How much salt (or any other substance one can find in a kitchen) do I need to add to make water boil at 104 °C? [closed]
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How much salt (or any other substance one can find in a kitchen) do I need to add to make water boil at 104 °C? [closed]
$begingroup$
I've seen some formulas around in other questions and Google searches, but my chemistry is pretty much dead so I have no clue where to find the relevant values to calculate it myself. I just need to make an oil bath at 104 °C, but I would prefer to use a water solution instead since it is cheaper and easier to clean up. Doesn't need to be salt, can be anything commonly available at your average household.
everyday-chemistry experimental-chemistry aqueous-solution boiling-point colligative-properties
edited Jun 3 at 6:25
andselisk♦
21.2k773142
asked Jun 3 at 5:52
Louis VictorLouis Victor
372
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Louis Victor is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
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closed as too broad by Nilay Ghosh, Mithoron, M.A.R. ಠ_ಠ, airhuff, Todd Minehardt Jun 3 at 22:10
Please edit the question to limit it to a specific problem with enough detail to identify an adequate answer. Avoid asking multiple distinct questions at once. See the How to Ask page for help clarifying this question. If this question can be reworded to fit the rules in the help center, please edit the question.
add a comment |
$begingroup$
I've seen some formulas around in other questions and Google searches, but my chemistry is pretty much dead so I have no clue where to find the relevant values to calculate it myself. I just need to make an oil bath at 104 °C, but I would prefer to use a water solution instead since it is cheaper and easier to clean up. Doesn't need to be salt, can be anything commonly available at your average household.
everyday-chemistry experimental-chemistry aqueous-solution boiling-point colligative-properties
edited Jun 3 at 6:25
andselisk♦
21.2k773142
asked Jun 3 at 5:52
Louis VictorLouis Victor
372
New contributor
Louis Victor is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
closed as too broad by Nilay Ghosh, Mithoron, M.A.R. ಠ_ಠ, airhuff, Todd Minehardt Jun 3 at 22:10
Please edit the question to limit it to a specific problem with enough detail to identify an adequate answer. Avoid asking multiple distinct questions at once. See the How to Ask page for help clarifying this question. If this question can be reworded to fit the rules in the help center, please edit the question.
add a comment |
$begingroup$
I've seen some formulas around in other questions and Google searches, but my chemistry is pretty much dead so I have no clue where to find the relevant values to calculate it myself. I just need to make an oil bath at 104 °C, but I would prefer to use a water solution instead since it is cheaper and easier to clean up. Doesn't need to be salt, can be anything commonly available at your average household.
everyday-chemistry experimental-chemistry aqueous-solution boiling-point colligative-properties
edited Jun 3 at 6:25
andselisk♦
21.2k773142
asked Jun 3 at 5:52
Louis VictorLouis Victor
372
New contributor
Louis Victor is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
I've seen some formulas around in other questions and Google searches, but my chemistry is pretty much dead so I have no clue where to find the relevant values to calculate it myself. I just need to make an oil bath at 104 °C, but I would prefer to use a water solution instead since it is cheaper and easier to clean up. Doesn't need to be salt, can be anything commonly available at your average household.
everyday-chemistry experimental-chemistry aqueous-solution boiling-point colligative-properties
everyday-chemistry experimental-chemistry aqueous-solution boiling-point colligative-properties
edited Jun 3 at 6:25
andselisk♦
21.2k773142
asked Jun 3 at 5:52
Louis VictorLouis Victor
372
New contributor
Louis Victor is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
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edited Jun 3 at 6:25
andselisk♦
21.2k773142
asked Jun 3 at 5:52
Louis VictorLouis Victor
372
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Louis Victor is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
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edited Jun 3 at 6:25
andselisk♦
21.2k773142
edited Jun 3 at 6:25
andselisk♦
21.2k773142
edited Jun 3 at 6:25
andselisk♦
21.2k773142
21.2k773142
asked Jun 3 at 5:52
Louis VictorLouis Victor
372
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Louis Victor is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
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asked Jun 3 at 5:52
Louis VictorLouis Victor
372
asked Jun 3 at 5:52
Louis VictorLouis Victor
372
372
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New contributor
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Check out our Code of Conduct.
