Why is a liquid nitrogen canister not cold on the outside when inside the temp of the sealed liquid is -320F?












1












$begingroup$


...or IS the inside temperature ambient temperature? Surely the insulation of the container is not sufficient to seal in that cold? I.e. if you had an unsealed bowl of liquid nitrogen with the same thickness of the sealed canister surely the temperature of that bowl on the outside would be cold?






thermodynamics fluid-dynamics condensed-matter temperature low-temperature-physics







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  • 3




    $begingroup$
    Why is my freezer room temperature on the outside and -18 Celsius inside?
    $endgroup$
    – my2cts
    5 hours ago
















1












$begingroup$


...or IS the inside temperature ambient temperature? Surely the insulation of the container is not sufficient to seal in that cold? I.e. if you had an unsealed bowl of liquid nitrogen with the same thickness of the sealed canister surely the temperature of that bowl on the outside would be cold?






thermodynamics fluid-dynamics condensed-matter temperature low-temperature-physics







share|cite|improve this question









New contributor




Andrew Strever is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.







$endgroup$








  • 3




    $begingroup$
    Why is my freezer room temperature on the outside and -18 Celsius inside?
    $endgroup$
    – my2cts
    5 hours ago














1












1








1





$begingroup$


...or IS the inside temperature ambient temperature? Surely the insulation of the container is not sufficient to seal in that cold? I.e. if you had an unsealed bowl of liquid nitrogen with the same thickness of the sealed canister surely the temperature of that bowl on the outside would be cold?






thermodynamics fluid-dynamics condensed-matter temperature low-temperature-physics







share|cite|improve this question









New contributor




Andrew Strever is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.







$endgroup$




...or IS the inside temperature ambient temperature? Surely the insulation of the container is not sufficient to seal in that cold? I.e. if you had an unsealed bowl of liquid nitrogen with the same thickness of the sealed canister surely the temperature of that bowl on the outside would be cold?






thermodynamics fluid-dynamics condensed-matter temperature low-temperature-physics




thermodynamics fluid-dynamics condensed-matter temperature low-temperature-physics






share|cite|improve this question









New contributor




Andrew Strever is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.











share|cite|improve this question









New contributor




Andrew Strever is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.









share|cite|improve this question




share|cite|improve this question








edited 4 hours ago









Qmechanic♦

104k121881195




104k121881195






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asked 5 hours ago









Andrew StreverAndrew Strever

61




61




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Andrew Strever is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
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New contributor





Andrew Strever is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.






Andrew Strever is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.








  • 3




    $begingroup$
    Why is my freezer room temperature on the outside and -18 Celsius inside?
    $endgroup$
    – my2cts
    5 hours ago














  • 3




    $begingroup$
    Why is my freezer room temperature on the outside and -18 Celsius inside?
    $endgroup$
    – my2cts
    5 hours ago








3




3




$begingroup$
Why is my freezer room temperature on the outside and -18 Celsius inside?
$endgroup$
– my2cts
5 hours ago




$begingroup$
Why is my freezer room temperature on the outside and -18 Celsius inside?
$endgroup$
– my2cts
5 hours ago










2 Answers
2






active

oldest

votes


















7












$begingroup$

Liquid nitrogen is usually kept in a Dewar flask. This flask protects the liquid nitrogen against all three kinds of heat transfer, as follows:



1) Convective heat transfer is largely eliminated because there is a hollow space inside the flask, between the outer and inner walls (or "containers") of the flask. This hollow space often is vacuumed out to eliminate heat convection via air.



2) Conductive heat transfer is largely eliminated because the inner container only touches the outer container at the very top of the flask, so any heat conduction from the mouth of the flask must travel the maximum path length to get to the liquid nitrogen. Accordingly, the rate of conductive heat transfer is minimized by doing this.



3) Radiative heat transfer is largely eliminated by putting a mirror finish on the outside of the inner container.



All of these techniques mean that heat transfer from the outside of the Dewar flask to the inside of the flask is minimized, and as a consequence, the outside of the flask does not feel cold.



For more info, see the following:



https://en.wikipedia.org/wiki/Vacuum_flask



https://en.wikipedia.org/wiki/Cryogenic_storage_dewar






share|cite|improve this answer









$endgroup$





















    1












    $begingroup$

    Gas molecules have higher energy than a molecule that is part of a liquid or solid. Their higher kinetic energy allows them to move freely and bounce off other molecules and atoms, giving them their gaseous properties.



