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Why does liquid water form when we exhale on a mirror?
Delta G at EqulibriumWhat would be the state of water in interstellar space or vaccum?Describing evaporation without entropy — what about Helmholtz?Liquid nitrogen superheating with a layer of oil?Is water committed to vapor state at boiling point or after?Mass of Ice during Phase ChangeHow do I select a sub-freezing temperature for my experiment that will allow the formation of frost, but not supercooled liquid water (rime)Effect of pressure on the freezing temperature of waterHow does water evaporate completely when at room temperature?Why does the distance between molecules increase when the temperature is raised?
$begingroup$
In the descriptions below, I always assume external pressure to be constant at 1atm, the condition when daily observations are made.
1) When I exhale on a mirror, liquid water forms on the mirror. That's condensation. Obviously, the temperature of mirror must be <100°C, so for water vapors to condense on mirror does make sense, but why do we have water vapors when our body temperature is also <100°C in the first place?
2) One reason for (1) may be like 'water vapors in air is in equilibrium with liquid water', so some water vapors can exist although T<100°C. If this is correct, based on this reasoning, then why not ice exists at T>0°C? [p=1atm only]
3) If liquid water can evaporate into gas at T<100°C, then why not ice turns into liquid at T<0°C? (I never use the term 'melt' here, just like evaporate≠boil) (both have hydrogen bonds, intermolecular forces should be the same?)
4) When I exhale on a wall, no water droplets form. Why water droplets form on mirror but not on wall(just an example)? The mirror must have same temperature as that of wall, both of them must have achieved thermal equilibrium with surrounding long time ago.
physical-chemistry phase
asked 1 hour ago
The99sLearnerThe99sLearner
6117
$endgroup$
add a comment |
$begingroup$
In the descriptions below, I always assume external pressure to be constant at 1atm, the condition when daily observations are made.
1) When I exhale on a mirror, liquid water forms on the mirror. That's condensation. Obviously, the temperature of mirror must be <100°C, so for water vapors to condense on mirror does make sense, but why do we have water vapors when our body temperature is also <100°C in the first place?
2) One reason for (1) may be like 'water vapors in air is in equilibrium with liquid water', so some water vapors can exist although T<100°C. If this is correct, based on this reasoning, then why not ice exists at T>0°C? [p=1atm only]
3) If liquid water can evaporate into gas at T<100°C, then why not ice turns into liquid at T<0°C? (I never use the term 'melt' here, just like evaporate≠boil) (both have hydrogen bonds, intermolecular forces should be the same?)
4) When I exhale on a wall, no water droplets form. Why water droplets form on mirror but not on wall(just an example)? The mirror must have same temperature as that of wall, both of them must have achieved thermal equilibrium with surrounding long time ago.
physical-chemistry phase
asked 1 hour ago
The99sLearnerThe99sLearner
6117
$endgroup$
add a comment |
$begingroup$
In the descriptions below, I always assume external pressure to be constant at 1atm, the condition when daily observations are made.
1) When I exhale on a mirror, liquid water forms on the mirror. That's condensation. Obviously, the temperature of mirror must be <100°C, so for water vapors to condense on mirror does make sense, but why do we have water vapors when our body temperature is also <100°C in the first place?
2) One reason for (1) may be like 'water vapors in air is in equilibrium with liquid water', so some water vapors can exist although T<100°C. If this is correct, based on this reasoning, then why not ice exists at T>0°C? [p=1atm only]
3) If liquid water can evaporate into gas at T<100°C, then why not ice turns into liquid at T<0°C? (I never use the term 'melt' here, just like evaporate≠boil) (both have hydrogen bonds, intermolecular forces should be the same?)
4) When I exhale on a wall, no water droplets form. Why water droplets form on mirror but not on wall(just an example)? The mirror must have same temperature as that of wall, both of them must have achieved thermal equilibrium with surrounding long time ago.
physical-chemistry phase
asked 1 hour ago
The99sLearnerThe99sLearner
6117
$endgroup$
In the descriptions below, I always assume external pressure to be constant at 1atm, the condition when daily observations are made.
1) When I exhale on a mirror, liquid water forms on the mirror. That's condensation. Obviously, the temperature of mirror must be <100°C, so for water vapors to condense on mirror does make sense, but why do we have water vapors when our body temperature is also <100°C in the first place?
2) One reason for (1) may be like 'water vapors in air is in equilibrium with liquid water', so some water vapors can exist although T<100°C. If this is correct, based on this reasoning, then why not ice exists at T>0°C? [p=1atm only]
3) If liquid water can evaporate into gas at T<100°C, then why not ice turns into liquid at T<0°C? (I never use the term 'melt' here, just like evaporate≠boil) (both have hydrogen bonds, intermolecular forces should be the same?)
