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Is it possible to find dry ice crystals lying around the base in Antarctica?



The Next CEO of Stack OverflowPhysicality of claims regarding AC ice energy storage unitsDry Ice in Liquid StatesDoes a cooler, submerged in water, keep beer colder, longer?How can we describe or model the spread of ice during the freezing of the surface of a still lake?Is air in the refrigerator dry? how much?Frozen lake ice formationEnergy efficiency: better to heat hot tub constantly or twice a day for a longer period?What can I do to be invisible for the IR-camera on board of a police helicopter?Am I right about IR vision?Is physical entropy opposite to information entropy?










3












$begingroup$


Dry ice sublimates at -78.5°C, while the lowest temperature registered is about -89.2°C around the Vostok station in Antarctica. Imagine a person living on that station on that day (or night, since it was measured during the polar night).



If that person goes outside, would they find any dry ice crystals laying on the ground?










share|cite|improve this question









$endgroup$
















    3












    $begingroup$


    Dry ice sublimates at -78.5°C, while the lowest temperature registered is about -89.2°C around the Vostok station in Antarctica. Imagine a person living on that station on that day (or night, since it was measured during the polar night).



    If that person goes outside, would they find any dry ice crystals laying on the ground?










    share|cite|improve this question









    $endgroup$














      3












      3








      3





      $begingroup$


      Dry ice sublimates at -78.5°C, while the lowest temperature registered is about -89.2°C around the Vostok station in Antarctica. Imagine a person living on that station on that day (or night, since it was measured during the polar night).



      If that person goes outside, would they find any dry ice crystals laying on the ground?










      share|cite|improve this question









      $endgroup$




      Dry ice sublimates at -78.5°C, while the lowest temperature registered is about -89.2°C around the Vostok station in Antarctica. Imagine a person living on that station on that day (or night, since it was measured during the polar night).



      If that person goes outside, would they find any dry ice crystals laying on the ground?







      thermodynamics phase-transition weather






      share|cite|improve this question













      share|cite|improve this question











      share|cite|improve this question




      share|cite|improve this question










      asked Mar 18 at 15:43









      alexeykuzmin0alexeykuzmin0

      1184




      1184




















          1 Answer
          1






          active

          oldest

          votes


















          6












          $begingroup$

          The equilibrium vapor pressure of carbon dioxide at -80 C is about 1 bar. The partial pressure of carbon dioxide in air is about 0.0004 atm. This tells you that CO2 will not sublime from air at -80 C.






          share|cite|improve this answer











          $endgroup$












          • $begingroup$
            That's why I always make sure to bring a sealed box of carbon dioxide when I vacation in Antarctica.
            $endgroup$
            – JMac
            Mar 18 at 17:48






          • 1




            $begingroup$
            While this answer is completely correct, I feel obliged to point out that drawing comparisons between two values in different units (atm vs. bar) is Not A Best Practice, particularly when they're not related by a standard SI prefix.
            $endgroup$
            – Michael Seifert
            Mar 18 at 17:58











          • $begingroup$
            Oops. I meant for the first to be atm.
            $endgroup$
            – Chet Miller
            Mar 18 at 18:01










          • $begingroup$
            So if I was brewing beer (what else is there to do at Vostok?), and thus had a container of carbon dioxide, which naturally happens during brewing, that container could have developed CO2 crystals, while it slowly deflated.
            $endgroup$
            – Cort Ammon
            Mar 18 at 22:00










          • $begingroup$
            Yes, if the pressure of pure CO2 in the container is higher than the equilibrium vapor pressure of CO2 at the temperature of the CO2.
            $endgroup$
            – Chet Miller
            Mar 18 at 22:28











          Your Answer





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          1 Answer
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          active

          oldest

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          1 Answer
          1






          active

          oldest

          votes









          active

          oldest

          votes






          active

          oldest

          votes









          6












          $begingroup$

          The equilibrium vapor pressure of carbon dioxide at -80 C is about 1 bar. The partial pressure of carbon dioxide in air is about 0.0004 atm. This tells you that CO2 will not sublime from air at -80 C.






