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Why do balloons get cold when they deflate?

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5

1

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When I deflate balloons by cutting one end and letting the air out, why does the surface of the balloon feel cooler?

Thanks,

thermodynamics

share|cite|improve this question

asked 8 hours ago

Shuheng ZhengShuheng Zheng

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add a comment | 

5

1

$begingroup$

When I deflate balloons by cutting one end and letting the air out, why does the surface of the balloon feel cooler?

Thanks,

thermodynamics

share|cite|improve this question

asked 8 hours ago

Shuheng ZhengShuheng Zheng

26822 silver badges1010 bronze badges

$endgroup$

add a comment | 

$begingroup$

When I deflate balloons by cutting one end and letting the air out, why does the surface of the balloon feel cooler?

Thanks,

thermodynamics

share|cite|improve this question

asked 8 hours ago

Shuheng ZhengShuheng Zheng

26822 silver badges1010 bronze badges

$endgroup$

share|cite|improve this question

asked 8 hours ago

Shuheng ZhengShuheng Zheng

26822 silver badges1010 bronze badges

share|cite|improve this question

asked 8 hours ago

Shuheng ZhengShuheng Zheng

26822 silver badges1010 bronze badges

asked 8 hours ago

Shuheng ZhengShuheng Zheng

26822 silver badges1010 bronze badges

asked 8 hours ago

Shuheng ZhengShuheng Zheng

26822 silver badges1010 bronze badges

1 Answer
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$begingroup$

A piece of rubber can act as a refrigerator of sorts, as follows:

If you take a piece of rubber and stretch it out, the molecular chains are pulled out in tension and the kinks in them get straightened out. they are now stiffer, and whatever frequency at which they were originally vibrating will go up slightly- and this means the rubber is now warmer by a tiny amount, as if it were a parcel of gas which you have compressed.

If you maintain the stretch while the heat leaves the rubber, eventually the rubber assumes the temperature of its surroundings- like the parcel of compressed gas would, if stored in a thermally conductive container under pressure.

Then, if you suddenly release the tension on the rubber band, its molecules relax back to their slack state and their vibrational frequency drops down a tiny bit- which means its temperature drops below ambient- just as if you released the pressure on that parcel of compressed gas and allowed it to expand.

This effect can be demonstrated with a rubber band, as follows: Hold the band with both hands and press it against your lip to sense its temperature. Now pull the band out tight with your hands and hold it there for 10 seconds. Then quickly bring your hands together so the rubber band goes slack and immediately press it against your lip again. You will detect that it is now cooler.

share|cite|improve this answer

answered 8 hours ago

niels nielsenniels nielsen

24.8k55 gold badges3333 silver badges6969 bronze badges

$endgroup$

• 
  
  
  

  
  

  
  
  
  
  
  

  
  $begingroup$
  That effect is very real and well documented. But how do we know for sure the air inside, which undergoes a quasi-isobaric expansion, does not drop also in temperature a bit?
  $endgroup$
  – Gert
  7 hours ago
  

  
  
  
  


• 
  
  
  

  
  

  
  
  
  
  
  

  
  $begingroup$
  Because its pressure remains almost constant as the balloon contracts. The air expansion occurs not in the body of the balloon itself, but in the neck of the balloon near its outlet.
  $endgroup$
  – niels nielsen
  6 hours ago
  

  
  
  
  


• 
  
  
  

  
  

  
  
  
  
  
  

  
  $begingroup$
  Yes, I believe you are correct. Ta
  $endgroup$
  – Gert
  4 hours ago
  

  
  
  
  

add a comment | 

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5

$begingroup$

A piece of rubber can act as a refrigerator of sorts, as follows:

If you take a piece of rubber and stretch it out, the molecular chains are pulled out in tension and the kinks in them get straightened out. they are now stiffer, and whatever frequency at which they were originally vibrating will go up slightly- and this means the rubber is now warmer by a tiny amount, as if it were a parcel of gas which you have compressed.

If you maintain the stretch while the heat leaves the rubber, eventually the rubber assumes the temperature of its surroundings- like the parcel of compressed gas would, if stored in a thermally conductive container under pressure.

Then, if you suddenly release the tension on the rubber band, its molecules relax back to their slack state and their vibrational frequency drops down a tiny bit- which means its temperature drops below ambient- just as if you released the pressure on that parcel of compressed gas and allowed it to expand.