closed as too broad by Nilay Ghosh, Mithoron, M.A.R. ಠ_ಠ, airhuff, Todd Minehardt Jun 3 at 22:10
Please edit the question to limit it to a specific problem with enough detail to identify an adequate answer. Avoid asking multiple distinct questions at once. See the How to Ask page for help clarifying this question. If this question can be reworded to fit the rules in the help center, please edit the question.
closed as too broad by Nilay Ghosh, Mithoron, M.A.R. ಠ_ಠ, airhuff, Todd Minehardt Jun 3 at 22:10
Please edit the question to limit it to a specific problem with enough detail to identify an adequate answer. Avoid asking multiple distinct questions at once. See the How to Ask page for help clarifying this question. If this question can be reworded to fit the rules in the help center, please edit the question.
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3 Answers
3
active
oldest
votes
$begingroup$
According to [1, pp. 281–282], solution of sodium chloride $ceNaCl$ prepared by dissolving 25 g of salt in 100 g of water has boiling point of 104.6 °C.
Additional data is available in the following table for the aqueous solutions of common salts and bases.
English transcription; column 1: Compound; columns 2–6: Concentration, g/100 g water — boiling points $(t_mathrmb.p.,~pu°C)$.
Note, however, that there is a significant drawback of using boiling salt solution due to the shift of boiling point upwards as the water boils off.
You either have to add water to the mark from time to time, or use a bath with another heat carrier and a thermal sensor.
References
- V.A. Rabinovich and Z.Y. Havin. (Eds.) "Kratkii khimicheskii spravochnik" (Brief chemical handbook), 2nd ed., Khimiya, Leningrad, 1978. (in Russian)
answered Jun 3 at 6:15
andselisk♦andselisk
21.2k773142
$endgroup$
6
$begingroup$
Consider the altitude at which you will run your operation, too. @Louis Victor.
$endgroup$
– Alchimista
Jun 3 at 10:03
1
$begingroup$
@Alchimista Thank you for the valuable addition to the flatlander's answer.:)
$endgroup$
– andselisk♦
Jun 3 at 10:10
1
$begingroup$
Wow, lithium chloride is powerful stuff!
$endgroup$
– Curt F.
Jun 3 at 20:42
add a comment |
$begingroup$
Boiling point elevation of water by adding salt can be predicted with the formula:
$$Delta T_b= K_b, b_solute , i$$
We look for $Delta T_b=4$, using water $K_b=0.512$, and $i=2$ for salt $ceNaCl$
$b$ is the molality, and as an estimation $b=4$ and it is the number $ceNaCl$ moles per kilogram of solution. Then $$fracg_salt100 g_H2O=fracbtimes100(1000-btimes PM_salt), PM_salt$$ $fracg_NaCl100 g_H2O=frac4times100(1000-4times 58.5)*58.5=30.55$ (results).
$i$ of Different salts can be found (some examples here).
edited Jun 4 at 4:07
Nilay Ghosh
9,8371046109
answered Jun 3 at 18:26
santimirandarpsantimirandarp
1,275524
$endgroup$
add a comment |
$begingroup$
A pressure cooker will allow boiling temperature to increase to 115 degrees or so by pressuring the cooking space. Its not quite salt, but you could find one in a kitchen.
Commonly set to HIGH or LOW using a weight on the vent
Setting LOW would be 0.4~0.55 bar and HIGH would be 0.9~1 bar so double atmospheric pressure. Readings are on top of the 1 bar normal atmospheric pressure of the room.
By comparison, a car tyre would be about 2.2 bar, so just over triple normal room pressure air.
0.5 bar would be a boiling point of 112 degrees C
1.0 bar would boil at 120 degrees C
2.6 bar would be 140 degrees C, but good luck getting such pressures in the kitchen.
Disclaimer, even 0.5 bar is a lot of pressure, and any rupture will cause significant damage.
answered Jun 3 at 16:49
CriggieCriggie
1114
New contributor
Criggie is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
2
$begingroup$
Maybe you should mention that these values refer to gauge pressure, and not to absolute pressure which is normally used in chemistry.