          share|cite|improve this answer











          $endgroup$












          • $begingroup$
            That's why I always make sure to bring a sealed box of carbon dioxide when I vacation in Antarctica.
            $endgroup$
            – JMac
            Mar 18 at 17:48






          • 1




            $begingroup$
            While this answer is completely correct, I feel obliged to point out that drawing comparisons between two values in different units (atm vs. bar) is Not A Best Practice, particularly when they're not related by a standard SI prefix.
            $endgroup$
            – Michael Seifert
            Mar 18 at 17:58











          • $begingroup$
            Oops. I meant for the first to be atm.
            $endgroup$
            – Chet Miller
            Mar 18 at 18:01










          • $begingroup$
            So if I was brewing beer (what else is there to do at Vostok?), and thus had a container of carbon dioxide, which naturally happens during brewing, that container could have developed CO2 crystals, while it slowly deflated.
            $endgroup$
            – Cort Ammon
            Mar 18 at 22:00










          • $begingroup$
            Yes, if the pressure of pure CO2 in the container is higher than the equilibrium vapor pressure of CO2 at the temperature of the CO2.
            $endgroup$
            – Chet Miller
            Mar 18 at 22:28















          6












          $begingroup$

          The equilibrium vapor pressure of carbon dioxide at -80 C is about 1 bar. The partial pressure of carbon dioxide in air is about 0.0004 atm. This tells you that CO2 will not sublime from air at -80 C.






          share|cite|improve this answer











          $endgroup$












          • $begingroup$
            That's why I always make sure to bring a sealed box of carbon dioxide when I vacation in Antarctica.
            $endgroup$
            – JMac
            Mar 18 at 17:48






          • 1




            $begingroup$
            While this answer is completely correct, I feel obliged to point out that drawing comparisons between two values in different units (atm vs. bar) is Not A Best Practice, particularly when they're not related by a standard SI prefix.
            $endgroup$
            – Michael Seifert
            Mar 18 at 17:58











          • $begingroup$
            Oops. I meant for the first to be atm.
            $endgroup$
            – Chet Miller
            Mar 18 at 18:01










          • $begingroup$
            So if I was brewing beer (what else is there to do at Vostok?), and thus had a container of carbon dioxide, which naturally happens during brewing, that container could have developed CO2 crystals, while it slowly deflated.
            $endgroup$
            – Cort Ammon
            Mar 18 at 22:00










          • $begingroup$
            Yes, if the pressure of pure CO2 in the container is higher than the equilibrium vapor pressure of CO2 at the temperature of the CO2.
            $endgroup$
            – Chet Miller
            Mar 18 at 22:28













          6












          6








          6





          $begingroup$

          The equilibrium vapor pressure of carbon dioxide at -80 C is about 1 bar. The partial pressure of carbon dioxide in air is about 0.0004 atm. This tells you that CO2 will not sublime from air at -80 C.






          share|cite|improve this answer











          $endgroup$



          The equilibrium vapor pressure of carbon dioxide at -80 C is about 1 bar. The partial pressure of carbon dioxide in air is about 0.0004 atm. This tells you that CO2 will not sublime from air at -80 C.







          share|cite|improve this answer














          share|cite|improve this answer



          share|cite|improve this answer








          edited Mar 18 at 17:15

























          answered Mar 18 at 16:02









          Chet MillerChet Miller

          15.9k2826




          15.9k2826











          • $begingroup$
            That's why I always make sure to bring a sealed box of carbon dioxide when I vacation in Antarctica.
            $endgroup$
            – JMac
            Mar 18 at 17:48






          • 1




            $begingroup$
            While this answer is completely correct, I feel obliged to point out that drawing comparisons between two values in different units (atm vs. bar) is Not A Best Practice, particularly when they're not related by a standard SI prefix.
            $endgroup$
            – Michael Seifert
            Mar 18 at 17:58











