactants, these two constants are not equal. So at the very least, keep in mind that the constant provided might be Kc. In the second question on the decomposition of nitrosyl bromide, the same K =/= Kc issue persists. But the new issue is that nitric oxide is specified as being in the solid phase for some reason (I'm not sure this is possible because the boiling point of NOBr is higher than for NO). Presumably it is a typo, but if it is meant to be treated as a solid just as a mathematical exercise, its activity should be 1, not [NO]. The solution provided is correct only if the K provided is used as Kc, and NO is considered to be in the gas phase.
The statement at 32:35 in incorrect. K>1 doesn't necessarily mean more products. Try to plug into this formula K=1.1 and see for yourself. (This is because we have twice more reactants than products here)
at 31:07 x has 2 solutions : 0.381 bar and 0.655 bar, why is 0.655 bar not discussed? partial pressure for N2O would be -0.310 bar (if x=0.655 bar),what does that mean?
I have important question to ask if anyone can guide me that :.In Iupac nomenclature "When numbering a cycloalkane with substituents, give the lowest number to the substituent that appears first in alphabetical order.But in some cases,the substituent with lowest alphabetical letter comes at higher locant while the substituent with higher alphabetical letter comes at lowest locant .so kindly explain what is the rule to follow here?
The class assignment analogy, at the start of the class introduces misconceptions into the concept of chemical equilibrium. Learning is much better, in the longer term, to explain with a scientific model! The real world is complex. We go about trying to understand and explain the real world with models. Totally remove homework assignments and personification, and the real world of chemical equilibrium continues unaffected!
![Blox Fruits Dragon Rework Update [Full Stream]](http://i.ytimg.com/vi/EqDAp8udhm0/mqdefault.jpg)
I really admire her commitment to her shirts!
I wish I was allowed to eat chinese food during lectures
no no no... please don't do that!
@@eren-sh1sq why not?
I don't suppose many people are still following this course now, but in case anyone is reading this and doing the problem sets on the ocw website: the solutions posted for the problem set for Lecture 18 are either incorrect or misleading. In the decomposition of phosgene question, the question provides an equilibrium constant as K, implying you might have to calculate the partial pressures to solve the problem, but the solution just uses that K value as Kc, the equilibrium constant expressed in terms of molar concentrations. In equations with a change in the total number of moles from products to reactants, these two constants are not equal. So at the very least, keep in mind that the constant provided might be Kc.
In the second question on the decomposition of nitrosyl bromide, the same K =/= Kc issue persists. But the new issue is that nitric oxide is specified as being in the solid phase for some reason (I'm not sure this is possible because the boiling point of NOBr is higher than for NO). Presumably it is a typo, but if it is meant to be treated as a solid just as a mathematical exercise, its activity should be 1, not [NO]. The solution provided is correct only if the K provided is used as Kc, and NO is considered to be in the gas phase.
The statement at 32:35 in incorrect. K>1 doesn't necessarily mean more products. Try to plug into this formula K=1.1 and see for yourself. (This is because we have twice more reactants than products here)
K value is already given in this question.
great class I could understand everything
i love the work u are doing pls do video on chemical equilibrum
The clicker time pressure is so real
and you feel it, even more, when you watch the video 2x faster
at 31:07 x has 2 solutions : 0.381 bar and 0.655 bar, why is 0.655 bar not discussed?
partial pressure for N2O would be -0.310 bar (if x=0.655 bar),what does that mean?
0.655 bar would be unrealistic because you don't have enough initial reactant. As you said, it would become negative measure which is impossible.
@@maxramirez8218 actually negative pressure exists, but only in liquids
How did you solve for x here?
@@tiburon181 quadratic formula
1-2x >0 so 1>2x and x
14:10 Why would the units always cancel? Since c + d might not = a + b, like in the example at 23:00, wouldn't the units there be bar^-2?
units would cancel inside bracket (Pc/Pref)^a is just some dimensionless quantity raised to some power. dimensional consistency is always there
I have important question to ask if anyone can guide me that :.In Iupac nomenclature
"When numbering a cycloalkane with substituents, give the lowest number to the substituent that appears first in alphabetical order.But in some cases,the substituent with lowest alphabetical letter comes at higher locant while the substituent with higher alphabetical letter comes at lowest locant .so kindly explain what is the rule to follow here?
The class assignment analogy, at the start of the class introduces misconceptions into the concept of chemical equilibrium. Learning is much better, in the longer term, to explain with a scientific model! The real world is complex. We go about trying to understand and explain the real world with models. Totally remove homework assignments and personification, and the real world of chemical equilibrium continues unaffected!
I enjoyed this lecture very much
1.55 was that guy eating in the lecture hall? Is that even allowed during lectures??
Yes. Sometimes students have many lectures back to back and don't have time to eat outside class.
I wish I was her student. She is so good at this and so gentle with her explanations.
What college is this??
@@chumadoshi6987 MIT
what is nit with the food is that what you wanna learn
Eating during class is allowed? it looks for me non equilibrium......
42:07 that small company was Toast and it is now worth $30 billion at its peak and has $1 billion in annual revenue, wow
3:25 hmm
😂😂 I wish I could travel in past ..reach there and told them about Covid 19. ..It will be a shocker 😂😂😂
I think MIT students can do whatever they want to do because they are extremely intelligent.
I love this
Thanks Mam
Great teacher. "No unit, this is very exciting" -> I know it's really boring please hang in there T_T
Thank you ....😇
i love dis
3:27 #2020 #COVID
understandable
Oh this is good!
They can eat during class 😳
perfeita
ياكلون وشذا ابغا ادرس هناك
13:30- Cameraman, good job! You found equations on her face by staring at her soo long! Or just attracted to her?
Next challenge is covid 19
Fractional reserve banking makes us all debt slaves!
How many paisas have seen this video 🤠 jaja
Pre covid 19!
She's funny.