    When a gas is compressed, it forces these high energy particles to get closer together. As they get closer, they aren't able to move as freely. This kinetic energy must be preserved, and is given off in the form of heat to the surrounding container of the gas. Eventually, as pressure increases, these particles will condense together to form a liquid.



    When depressurized, as the liquid converts back to a gas, it will absorb the same amount of heat energy that it expelled when compressed. The heat energy in the container will be taken back by the expanding gas, making the container cool down.



    As for your question, the temperature of the liquid is ambient but at a very high pressure. Having an unsealed bowl of liquid nitrogen would not last long, and would get very cold as the liquid turned back into a gas.



    It has less to do with the static state of the liquid and more to do with the process of going from liquid to gas or vice versa.



    Did this help?






    share|cite|improve this answer









    $endgroup$













    • $begingroup$
      It did help thank you! My presumption was the temperature of liquid gas was constant in that state, so the gas would remain at -320F (nitrogen for example) while in liquid form - including inside a sealer canister/bottle etc. So: the temp of the gas (in liquid form) is only due to the process of the pressure decrease (?) I am just amazed at how quickly it happens. If you had a gallon of liquid nitrogen in a sealed canister at ambient temperature and poured it out into a gallon bucket it would immediately become -320F even in the middle due to the heat energy expelled. (?) thx!!
      $endgroup$
      – Andrew Strever
      1 hour ago










    • $begingroup$
      @AndrewStrever, I think you are drawing the wrong conclusions. Liquid nitrogen cannot exist at ambient temperature, as this is far above its critical temperature. Also, the temperature of a liquid and its vapor inside a sealed container depends on the pressure. As the pressure increases due to evaporation that occurs as a result of heating, the temperature increases also. In a pressurized container of liquid nitrogen, as heat "seeps" into the container, the temperature and pressure increase.
      $endgroup$
      – David White
      41 mins ago












    • $begingroup$
      CuriousOne, your posted answer did not answer the question that the OP asked.
      $endgroup$
      – David White
      37 mins ago











    Your Answer





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    2 Answers
    2






    active

    oldest

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    2 Answers
    2






    active

    oldest

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    active

    oldest

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    active

    oldest

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    7












    $begingroup$

    Liquid nitrogen is usually kept in a Dewar flask. This flask protects the liquid nitrogen against all three kinds of heat transfer, as follows:



    1) Convective heat transfer is largely eliminated because there is a hollow space inside the flask, between the outer and inner walls (or "containers") of the flask. This hollow space often is vacuumed out to eliminate heat convection via air.



    2) Conductive heat transfer is largely eliminated because the inner container only touches the outer container at the very top of the flask, so any heat conduction from the mouth of the flask must travel the maximum path length to get to the liquid nitrogen. Accordingly, the rate of conductive heat transfer is minimized by doing this.



    3) Radiative heat transfer is largely eliminated by putting a mirror finish on the outside of the inner container.



    All of these techniques mean that heat transfer from the outside of the Dewar flask to the inside of the flask is minimized, and as a consequence, the outside of the flask does not feel cold.



    For more info, see the following:



    https://en.wikipedia.org/wiki/Vacuum_flask



    https://en.wikipedia.org/wiki/Cryogenic_storage_dewar






    share|cite|improve this answer









    $endgroup$


















      7












      $begingroup$

      Liquid nitrogen is usually kept in a Dewar flask. This flask protects the liquid nitrogen against all three kinds of heat transfer, as follows:



      1) Convective heat transfer is largely eliminated because there is a hollow space inside the flask, between the outer and inner walls (or "containers") of the flask. This hollow space often is vacuumed out to eliminate heat convection via air.



      2) Conductive heat transfer is largely eliminated because the inner container only touches the outer container at the very top of the flask, so any heat conduction from the mouth of the flask must travel the maximum path length to get to the liquid nitrogen. Accordingly, the rate of conductive heat transfer is minimized by doing this.



      3) Radiative heat transfer is largely eliminated by putting a mirror finish on the outside of the inner container.



      All of these techniques mean that heat transfer from the outside of the Dewar flask to the inside of the flask is minimized, and as a consequence, the outside of the flask does not feel cold.