          • $begingroup$
            Oops. I meant for the first to be atm.
            $endgroup$
            – Chet Miller
            Mar 18 at 18:01










          • $begingroup$
            So if I was brewing beer (what else is there to do at Vostok?), and thus had a container of carbon dioxide, which naturally happens during brewing, that container could have developed CO2 crystals, while it slowly deflated.
            $endgroup$
            – Cort Ammon
            Mar 18 at 22:00










          • $begingroup$
            Yes, if the pressure of pure CO2 in the container is higher than the equilibrium vapor pressure of CO2 at the temperature of the CO2.
            $endgroup$
            – Chet Miller
            Mar 18 at 22:28
















          • $begingroup$
            That's why I always make sure to bring a sealed box of carbon dioxide when I vacation in Antarctica.
            $endgroup$
            – JMac
            Mar 18 at 17:48






          • 1




            $begingroup$
            While this answer is completely correct, I feel obliged to point out that drawing comparisons between two values in different units (atm vs. bar) is Not A Best Practice, particularly when they're not related by a standard SI prefix.
            $endgroup$
            – Michael Seifert
            Mar 18 at 17:58











          • $begingroup$
            Oops. I meant for the first to be atm.
            $endgroup$
            – Chet Miller
            Mar 18 at 18:01










          • $begingroup$
            So if I was brewing beer (what else is there to do at Vostok?), and thus had a container of carbon dioxide, which naturally happens during brewing, that container could have developed CO2 crystals, while it slowly deflated.
            $endgroup$
            – Cort Ammon
            Mar 18 at 22:00










          • $begingroup$
            Yes, if the pressure of pure CO2 in the container is higher than the equilibrium vapor pressure of CO2 at the temperature of the CO2.
            $endgroup$
            – Chet Miller
            Mar 18 at 22:28















          $begingroup$
          That's why I always make sure to bring a sealed box of carbon dioxide when I vacation in Antarctica.
          $endgroup$
          – JMac
          Mar 18 at 17:48




          $begingroup$
          That's why I always make sure to bring a sealed box of carbon dioxide when I vacation in Antarctica.
          $endgroup$
          – JMac
          Mar 18 at 17:48




          1




          1




          $begingroup$
          While this answer is completely correct, I feel obliged to point out that drawing comparisons between two values in different units (atm vs. bar) is Not A Best Practice, particularly when they're not related by a standard SI prefix.
          $endgroup$
          – Michael Seifert
          Mar 18 at 17:58





          $begingroup$
          While this answer is completely correct, I feel obliged to point out that drawing comparisons between two values in different units (atm vs. bar) is Not A Best Practice, particularly when they're not related by a standard SI prefix.
          $endgroup$
          – Michael Seifert
          Mar 18 at 17:58













          $begingroup$
          Oops. I meant for the first to be atm.
          $endgroup$
          – Chet Miller
          Mar 18 at 18:01




          $begingroup$
          Oops. I meant for the first to be atm.
          $endgroup$
          – Chet Miller
          Mar 18 at 18:01












          $begingroup$
          So if I was brewing beer (what else is there to do at Vostok?), and thus had a container of carbon dioxide, which naturally happens during brewing, that container could have developed CO2 crystals, while it slowly deflated.
          $endgroup$
          – Cort Ammon
          Mar 18 at 22:00




          $begingroup$
          So if I was brewing beer (what else is there to do at Vostok?), and thus had a container of carbon dioxide, which naturally happens during brewing, that container could have developed CO2 crystals, while it slowly deflated.
          $endgroup$
          – Cort Ammon
          Mar 18 at 22:00












          $begingroup$
          Yes, if the pressure of pure CO2 in the container is higher than the equilibrium vapor pressure of CO2 at the temperature of the CO2.
          $endgroup$
          – Chet Miller
          Mar 18 at 22:28




          $begingroup$
          Yes, if the pressure of pure CO2 in the container is higher than the equilibrium vapor pressure of CO2 at the temperature of the CO2.
          $endgroup$
          – Chet Miller
          Mar 18 at 22:28

















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