Calorimetry Problems, Thermochemistry Practice, Specific Heat Capacity, Enthalpy Fusion, Chemistry
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- Опубликовано: 17 дек 2016
- This chemistry video tutorial explains how to solve calorimetry problems in thermochemistry. It shows you how to calculate the quantity of heat transferred using specific heat capacity during a temperature change process and using the enthalpy of fusion and heat of vaporization during a phase change process. This video contains plenty of examples and practice problems.
First Law of Thermodynamics:
• First Law of Thermodyn...
Thermochemistry Equations:
• Thermochemistry Equati...
Internal Energy, Heat, and Work:
• Internal Energy, Heat,...
Thermochemical Equations:
• Thermochemical Equations
Specific Vs Molar Heat Capacity:
• What Is The Difference...
________________________________
Basic Calorimetry Problems:
• How To Solve Basic Cal...
Final Temperature Calorimetry Problems:
• Final Temperature Calo...
Latent Heat of Fusion & Vaporization:
• Latent Heat of Fusion ...
Coffee Cup Calorimeter:
• Coffee Cup Calorimeter...
More Calorimeter Problems:
• Bomb Calorimeter vs Co...
__________________________________
Specific Heat Capacity Problems:
• Specific Heat Capacity...
Hess Law Problems:
• Hess's Law Problems & ...
More Hess Law Problems:
• Hess Law Chemistry Pro...
Enthalpy of Formation & Heat Combustion:
• Enthalpy of Formation ...
Enthalpy Practice Problems:
• Enthalpy Change of Rea...
__________________________________
Speed of Light, Frequency, & Wavelength:
• Speed of Light, Freque...
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Carson k sig figs make it easier for scientists to calculate things in a hurry to get a good estimate
Sig figs is just the perpetuation of useless shit.
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Professor Organic Chemistry Tutor, this is a lengthy and awesome video/lecture in AP/General Chemistry on Calorimetry Problems. The Calorimetry problem selection are excellent from start to finish. This is an error free video/lecture on RUclips TV with the Organic Chemistry Tutor.
We'll have a summative test in general chemistry hours later, so this is a very big help, especially when these calculations and explanations are all left out by the teacher in the lecture yet included in the test. That teacher have high standards I tell you
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My teacher is typically good at teaching chem stuff, but for some reason I just can't understand this unit, even when she goes over everything. I tried asking her for extra help but she gave me a really vague answer for some reason and then just said I was getting too distracted (despite immediately coming up with actual times for other students who asked, including my friend who sits right next to me and is equally distracted). But besides that, thank you so much for this video (and entire channel). It always helps me whenever I don't know what to do.
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for the problem at 14:00 shouldnt the mass used be (2.6+260 grams) instead of 260
you would still divide by the moles of CaCl2
well this is much more helpful than my teacher's demonstration and notes of this. Thank you!
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that kJ/mol in the last problem caught me offguard
learned more by 1:23 than from watching my teacher's videos over and over for a half an hour. THANK YOU!
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Thanks. I'm still a bit confused but the onus is on my professor, who hasn't introduced any of these terms or formulas to us and just linked us to this video. It's pretty discouraging how lazy some teachers have become, not even providing the basic tools for students.
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19:47 BTW, the specific heat of ice is 2.1 j/g Celsius, and the specific heat of steam is 1.7 j/g Celsius. (Just in case of any confusion) Also, yeah, the sig figs here are VERY WRONG, but this video is a great basis to help you study. As long as you do your own rounding and calculations.
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do you take the mass of the solution or the mass of water when calculating Q(soln) cause in one of the vids you took the mass of the entire soln. Am confused now????!!
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for the question at 8:00 does it matter which one gets the negative sign because I can understand why Fe gets a negative since it is losing heat but I'm wondering if it would make a difference in the final answer, mathematically.
Ibrahim Malki he said that it does not matter. I tried it by putting the sign in any one of them and I got the same answer.
I have a good feeling you're going to save my chemistry grade this semester
Are the units in the last question joules or joules per minute?
Where did the enthalpy of reaction formula at 18:00 come from/what is it derived from?
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15:52 what does he mean by anytime the temperature of the solution goes up that tells you the reaction is endothermic, if the temperature of the solution went down the reaction would be endothermic? I'm so confused at this part please help!
Endothermic means that the reaction gained heat and so the temperature of the solution would increase.
Exothermic means that the reaction lost heat and so the temperature of the solution would decrease.
For you in two years ago. I think its his error he made. He supposed to say "by anytime the temperature of the solution goes up that tells you the reaction is EXOthermic, if the temperature of the solution went down the reaction would be endothermic"
Furthermore, If the temperature of the solution increase, the reaction must release energy so its exothermic in order to raise the temperature for the water, thus, the water absorbs heat which become endothermic for the water.
Very helpful 😊
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How can we calculate the enthalpy for different temperatures using heat capacity of each species? I am specifically looking for the reaction CO2 + H2 to give HCOOH.
very informative lecture dude
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At 14:31 dint you have to use the total of g in the system the 260 plus the 2.6?
I luv u organic chemist cx
At 15:51, I heard "so any time the temperature of the solution goes up that tells you the reaction was endothermic; if the temperature of the solution goes down the reaction would be endothermic." Did you mean exothermic for when the temperature of the solution goes down?
I hope that's what he meant! Otherwise, I'm thoroughly confused.
Here’s a helpful way I remember. Endothermic (Endo- en= enter) heat entering. And exothermic. Ex= exit. Heat leaving.
Jack Johannessen yes
no, he is right!! , whenever something reacts in Water if its endothermic( it absorbs Energy special case a salt in Water: the lattice Energy is higher than the Hydration energy) the Water has to give Energy (heat) to Reaction, so it will make the Water cold( Water gave heat , so Exothermic) the Reactant absorbed Energy so Endothermic!
Naku Chan ty furry
Hello! Its a great video and I learned a lot. Thank you! But I just want to clarify the last part. (1.33)(40.7)(1000)=54131J so the total Q would be Q=80,399J.
Hi Kai! I just want to make a correction to your point as this can confuse other students. So, The Tutor is actually correct. It is 54266.7 and not 54131.
The thing is you rounded off 1.333333 into 1.33. As you can observe, he calculated it straight without rounding off 1.33. No hate please.
In short,
(1.3333333)(40.7)(1000)=54266.7J
Hope it helps!
How you comeout the heat of vaporization ???thank you..🧡
Isn't the formula for the delta H is (-q/moles)?
lovely. errors fixed.
Can someone help me please? Some examples I saw in books used q= mc~T + C~T for bomb calorimeter. Which one should I use?
perfect example for latent heat and phase change at : 19:44
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