4) When I exhale on a wall, no water droplets form. Why water droplets form on mirror but not on wall(just an example)? The mirror must have same temperature as that of wall, both of them must have achieved thermal equilibrium with surrounding long time ago.
physical-chemistry phase
physical-chemistry phase
asked 1 hour ago
The99sLearnerThe99sLearner
6117
asked 1 hour ago
The99sLearnerThe99sLearner
6117
asked 1 hour ago
The99sLearnerThe99sLearner
6117
asked 1 hour ago
The99sLearnerThe99sLearner
6117
asked 1 hour ago
The99sLearnerThe99sLearner
6117
6117
add a comment |
add a comment |
1 Answer
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$begingroup$
Why do we have water vapors when our body temperature is also <100°C in the first place?
At normal pressure, water boils at 100°C, meaning that bubbles of pure steam form under water. At lower temperatures, water is in equilibrium between the liquid and the gas phase. The higher the temperature, the higher the vapor pressure, and the higher the equilibrium concentration (partial pressure) of water in air. On the geological scale, there is no equilibrium, and we experience different temperatures, different humidity (related to partial pressure of water in air), and different pressures depending on location.
Why does ice not exist at T>0°C
Ice, as a pure solid, and water, as a pure liquid, have defined concentration at given pressure and temperature. Above the melting temperature, all the ice melts, there is no equilibrium. This is different from the liquid:gas equilibrium, which exists at temperatures below the boiling point, with lower and lower concentrations of the gas as the temperature drops.
If liquid water can evaporate into gas at T<100°C, then why not ice turns into liquid at T<0°C?
Again, this has to do with pure liquids and pure solids having a constant (or nearly constant) concentration. If you add salt to the liquid, however, ice will turn into liquid below the freezing point (effectively lowering the concentration of water in the liquid). Also, the surface of the ice melts at lower temperature than the bulk, so even for pure water, there can be liquid at temperatures below the bulk freezing point.
When I exhale on a wall, no water droplets form.
I would do an experiment and check. I think the water droplets are easier to see on a mirror. Try a grand piano (i.e a smooth surface painted with shiny black paint), you might see the water droplets there as well. Or take a long hot shower and check whether water droplets form on surfaces other than a mirror.
answered 1 hour ago
Karsten TheisKarsten Theis
2,334327
$endgroup$
add a comment |
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$begingroup$
Why do we have water vapors when our body temperature is also <100°C in the first place?
At normal pressure, water boils at 100°C, meaning that bubbles of pure steam form under water. At lower temperatures, water is in equilibrium between the liquid and the gas phase. The higher the temperature, the higher the vapor pressure, and the higher the equilibrium concentration (partial pressure) of water in air. On the geological scale, there is no equilibrium, and we experience different temperatures, different humidity (related to partial pressure of water in air), and different pressures depending on location.
Why does ice not exist at T>0°C
Ice, as a pure solid, and water, as a pure liquid, have defined concentration at given pressure and temperature. Above the melting temperature, all the ice melts, there is no equilibrium. This is different from the liquid:gas equilibrium, which exists at temperatures below the boiling point, with lower and lower concentrations of the gas as the temperature drops.
If liquid water can evaporate into gas at T<100°C, then why not ice turns into liquid at T<0°C?
Again, this has to do with pure liquids and pure solids having a constant (or nearly constant) concentration. If you add salt to the liquid, however, ice will turn into liquid below the freezing point (effectively lowering the concentration of water in the liquid). Also, the surface of the ice melts at lower temperature than the bulk, so even for pure water, there can be liquid at temperatures below the bulk freezing point.
When I exhale on a wall, no water droplets form.
I would do an experiment and check. I think the water droplets are easier to see on a mirror. Try a grand piano (i.e a smooth surface painted with shiny black paint), you might see the water droplets there as well. Or take a long hot shower and check whether water droplets form on surfaces other than a mirror.
answered 1 hour ago
Karsten TheisKarsten Theis
2,334327
$endgroup$
add a comment |
$begingroup$
Why do we have water vapors when our body temperature is also <100°C in the first place?
At normal pressure, water boils at 100°C, meaning that bubbles of pure steam form under water. At lower temperatures, water is in equilibrium between the liquid and the gas phase. The higher the temperature, the higher the vapor pressure, and the higher the equilibrium concentration (partial pressure) of water in air. On the geological scale, there is no equilibrium, and we experience different temperatures, different humidity (related to partial pressure of water in air), and different pressures depending on location.