$endgroup$
– Loong♦
Jun 3 at 17:03
add a comment |
3 Answers
3
active
oldest
votes
3 Answers
3
active
oldest
votes
active
oldest
votes
active
oldest
votes
$begingroup$
According to [1, pp. 281–282], solution of sodium chloride $ceNaCl$ prepared by dissolving 25 g of salt in 100 g of water has boiling point of 104.6 °C.
Additional data is available in the following table for the aqueous solutions of common salts and bases.
English transcription; column 1: Compound; columns 2–6: Concentration, g/100 g water — boiling points $(t_mathrmb.p.,~pu°C)$.
Note, however, that there is a significant drawback of using boiling salt solution due to the shift of boiling point upwards as the water boils off.
You either have to add water to the mark from time to time, or use a bath with another heat carrier and a thermal sensor.
References
- V.A. Rabinovich and Z.Y. Havin. (Eds.) "Kratkii khimicheskii spravochnik" (Brief chemical handbook), 2nd ed., Khimiya, Leningrad, 1978. (in Russian)
answered Jun 3 at 6:15
andselisk♦andselisk
21.2k773142
$endgroup$
6
$begingroup$
Consider the altitude at which you will run your operation, too. @Louis Victor.
$endgroup$
– Alchimista
Jun 3 at 10:03
1
$begingroup$
@Alchimista Thank you for the valuable addition to the flatlander's answer.:)
$endgroup$
– andselisk♦
Jun 3 at 10:10
1
$begingroup$
Wow, lithium chloride is powerful stuff!
$endgroup$
– Curt F.
Jun 3 at 20:42
add a comment |
$begingroup$
According to [1, pp. 281–282], solution of sodium chloride $ceNaCl$ prepared by dissolving 25 g of salt in 100 g of water has boiling point of 104.6 °C.
Additional data is available in the following table for the aqueous solutions of common salts and bases.
English transcription; column 1: Compound; columns 2–6: Concentration, g/100 g water — boiling points $(t_mathrmb.p.,~pu°C)$.
Note, however, that there is a significant drawback of using boiling salt solution due to the shift of boiling point upwards as the water boils off.
You either have to add water to the mark from time to time, or use a bath with another heat carrier and a thermal sensor.
References
- V.A. Rabinovich and Z.Y. Havin. (Eds.) "Kratkii khimicheskii spravochnik" (Brief chemical handbook), 2nd ed., Khimiya, Leningrad, 1978. (in Russian)
answered Jun 3 at 6:15
andselisk♦andselisk
21.2k773142
$endgroup$
6
$begingroup$
Consider the altitude at which you will run your operation, too. @Louis Victor.
$endgroup$
– Alchimista
Jun 3 at 10:03
1
$begingroup$
@Alchimista Thank you for the valuable addition to the flatlander's answer.:)
$endgroup$
– andselisk♦
Jun 3 at 10:10
1
$begingroup$
Wow, lithium chloride is powerful stuff!
$endgroup$
– Curt F.
Jun 3 at 20:42
add a comment |
$begingroup$
According to [1, pp. 281–282], solution of sodium chloride $ceNaCl$ prepared by dissolving 25 g of salt in 100 g of water has boiling point of 104.6 °C.
Additional data is available in the following table for the aqueous solutions of common salts and bases.
English transcription; column 1: Compound; columns 2–6: Concentration, g/100 g water — boiling points $(t_mathrmb.p.,~pu°C)$.
Note, however, that there is a significant drawback of using boiling salt solution due to the shift of boiling point upwards as the water boils off.
You either have to add water to the mark from time to time, or use a bath with another heat carrier and a thermal sensor.
References
- V.A. Rabinovich and Z.Y. Havin. (Eds.) "Kratkii khimicheskii spravochnik" (Brief chemical handbook), 2nd ed., Khimiya, Leningrad, 1978. (in Russian)
answered Jun 3 at 6:15
andselisk♦andselisk
21.2k773142
$endgroup$
According to [1, pp. 281–282], solution of sodium chloride $ceNaCl$ prepared by dissolving 25 g of salt in 100 g of water has boiling point of 104.6 °C.
