Calorimetry of a Cheeto - Determine the Calories per gram

[@mujibrahman3212]

“The Cheeto gosh darn it is gonna burn“ 7:37

[@Youngkhan529]

You should’ve write everything on the paper cuz This my assignment and I don’t know what to do man my head hurts now

[@czylbauer5812]

hate chem

[@babyyangie1594]

Sis do you have the answers 😭

[@czylbauer5812]

@@babyyangie1594 no boo

[@carolinafigueroa9705]

Sameeee!

[@santibeanieboi3577]

anyone got the answers?

[@tokofeigy]

when the cheeto got burnt it look like the old worm women thing in SpongeBob

[@shirfarkash3904]

When calculating the Cal/serving (to eventually find the percent error) will you subtract to mass of the burnt cheeto from the original mass? (1.67-0.19). I am not sure how to use that piece of information. When I subtract I arrive at 56% percent error and when I don't I arrive at 62%.

[@MrGrodskiChemistry]

Subtracting the burnt cheeto from the remaining burnt one just ensures that you only measures the mass of the cheeto that was consumed by the combustion which is the fat or oils. The large negative percent error is expected as the their will be heat lost to the environment.

[@User4o3p93ghvjkaehvji]

@@MrGrodskiChemistry I'll try it too. Mine is 40% 😳

[@shirfarkash3904]

@@MrGrodskiChemistry Thank you!

[@TheSpencomatic]

thank, much appreciated

[@amandacrosson3554]

Great video! We did this in my class. My percent error was way off, but after watching this I think it was because I looked at overall calories instead of calories from fat per gram. So, this only applies to calories from fat and not overall calories? I had to google the calories for fat because my nutritional labels only had overall calories and not calories from fat listed.

[@jackymedrano8717]

When determining the % error, a 56% error was calculated. That means the measured heat was more than half missing right .where the missing energy went?

[@MrGrodskiChemistry]

Very good! The missing heat dispersed into the environment. Heat loss from calorimeter experiments are their greatest error.

[@User4o3p93ghvjkaehvji]

😳 yehay I have one who tested too. Mine 40% . 😳

[@User4o3p93ghvjkaehvji]

@@MrGrodskiChemistry Is my value okay? 😳

[@LexGlad]

How is this in any way more accurate than calculating the chemical energy density of the nutrients. This is not how food works in the body, so maybe all the food labels are, at best, physics inaccurate. ATP conversion has well-known formulas.

[@amandacrosson3554]

Also, what would the percent error typically be on this lab? Like a good range?

[@MrGrodskiChemistry]

It will be high. I really try to drive home the point that heat will be lost to the environment. We should embrace the errors or limitations as they point to a greater understanding of the process.

[@mckennablack1000]

For my percent error I got 73.83 but this can't be correct because you said it supposed to be negative correct?

[@glarycelishernandezpabon507]

Percent error should be in absolute value. Meaning you shouldn’t get a negative percent.

[@sparklingwater2471]

that scale been through more AP classes than I can imagine 9:30

[@MrGrodskiChemistry]

It is still going strong!

[@leofu5015]

Hi, what is the mass of the AI can and the glass flask?

[@jer1cka]

Hello, I had a question on how to caculate the Kcals of heat. Is it possible you help explain how to solve it step by step ?

[@MrGrodskiChemistry]

First you need to calculate the calories of heat needed to raise the temperature of the water from its initial temperature to its higher final temperature using q = mc (change) T. The calories( q) of heat needed to make the water increase its temperature equals the mass of the water times the specific heat of the water (1 cal per gram Celsius) times the temperature change of the water. This calculated calories of heat needed to raise the water temperature is the same calories that the Cheeto released (assuming no loss of heat ). Convert this calorie value in Kcals and divide by the Cheeto mass that was missing (or burned away) to obtain Kcal per gram. A kilocalorie is the same as a nutritional Calorie.

[@irinahernandez4885]

Hi! I was wondering if you could explain how to calculate the Kcal's of heat, I got a really high number and not sure if its correct. My teacher also never actually explains or teaches so im kinda lost.

[@MrGrodskiChemistry]

First you need to calculate the calories of heat needed to raise the temperature of the water from its initial temperature to its higher final temperature using q = mc (change) T. The calories( q) of heat needed to make the water increase its temperature equals the mass of the water times the specific heat of the water (1 cal per gram Celsius) times the temperature change of the water. This calculated calories of heat needed to raise the water temperature is the same calories that the Cheeto released (assuming no loss of heat ). Convert this calorie value in Kcals and divide by the Cheeto mass that was missing (or burned away) to obtain Kcal per gram. A kilocalorie is the same as a nutritional Calorie.

[@babyyangie1594]

Did you figure it out sis ? And also did you figure out the percent error ?😭

[@milktxtea]

Hi does the mass of the water change after being heated, or is it still 100 grams? Also, my teacher is asking for the mass of the aluminum can and the glass flask before and after heating, but I don't know where to find this information.

[@MrGrodskiChemistry]

In a closed system the mass of the water would not change but in an open system like the lab in video could you possibly think of way the mass of the water would change? The mass of the can and glass flask are not provided,

[@User4o3p93ghvjkaehvji]

My percent error is high. Only 40‰ of calories of cheetos I calculated 😳. What happened?

[@MrGrodskiChemistry]

Did all the heat released by the Cheeto get absorbed by the water?

[@User4o3p93ghvjkaehvji]

@@MrGrodskiChemistry I burned it using flat can with holes. 13 g Cheetos. I used matches side by side for flame then it burns continuesly. I used old cooker for stand. When I placed my tank with thermometer, it almost close my flat can with holes so I think the flames are near. My flat can is 1.5 in height.

[@User4o3p93ghvjkaehvji]

@@MrGrodskiChemistry i uses old tech. I measure grams using ruler 😄

[@User4o3p93ghvjkaehvji]

@@MrGrodskiChemistry 🙏

[@User4o3p93ghvjkaehvji]

@@MrGrodskiChemistry maybe some absorbed by air convection . Maybe some flames are small and tank absorbed smoke heat 🙏. How much percent did you get? 🙏.

[@TheSpencomatic]

do you have a copy of the instructions to share?

[@MrGrodskiChemistry]

I just placed the link to the lab in the description. Good Luck.

[@igotapochahontas]

this is a very well done video. exactly what I was looking for. you may consider changing the title, it gave me low expectations for the content that I'm happy to report being wrong about.

[@phil5514]

wowwww he burned a cheeto. ground breakinggggg

[@ilifir136]

Man clean your scale thats nasty

[@jonathontrei3538]

you should remake this video and stop jumping forward and backwards in your explanation. I've never in my life had trouble following an explanation in a lab as I did in this video.

[@LordDiabetus]

Would be a much better video if stuff wasn't repeated so much. We should all already know going in that 100 ml of water is 100g. Even if not, once is enough, you don't have to repeat that six times, it makes it an interminable watch.