      For more info, see the following:



      https://en.wikipedia.org/wiki/Vacuum_flask



      https://en.wikipedia.org/wiki/Cryogenic_storage_dewar






      share|cite|improve this answer









      $endgroup$
















        7












        7








        7





        $begingroup$

        Liquid nitrogen is usually kept in a Dewar flask. This flask protects the liquid nitrogen against all three kinds of heat transfer, as follows:



        1) Convective heat transfer is largely eliminated because there is a hollow space inside the flask, between the outer and inner walls (or "containers") of the flask. This hollow space often is vacuumed out to eliminate heat convection via air.



        2) Conductive heat transfer is largely eliminated because the inner container only touches the outer container at the very top of the flask, so any heat conduction from the mouth of the flask must travel the maximum path length to get to the liquid nitrogen. Accordingly, the rate of conductive heat transfer is minimized by doing this.



        3) Radiative heat transfer is largely eliminated by putting a mirror finish on the outside of the inner container.



        All of these techniques mean that heat transfer from the outside of the Dewar flask to the inside of the flask is minimized, and as a consequence, the outside of the flask does not feel cold.



        For more info, see the following:



        https://en.wikipedia.org/wiki/Vacuum_flask



        https://en.wikipedia.org/wiki/Cryogenic_storage_dewar






        share|cite|improve this answer









        $endgroup$



        Liquid nitrogen is usually kept in a Dewar flask. This flask protects the liquid nitrogen against all three kinds of heat transfer, as follows:



        1) Convective heat transfer is largely eliminated because there is a hollow space inside the flask, between the outer and inner walls (or "containers") of the flask. This hollow space often is vacuumed out to eliminate heat convection via air.



        2) Conductive heat transfer is largely eliminated because the inner container only touches the outer container at the very top of the flask, so any heat conduction from the mouth of the flask must travel the maximum path length to get to the liquid nitrogen. Accordingly, the rate of conductive heat transfer is minimized by doing this.



        3) Radiative heat transfer is largely eliminated by putting a mirror finish on the outside of the inner container.



        All of these techniques mean that heat transfer from the outside of the Dewar flask to the inside of the flask is minimized, and as a consequence, the outside of the flask does not feel cold.



        For more info, see the following:



        https://en.wikipedia.org/wiki/Vacuum_flask



        https://en.wikipedia.org/wiki/Cryogenic_storage_dewar







        share|cite|improve this answer












        share|cite|improve this answer



        share|cite|improve this answer










        answered 5 hours ago









        David WhiteDavid White

        4,4272619




        4,4272619























            1












            $begingroup$

            Gas molecules have higher energy than a molecule that is part of a liquid or solid. Their higher kinetic energy allows them to move freely and bounce off other molecules and atoms, giving them their gaseous properties.



            When a gas is compressed, it forces these high energy particles to get closer together. As they get closer, they aren't able to move as freely. This kinetic energy must be preserved, and is given off in the form of heat to the surrounding container of the gas. Eventually, as pressure increases, these particles will condense together to form a liquid.



            When depressurized, as the liquid converts back to a gas, it will absorb the same amount of heat energy that it expelled when compressed. The heat energy in the container will be taken back by the expanding gas, making the container cool down.



            As for your question, the temperature of the liquid is ambient but at a very high pressure. Having an unsealed bowl of liquid nitrogen would not last long, and would get very cold as the liquid turned back into a gas.



            It has less to do with the static state of the liquid and more to do with the process of going from liquid to gas or vice versa.



            Did this help?






            share|cite|improve this answer









            $endgroup$













            • $begingroup$
              It did help thank you! My presumption was the temperature of liquid gas was constant in that state, so the gas would remain at -320F (nitrogen for example) while in liquid form - including inside a sealer canister/bottle etc. So: the temp of the gas (in liquid form) is only due to the process of the pressure decrease (?) I am just amazed at how quickly it happens. If you had a gallon of liquid nitrogen in a sealed canister at ambient temperature and poured it out into a gallon bucket it would immediately become -320F even in the middle due to the heat energy expelled. (?) thx!!
              $endgroup$
              – Andrew Strever
              1 hour ago










            • $begingroup$
              @AndrewStrever, I think you are drawing the wrong conclusions. Liquid nitrogen cannot exist at ambient temperature, as this is far above its critical temperature. Also, the temperature of a liquid and its vapor inside a sealed container depends on the pressure. As the pressure increases due to evaporation that occurs as a result of heating, the temperature increases also. In a pressurized container of liquid nitrogen, as heat "seeps" into the container, the temperature and pressure increase.
              $endgroup$
              – David White
              41 mins ago












            • $begingroup$
              CuriousOne, your posted answer did not answer the question that the OP asked.
              $endgroup$
              – David White
              37 mins ago
















            1












            $begingroup$

            Gas molecules have higher energy than a molecule that is part of a liquid or solid. Their higher kinetic energy allows them to move freely and bounce off other molecules and atoms, giving them their gaseous properties.