This effect can be demonstrated with a rubber band, as follows: Hold the band with both hands and press it against your lip to sense its temperature. Now pull the band out tight with your hands and hold it there for 10 seconds. Then quickly bring your hands together so the rubber band goes slack and immediately press it against your lip again. You will detect that it is now cooler.

share|cite|improve this answer

answered 8 hours ago

niels nielsenniels nielsen

24.8k55 gold badges3333 silver badges6969 bronze badges

$endgroup$

• 
  
  
  

  
  

  
  
  
  
  
  

  
  $begingroup$
  That effect is very real and well documented. But how do we know for sure the air inside, which undergoes a quasi-isobaric expansion, does not drop also in temperature a bit?
  $endgroup$
  – Gert
  7 hours ago
  

  
  
  
  


• 
  
  
  

  
  

  
  
  
  
  
  

  
  $begingroup$
  Because its pressure remains almost constant as the balloon contracts. The air expansion occurs not in the body of the balloon itself, but in the neck of the balloon near its outlet.
  $endgroup$
  – niels nielsen
  6 hours ago
  

  
  
  
  


• 
  
  
  

  
  

  
  
  
  
  
  

  
  $begingroup$
  Yes, I believe you are correct. Ta
  $endgroup$
  – Gert
  4 hours ago
  

  
  
  
  

add a comment | 

5

$begingroup$

A piece of rubber can act as a refrigerator of sorts, as follows:

If you take a piece of rubber and stretch it out, the molecular chains are pulled out in tension and the kinks in them get straightened out. they are now stiffer, and whatever frequency at which they were originally vibrating will go up slightly- and this means the rubber is now warmer by a tiny amount, as if it were a parcel of gas which you have compressed.

If you maintain the stretch while the heat leaves the rubber, eventually the rubber assumes the temperature of its surroundings- like the parcel of compressed gas would, if stored in a thermally conductive container under pressure.

Then, if you suddenly release the tension on the rubber band, its molecules relax back to their slack state and their vibrational frequency drops down a tiny bit- which means its temperature drops below ambient- just as if you released the pressure on that parcel of compressed gas and allowed it to expand.

This effect can be demonstrated with a rubber band, as follows: Hold the band with both hands and press it against your lip to sense its temperature. Now pull the band out tight with your hands and hold it there for 10 seconds. Then quickly bring your hands together so the rubber band goes slack and immediately press it against your lip again. You will detect that it is now cooler.

share|cite|improve this answer

answered 8 hours ago

niels nielsenniels nielsen

24.8k55 gold badges3333 silver badges6969 bronze badges

$endgroup$

• 
  
  
  

  
  

  
  
  
  
  
  

  
  $begingroup$
  That effect is very real and well documented. But how do we know for sure the air inside, which undergoes a quasi-isobaric expansion, does not drop also in temperature a bit?
  $endgroup$
  – Gert
  7 hours ago
  

  
  
  
  


• 
  
  
  

  
  

  
  
  
  
  
  

  
  $begingroup$
  Because its pressure remains almost constant as the balloon contracts. The air expansion occurs not in the body of the balloon itself, but in the neck of the balloon near its outlet.
  $endgroup$
  – niels nielsen
  6 hours ago
  

  
  
  
  


• 
  
  
  

  
  

  
  
  
  
  
  

  
  $begingroup$
  Yes, I believe you are correct. Ta
  $endgroup$
  – Gert
  4 hours ago
  

  
  
  
  

add a comment | 

$begingroup$

A piece of rubber can act as a refrigerator of sorts, as follows:

If you take a piece of rubber and stretch it out, the molecular chains are pulled out in tension and the kinks in them get straightened out. they are now stiffer, and whatever frequency at which they were originally vibrating will go up slightly- and this means the rubber is now warmer by a tiny amount, as if it were a parcel of gas which you have compressed.

If you maintain the stretch while the heat leaves the rubber, eventually the rubber assumes the temperature of its surroundings- like the parcel of compressed gas would, if stored in a thermally conductive container under pressure.

Then, if you suddenly release the tension on the rubber band, its molecules relax back to their slack state and their vibrational frequency drops down a tiny bit- which means its temperature drops below ambient- just as if you released the pressure on that parcel of compressed gas and allowed it to expand.

This effect can be demonstrated with a rubber band, as follows: Hold the band with both hands and press it against your lip to sense its temperature. Now pull the band out tight with your hands and hold it there for 10 seconds. Then quickly bring your hands together so the rubber band goes slack and immediately press it against your lip again. You will detect that it is now cooler.

share|cite|improve this answer

answered 8 hours ago

niels nielsenniels nielsen

24.8k55 gold badges3333 silver badges6969 bronze badges

$endgroup$

share|cite|improve this answer

answered 8 hours ago

niels nielsenniels nielsen

24.8k55 gold badges3333 silver badges6969 bronze badges

answered 8 hours ago

niels nielsenniels nielsen

24.8k55 gold badges3333 silver badges6969 bronze badges

answered 8 hours ago

niels nielsenniels nielsen

24.8k55 gold badges3333 silver badges6969 bronze badges