Why does ice not exist at T>0°C
Ice, as a pure solid, and water, as a pure liquid, have defined concentration at given pressure and temperature. Above the melting temperature, all the ice melts, there is no equilibrium. This is different from the liquid:gas equilibrium, which exists at temperatures below the boiling point, with lower and lower concentrations of the gas as the temperature drops.
If liquid water can evaporate into gas at T<100°C, then why not ice turns into liquid at T<0°C?
Again, this has to do with pure liquids and pure solids having a constant (or nearly constant) concentration. If you add salt to the liquid, however, ice will turn into liquid below the freezing point (effectively lowering the concentration of water in the liquid). Also, the surface of the ice melts at lower temperature than the bulk, so even for pure water, there can be liquid at temperatures below the bulk freezing point.
When I exhale on a wall, no water droplets form.
I would do an experiment and check. I think the water droplets are easier to see on a mirror. Try a grand piano (i.e a smooth surface painted with shiny black paint), you might see the water droplets there as well. Or take a long hot shower and check whether water droplets form on surfaces other than a mirror.
answered 1 hour ago
Karsten TheisKarsten Theis
2,334327
$endgroup$
add a comment |
$begingroup$
Why do we have water vapors when our body temperature is also <100°C in the first place?
At normal pressure, water boils at 100°C, meaning that bubbles of pure steam form under water. At lower temperatures, water is in equilibrium between the liquid and the gas phase. The higher the temperature, the higher the vapor pressure, and the higher the equilibrium concentration (partial pressure) of water in air. On the geological scale, there is no equilibrium, and we experience different temperatures, different humidity (related to partial pressure of water in air), and different pressures depending on location.
Why does ice not exist at T>0°C
Ice, as a pure solid, and water, as a pure liquid, have defined concentration at given pressure and temperature. Above the melting temperature, all the ice melts, there is no equilibrium. This is different from the liquid:gas equilibrium, which exists at temperatures below the boiling point, with lower and lower concentrations of the gas as the temperature drops.
If liquid water can evaporate into gas at T<100°C, then why not ice turns into liquid at T<0°C?
Again, this has to do with pure liquids and pure solids having a constant (or nearly constant) concentration. If you add salt to the liquid, however, ice will turn into liquid below the freezing point (effectively lowering the concentration of water in the liquid). Also, the surface of the ice melts at lower temperature than the bulk, so even for pure water, there can be liquid at temperatures below the bulk freezing point.
When I exhale on a wall, no water droplets form.
I would do an experiment and check. I think the water droplets are easier to see on a mirror. Try a grand piano (i.e a smooth surface painted with shiny black paint), you might see the water droplets there as well. Or take a long hot shower and check whether water droplets form on surfaces other than a mirror.
answered 1 hour ago
Karsten TheisKarsten Theis
2,334327
$endgroup$
Why do we have water vapors when our body temperature is also <100°C in the first place?
At normal pressure, water boils at 100°C, meaning that bubbles of pure steam form under water. At lower temperatures, water is in equilibrium between the liquid and the gas phase. The higher the temperature, the higher the vapor pressure, and the higher the equilibrium concentration (partial pressure) of water in air. On the geological scale, there is no equilibrium, and we experience different temperatures, different humidity (related to partial pressure of water in air), and different pressures depending on location.
Why does ice not exist at T>0°C
Ice, as a pure solid, and water, as a pure liquid, have defined concentration at given pressure and temperature. Above the melting temperature, all the ice melts, there is no equilibrium. This is different from the liquid:gas equilibrium, which exists at temperatures below the boiling point, with lower and lower concentrations of the gas as the temperature drops.
If liquid water can evaporate into gas at T<100°C, then why not ice turns into liquid at T<0°C?
Again, this has to do with pure liquids and pure solids having a constant (or nearly constant) concentration. If you add salt to the liquid, however, ice will turn into liquid below the freezing point (effectively lowering the concentration of water in the liquid). Also, the surface of the ice melts at lower temperature than the bulk, so even for pure water, there can be liquid at temperatures below the bulk freezing point.
When I exhale on a wall, no water droplets form.
I would do an experiment and check. I think the water droplets are easier to see on a mirror. Try a grand piano (i.e a smooth surface painted with shiny black paint), you might see the water droplets there as well. Or take a long hot shower and check whether water droplets form on surfaces other than a mirror.
answered 1 hour ago
Karsten TheisKarsten Theis
2,334327
answered 1 hour ago
Karsten TheisKarsten Theis
2,334327
answered 1 hour ago
Karsten TheisKarsten Theis
2,334327
answered 1 hour ago
Karsten TheisKarsten Theis
2,334327
2,334327
add a comment |
add a comment |
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