            When a gas is compressed, it forces these high energy particles to get closer together. As they get closer, they aren't able to move as freely. This kinetic energy must be preserved, and is given off in the form of heat to the surrounding container of the gas. Eventually, as pressure increases, these particles will condense together to form a liquid.



            When depressurized, as the liquid converts back to a gas, it will absorb the same amount of heat energy that it expelled when compressed. The heat energy in the container will be taken back by the expanding gas, making the container cool down.



            As for your question, the temperature of the liquid is ambient but at a very high pressure. Having an unsealed bowl of liquid nitrogen would not last long, and would get very cold as the liquid turned back into a gas.



            It has less to do with the static state of the liquid and more to do with the process of going from liquid to gas or vice versa.



            Did this help?






            share|cite|improve this answer









            $endgroup$













            • $begingroup$
              It did help thank you! My presumption was the temperature of liquid gas was constant in that state, so the gas would remain at -320F (nitrogen for example) while in liquid form - including inside a sealer canister/bottle etc. So: the temp of the gas (in liquid form) is only due to the process of the pressure decrease (?) I am just amazed at how quickly it happens. If you had a gallon of liquid nitrogen in a sealed canister at ambient temperature and poured it out into a gallon bucket it would immediately become -320F even in the middle due to the heat energy expelled. (?) thx!!
              $endgroup$
              – Andrew Strever
              1 hour ago










            • $begingroup$
              @AndrewStrever, I think you are drawing the wrong conclusions. Liquid nitrogen cannot exist at ambient temperature, as this is far above its critical temperature. Also, the temperature of a liquid and its vapor inside a sealed container depends on the pressure. As the pressure increases due to evaporation that occurs as a result of heating, the temperature increases also. In a pressurized container of liquid nitrogen, as heat "seeps" into the container, the temperature and pressure increase.
              $endgroup$
              – David White
              41 mins ago












            • $begingroup$
              CuriousOne, your posted answer did not answer the question that the OP asked.
              $endgroup$
              – David White
              37 mins ago














            1












            1








            1





            $begingroup$

            Gas molecules have higher energy than a molecule that is part of a liquid or solid. Their higher kinetic energy allows them to move freely and bounce off other molecules and atoms, giving them their gaseous properties.



            When a gas is compressed, it forces these high energy particles to get closer together. As they get closer, they aren't able to move as freely. This kinetic energy must be preserved, and is given off in the form of heat to the surrounding container of the gas. Eventually, as pressure increases, these particles will condense together to form a liquid.



            When depressurized, as the liquid converts back to a gas, it will absorb the same amount of heat energy that it expelled when compressed. The heat energy in the container will be taken back by the expanding gas, making the container cool down.



            As for your question, the temperature of the liquid is ambient but at a very high pressure. Having an unsealed bowl of liquid nitrogen would not last long, and would get very cold as the liquid turned back into a gas.



            It has less to do with the static state of the liquid and more to do with the process of going from liquid to gas or vice versa.



            Did this help?






            share|cite|improve this answer









            $endgroup$



            Gas molecules have higher energy than a molecule that is part of a liquid or solid. Their higher kinetic energy allows them to move freely and bounce off other molecules and atoms, giving them their gaseous properties.



            When a gas is compressed, it forces these high energy particles to get closer together. As they get closer, they aren't able to move as freely. This kinetic energy must be preserved, and is given off in the form of heat to the surrounding container of the gas. Eventually, as pressure increases, these particles will condense together to form a liquid.



            When depressurized, as the liquid converts back to a gas, it will absorb the same amount of heat energy that it expelled when compressed. The heat energy in the container will be taken back by the expanding gas, making the container cool down.



            As for your question, the temperature of the liquid is ambient but at a very high pressure. Having an unsealed bowl of liquid nitrogen would not last long, and would get very cold as the liquid turned back into a gas.



