Calorimetry Problems, Thermochemistry Practice, Specific Heat Capacity, Enthalpy Fusion, Chemistry
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- Опубліковано 17 гру 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...
Final Exams and Video Playlists:
www.video-tutor.net/
Full-Length Videos and Worksheets:
/ collections
Final Exams and Video Playlists: www.video-tutor.net/
Full-Length Videos & Worksheets: www.patreon.com/MathScienceTutor/collections
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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
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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????!!
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.
Very helpful 😊
perfect example for latent heat and phase change at : 19:44
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lovely. errors fixed.
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Almost numerical part has been
Covered and very much helpful to me, thank you sir.
Where did the enthalpy of reaction formula at 18:00 come from/what is it derived from?
THANK YOU!!!!!!
At 14:31 dint you have to use the total of g in the system the 260 plus the 2.6?
Starting of this vedio,I thought
In this vedio we're going to talk about. .......
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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?
Are the units in the last question joules or joules per minute?
THANK YOU
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!
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.