Heat Capacity, Specific Heat, and Calorimetry
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- เผยแพร่เมื่อ 24 พ.ย. 2015
- We can use coffee cups to do simple experiments to figure out how quickly different materials heat up and cool down. It's called calorimetry. Take a look!
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you are amazing
what the teacher do in 50 min
you did it in 5 min
I always wondered why it would take them 30 minutes to explain a concept which can be done in 2 minutes.
@@JihadAlAnsari because then they wouldn't have jobs lol
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indeed
@@JihadAlAnsari because they are teaching 20+ people who learn in different ways, they also need to go over multiple topics at a time. Imagine you have a 2 minute class and don’t pay attention for one minute (zone out) you’re done for!
"He knows lot about science stuffs, Professor David explains! Turuttu ! "
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It's dave*
@@DvolWOLF no it's chemistry Jesus
I love that too lol I'm always singing along 😂
How tf does that sound like "turuttu" to you ?
It's my 2nd semester of first-year university chemistry... and of course, Professor Dave saves me once again.
Same here and agreed 🥹
@@yunyung lmao same as well
Then why am I doing this in 10th grade. Not fair
Then why am I doing this in 10th grade. Not fair
@@riruruuu bcaz what that person is doing is a intro chem course, they refresh the basics first then dive into the harder stuff as they progress
At the beginning, it thought I would be really difficult, but you explained it well! I see that you omitted the cancelation of the negative signs of the metal q and the metal Delta temperature, that confused me at first but made me think a little harder (which was good!). Thank you again!
Hello guys,
just to help you guys out the equations is missing negative in the calculation. To end up with the Ans: 2.19 J/g °C i thought i would simplify for those that may need it.
Don't forget the metal is losing energy and the water or liquid is gaining energy 'joules' So :- Qmetal/metal DT " -850J /(4.82) (-80.5°C) = 2.190665189.
COOL WELL EXPLAINED VIDEO THOUGH.
hope this helped.
hello sir ! my self rishabh , i am from india. today fortunately i came to your channel. your style of teaching is fantastic it attracts me a lot . thanks for free education. you are making a great effort to make this world Literate wish you all the best. you cover the topics very earlier and effectivily it is very benificial for all
Same bro
Thanks Professor Dave for doing something in four minuets my professor couldn't do in forty minuets. Explain the material.
This really helped my understanding of this topic thank you!
Thank you Professor Dave!!!!!
Awesome video hit the nail right on the head
I love this man!
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The best part is your video is concise and useful . thanks
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You are very fantastic prof. Thank you for making this channel
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thank u very much really its clear more about calorimeter
THANK YOU FOR THIS!!!
Thankyou for the video on Heat Capacity, Specific Heat, and Calorimetry.-Alexis Kironde.
Such a wholesome comment written like an email
This is TH-cam you didint have to be that formal take a chill pill😂
Amei a explicação ❤🎉 muito obrigada! O Brasil te assiste!!
I know this video was a while ago but if you ever do remakes, putting everything in standard units would be awesome so it's consistent with college courses. Like kg, K, and all that.
The visuals you put in are so helpful, thanks! ;]
so u are a studend of thermodynamics?
Why is he using Celsius and not Kelvin? The equations I saw multply by Kelvin not Celsius. Won't you get a wrong result this way? Please help.
Dave, you are really good.Thank you very much.
It was a couple years I haven't learn about different of heat capacity or specific heat. Thanks for explaining us.
This dude is so amazing even the teacher all over the philippines LINKED his vids for me and my class mates to whatch
I would much prefer you use the equality of heat lost = heat gained. q(water) = -q(metal) Thus you can be consistent in the determination of delta T as final T - initial T. Your video is really nice for an introduction to the concept of calorimetry but may be confusing when instructors discuss exothermic changes which are given a negative q or delta H.
thank you professor Dave, for eplaining me calorimetry in simple words.
Liked and subscribed. Thank you professor Dave, this is dope
Very insightful helped me to understand that coffee cup experiment
Wow, I needed that visualization. 👀👌 This is good stuff.
I love you Professor Dave
I didn't do the comprehension I was to busy jamming to the sick beats
check out the song at the end of any clip in my organic chemistry practice problems series. that's the dopest beat of them all.
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@@ProfessorDaveExplains Why are you using Celsius and not Kelvin? The equations I saw multply by Kelvin not Celsius. Won't you get a wrong result this way? Please help.
I love your content so much but bro you your intro is the funniest thing ever it really made my day
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thank you brother, u help alot of fellow studs by ur lecs
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very nice explained sir
That's great explanation
THANK YOU !
Thank you sir
Bless this video
Awesome comprehension question!
thamks
Thanks Dave.
Τhank you very much for sharing!
I am watching you lectures to revise material which is needed in order to earn my master's degree.
The only thing that I would like to say is that since the volume of the water has two significant figures, the end result should have two significant figures too [2.2 J/(gr*°C)] (3:38).
Apropos, I couldn't find a metal that has this specific heat; could you reveal it to me?
sir, will you define heat capacity with some other lab activities??
lovely explaination
Great videos! Keep it up!
Very intelligently explains. Prof Dave is the best
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Thank you bro 🙏
i have long graduated and sometimes this very simple thing is not remembered (we cant remember everything right), so this video is an excellent video for a short revision.
Your videos r very useful but can u plz talk about thermal decompostion
Omg. Thank you! Im a chemistry major but this type of problem was so confusing to me. Thanks!
Zeima Rodriguez bruh i’m in 6th grade tryna figure this out😭
Nice lecture
Thank you so much !!