            It has less to do with the static state of the liquid and more to do with the process of going from liquid to gas or vice versa.



            Did this help?







            share|cite|improve this answer












            share|cite|improve this answer



            share|cite|improve this answer










            answered 5 hours ago









            CuriousOneCuriousOne

            544




            544












            • $begingroup$
              It did help thank you! My presumption was the temperature of liquid gas was constant in that state, so the gas would remain at -320F (nitrogen for example) while in liquid form - including inside a sealer canister/bottle etc. So: the temp of the gas (in liquid form) is only due to the process of the pressure decrease (?) I am just amazed at how quickly it happens. If you had a gallon of liquid nitrogen in a sealed canister at ambient temperature and poured it out into a gallon bucket it would immediately become -320F even in the middle due to the heat energy expelled. (?) thx!!
              $endgroup$
              – Andrew Strever
              1 hour ago










            • $begingroup$
              @AndrewStrever, I think you are drawing the wrong conclusions. Liquid nitrogen cannot exist at ambient temperature, as this is far above its critical temperature. Also, the temperature of a liquid and its vapor inside a sealed container depends on the pressure. As the pressure increases due to evaporation that occurs as a result of heating, the temperature increases also. In a pressurized container of liquid nitrogen, as heat "seeps" into the container, the temperature and pressure increase.
              $endgroup$
              – David White
              41 mins ago












            • $begingroup$
              CuriousOne, your posted answer did not answer the question that the OP asked.
              $endgroup$
              – David White
              37 mins ago


















            • $begingroup$
              It did help thank you! My presumption was the temperature of liquid gas was constant in that state, so the gas would remain at -320F (nitrogen for example) while in liquid form - including inside a sealer canister/bottle etc. So: the temp of the gas (in liquid form) is only due to the process of the pressure decrease (?) I am just amazed at how quickly it happens. If you had a gallon of liquid nitrogen in a sealed canister at ambient temperature and poured it out into a gallon bucket it would immediately become -320F even in the middle due to the heat energy expelled. (?) thx!!
              $endgroup$
              – Andrew Strever
              1 hour ago










            • $begingroup$
              @AndrewStrever, I think you are drawing the wrong conclusions. Liquid nitrogen cannot exist at ambient temperature, as this is far above its critical temperature. Also, the temperature of a liquid and its vapor inside a sealed container depends on the pressure. As the pressure increases due to evaporation that occurs as a result of heating, the temperature increases also. In a pressurized container of liquid nitrogen, as heat "seeps" into the container, the temperature and pressure increase.
              $endgroup$
              – David White
              41 mins ago












            • $begingroup$
              CuriousOne, your posted answer did not answer the question that the OP asked.
              $endgroup$
              – David White
              37 mins ago
















            $begingroup$
            It did help thank you! My presumption was the temperature of liquid gas was constant in that state, so the gas would remain at -320F (nitrogen for example) while in liquid form - including inside a sealer canister/bottle etc. So: the temp of the gas (in liquid form) is only due to the process of the pressure decrease (?) I am just amazed at how quickly it happens. If you had a gallon of liquid nitrogen in a sealed canister at ambient temperature and poured it out into a gallon bucket it would immediately become -320F even in the middle due to the heat energy expelled. (?) thx!!
            $endgroup$
            – Andrew Strever
            1 hour ago




            $begingroup$
            It did help thank you! My presumption was the temperature of liquid gas was constant in that state, so the gas would remain at -320F (nitrogen for example) while in liquid form - including inside a sealer canister/bottle etc. So: the temp of the gas (in liquid form) is only due to the process of the pressure decrease (?) I am just amazed at how quickly it happens. If you had a gallon of liquid nitrogen in a sealed canister at ambient temperature and poured it out into a gallon bucket it would immediately become -320F even in the middle due to the heat energy expelled. (?) thx!!
            $endgroup$
            – Andrew Strever
            1 hour ago












            $begingroup$
            @AndrewStrever, I think you are drawing the wrong conclusions. Liquid nitrogen cannot exist at ambient temperature, as this is far above its critical temperature. Also, the temperature of a liquid and its vapor inside a sealed container depends on the pressure. As the pressure increases due to evaporation that occurs as a result of heating, the temperature increases also. In a pressurized container of liquid nitrogen, as heat "seeps" into the container, the temperature and pressure increase.
            $endgroup$
            – David White
            41 mins ago