I am from Egypt , Really Thnx 💙
What is the initial value of metal temperature?
That last q helped me understand that I understood. Tnku
Thanks!!
Hello sir.. thanks for this video. Just wanna ask how to measure sp of soluble solids like sugar? pls reply thanks
Superb bro!!
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Thank you
Nice lecture sir
Helps alot
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I have another question is
Does material has high heat capacity means to faster speed in change of temperature , in the condition of provide same heat to different material?
For practical reasons, the change in water temperature is to be recorded in time. When the graphic peaks, that is the temperature change for the given equations. That is because the calorimeter change heat with the environment as well. Your thoughts?
My native language is Spanish but I study in Brazil so all my classes are in Portuguese and the only way that I found to understand this topic was theses videos in English hhahahahah, I love your videos
Really? kkkkkkk I'm from Brazil
Thanks
Yess
Hi Professor Dave
THANK YOU! Your videos are very helpful with my SAT Chemistry prep.
I have a question tho, how do you get delta T for the second equation of the metal?
the initial temperature of the metal is 115 so you have to use that!
@@ProfessorDaveExplains sir why we are taking the subtraction whether both are differently placed?
Hi@@ProfessorDaveExplains, I also have a question. Why are we subtracting from the initial temp for the delta T (change in temp) and not from the final temp (i.e. 34.5 C - 115 C)?
I have my examen in 1 hour and I so nervious, thanks for help me
Thank u sir
Hello prof. , im confused by the concept of this question which is contrast to my understanding, the solution explains that the q of the diamond is equal to the "-" q of the water (q[diamond]= - q[water]. Why did the water absorbed heat and has a negative value?
5. As a purity check for industrial diamonds, a 10.25-carat diamond (1 carat = 0.2000 g) is heated to 74.21 oC and immersed in 26.05 g of water in a calorimeter. The initial temperature of the water is 27.20 oC. If the specific heat of diamond is 0.519 J/g oC, what is the final temperature of the water?
Please prof, I have a question on the enthalpy as, If the elementary step A to B has a reaction enthalpy of XKJ and the activation energy of the reverse step B to A is YKJ, then the activation energy of the process A to B would be what?
More examples, please!
Thanks that helped alot
But did you assume that the metal started up at 25.5°C when the question doesn't mention it. I thought that when the starting temperature isn't mentioned we just take the standard which is 25. So my answer was slightly different, s≈1.958J/g°C
thanks,
thank you sir.l was not able to understand the concept clearly when l was taught at school.this video helped me tremendously....😂😂😂😂😁📣
Thanks .. Prof. DAVE
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Sir, how specific heat different from conductivity or with other mode of heat transfer....
Specific heat is not a means of heat transfer , it is the characteristic property of every substance and is different for all.
What's the difference between ''heat transfer'' and ''change in temperature''?
Good
hey professor dave, thanks a lot for the explanation
but I have a question though
in the example how could the initial temperature of the metal be 100c and the water is 25c
but the final temperature for both of them is 33.8c
shouldn't it be at 62.5c so both of them can be at thermal equilibrium?
are these just arbitrary numbers for the example or am I missing something??
the hot metal starts at the hot temperature, and it is placed into room temperature water. then the system equilibrates at an intermediate temperature, but these objects have totally different specific heats, the metal cools at a different rate than water heats, so the final temperature is not just the average of the temperatures, you have to do the math
oh I didn't know that my teacher just taught it to me like that in prep school or something :""
I appreciate the very quick response too! thanks a lot
Each of your videos first illuminates my mood and then your reference illuminates my concentration power.😇
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In the problem 4.82g of an unknown metal is heated to 115.0c and then placed in 35L of water at 28.7c,which then heats uptp 34.5c.What is the specific heat of the metal?
For the waterq=(4.186 j/g) (35g)(5.8c)
how or where did you get the 5.8cand for the Metal 850j =s(4.82g)(80.5c)
S=2.19 j/g cwhere or how to get 80.5c as these temperatures are not mentioned in the question and also when i multiply the specific heat and the temperature i dont get 2.19 j/g ci get 4.82*80.5=388.01
Please explain at your earliest convenience as iam in a dark dark place
Professor Dave, saves 😅
His face looks like ranveer Kapoor
These videos are very helpful. But just one suggestion, put them into an organized playlist of some sort so that people don't have to go around and search for the next topic
buddy all of my tutorials are immaculately organized into playlists! did you even think to check before commenting?
I didnt do this in chem 1 but i am now doing it in physics 1 non calc
sir wht we define heat capacity from celcias instedof kelvin
Specific Heat of Water is 4.186 J/gC for the comprehension part.
TheChosenOne thanks. i was going crazy as i was using 1 cal/g C and getting the wrong answer hahah
how does he get 4.186?
@@keylal3339 exactly i want to know as well
shouldn't be the q in computing for the specific heat capacity of metal be negative? Heat was released by the metal isn't it?
2:31 Is the specificheat before or after the water absorbs the heat from the rock?
I like how simply Professor Dave explains science stuff
Mathematically you can use grams, but the SI unit of mass is the kg. So specific heat capacity is often quoted in joules per kg per degree C. (Wouldn't it be nice if the SI unit was gram)
Tq prof.Dave!!!!! It was very useful!!!!
Why is 66.5 degrees not a negative change in temperature at 3:05? The temperature of the metal decreases to reach the final temperature, right?
Sir i now know a lot from your teaching .can you the difference between melting point and boiling point
One marks the transition from solid to liquid, the other from liquid to gas.