            $begingroup$
            @AndrewStrever, I think you are drawing the wrong conclusions. Liquid nitrogen cannot exist at ambient temperature, as this is far above its critical temperature. Also, the temperature of a liquid and its vapor inside a sealed container depends on the pressure. As the pressure increases due to evaporation that occurs as a result of heating, the temperature increases also. In a pressurized container of liquid nitrogen, as heat "seeps" into the container, the temperature and pressure increase.
            $endgroup$
            – David White
            41 mins ago














            $begingroup$
            CuriousOne, your posted answer did not answer the question that the OP asked.
            $endgroup$
            – David White
            37 mins ago




            $begingroup$
            CuriousOne, your posted answer did not answer the question that the OP asked.
            $endgroup$
            – David White
            37 mins ago










            Andrew Strever is a new contributor. Be nice, and check out our Code of Conduct.










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            Plaza Victoria

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            Plaza Victoria Plaza Victoria en 2017 Otros nombres Plaza de La Victoria Localización El Almendral, Valparaíso, Chile Vías adyacentes Chacabuco, Molina, Plaza Victoria y Edwards Creación 1841 Metro Bellavista Ubicación 33°02′46″S 71°37′11″O  /  -33.04624167, -71.61980833 Coordenadas: 33°02′46″S 71°37′11″O  /  -33.04624167, -71.61980833 [editar datos en Wikidata] La Plaza Victoria , también llamada Plaza de la Victoria , [ 1 ] ​ es una plaza ubicada en el sector El Almendral del plan de la ciudad de Valparaíso, Chile, de importancia patrimonial, que incluye valiosas estatuas y especies vegetales. [ 2 ] ​ La plaza se creó como tal en la primera mitad del siglo XIX, tomando previamente los nombres de Plaza Nueva y Plaza de Orrego . Si bien desde sus inicios tuvo relevancia histórica, no fue sino a partir de fines de los años 1860 cuando comenzó a cobrar mayor importancia y se convirtió en uno de los principales centros sociales de l...
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            Puebla de Zaragoza

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            Para otros usos de este término, véase Puebla (desambiguación). Heroica Puebla de Zaragoza Localidad De arriba a abajo de izquierda a derecha: Estrella de Puebla, Volcán Popocatépetl, Catedral de Puebla, Monumento a Ignacio Zaragoza, Estadio Cuauhtémoc, Angelópolis y Vista panorámica de la ciudad. Escudo Otros nombres: El relicario de América/ La ciudad de los Ángeles/ La Angelópolis Lema: Muy noble y muy leal ciudad de Puebla de los Ángeles Heroica Puebla de Zaragoza Localización de Heroica Puebla de Zaragoza en México Heroica Puebla de Zaragoza Localización de Heroica Puebla de Zaragoza en Puebla Mapa interactivo Coordenadas 19°03′05″N 98°13′04″O  /  19.051388888889, -98.217777777778 Coordenadas: 19°03′05″N 98°13′04″O  /  19.051388888889, -98.217777777778 Idioma oficial Español Entidad Localidad  • País   México  • Estado Puebla  • Municipio Puebla Presidente municipal Claudia Rivera Vivanc...
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            Musa

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            Para el género de plantas, véase Musa (planta). Apolo y la Nueve Musas En la mitología griega, las musas (en griego antiguo μοῦσαι « mousai» ) son, según los escritores más antiguos, las divinidades inspiradoras de las Artes: cada una de ellas está relacionada con ramas artísticas y del conocimiento. Son hijas de Zeus y de Mnemósine, compañeras del séquito de Apolo, dios olímpico de la música y patrón de las bellas artes, quien tuvo romances con cada una de ellas, dejando descendientes. Bajaban a la tierra a susurrar ideas e inspirar a aquellos mortales que las invocaran. En la época más arcaica eran las ninfas inspiradoras de las fuentes, en las cuales eran adoradas. Finalmente, alrededor de los siglos VIII-VII a. C. [ 1 ] ​ prevaleció en todo el territorio de la Hélade la adoración de las nueve Musas, que son Calíope, Clío, Erato, Euterpe, Melpómene, Polimnia, Talía, Terpsícore y Urania. El culto a las musas era originalmente de Tracia y Beocia, y fueron de vital impo...
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