Additional data is available in the following table for the aqueous solutions of common salts and bases.
English transcription; column 1: Compound; columns 2–6: Concentration, g/100 g water — boiling points $(t_mathrmb.p.,~pu°C)$.
Note, however, that there is a significant drawback of using boiling salt solution due to the shift of boiling point upwards as the water boils off.
You either have to add water to the mark from time to time, or use a bath with another heat carrier and a thermal sensor.
References
- V.A. Rabinovich and Z.Y. Havin. (Eds.) "Kratkii khimicheskii spravochnik" (Brief chemical handbook), 2nd ed., Khimiya, Leningrad, 1978. (in Russian)
answered Jun 3 at 6:15
andselisk♦andselisk
21.2k773142
edited Jun 3 at 6:31
answered Jun 3 at 6:15
andselisk♦andselisk
21.2k773142
answered Jun 3 at 6:15
andselisk♦andselisk
21.2k773142
answered Jun 3 at 6:15
andselisk♦andselisk
21.2k773142
21.2k773142
6
$begingroup$
Consider the altitude at which you will run your operation, too. @Louis Victor.
$endgroup$
– Alchimista
Jun 3 at 10:03
1
$begingroup$
@Alchimista Thank you for the valuable addition to the flatlander's answer.:)
$endgroup$
– andselisk♦
Jun 3 at 10:10
1
$begingroup$
Wow, lithium chloride is powerful stuff!
$endgroup$
– Curt F.
Jun 3 at 20:42
add a comment |
6
$begingroup$
Consider the altitude at which you will run your operation, too. @Louis Victor.
$endgroup$
– Alchimista
Jun 3 at 10:03
1
$begingroup$
@Alchimista Thank you for the valuable addition to the flatlander's answer.:)
$endgroup$
– andselisk♦
Jun 3 at 10:10
1
$begingroup$
Wow, lithium chloride is powerful stuff!
$endgroup$
– Curt F.
Jun 3 at 20:42
6
6
$begingroup$
Consider the altitude at which you will run your operation, too. @Louis Victor.
$endgroup$
– Alchimista
Jun 3 at 10:03
$begingroup$
Consider the altitude at which you will run your operation, too. @Louis Victor.
$endgroup$
– Alchimista
Jun 3 at 10:03
1
1
$begingroup$
@Alchimista Thank you for the valuable addition to the flatlander's answer.:)
$endgroup$
– andselisk♦
Jun 3 at 10:10
$begingroup$
@Alchimista Thank you for the valuable addition to the flatlander's answer.:)
$endgroup$
– andselisk♦
Jun 3 at 10:10
1
1
$begingroup$
Wow, lithium chloride is powerful stuff!
$endgroup$
– Curt F.
Jun 3 at 20:42
$begingroup$
Wow, lithium chloride is powerful stuff!
$endgroup$
– Curt F.
Jun 3 at 20:42
add a comment |
$begingroup$
Boiling point elevation of water by adding salt can be predicted with the formula:
$$Delta T_b= K_b, b_solute , i$$
We look for $Delta T_b=4$, using water $K_b=0.512$, and $i=2$ for salt $ceNaCl$
$b$ is the molality, and as an estimation $b=4$ and it is the number $ceNaCl$ moles per kilogram of solution. Then $$fracg_salt100 g_H2O=fracbtimes100(1000-btimes PM_salt), PM_salt$$ $fracg_NaCl100 g_H2O=frac4times100(1000-4times 58.5)*58.5=30.55$ (results).
$i$ of Different salts can be found (some examples here).
edited Jun 4 at 4:07
Nilay Ghosh
9,8371046109
answered Jun 3 at 18:26
santimirandarpsantimirandarp
1,275524
$endgroup$
add a comment |
$begingroup$
Boiling point elevation of water by adding salt can be predicted with the formula:
$$Delta T_b= K_b, b_solute , i$$
We look for $Delta T_b=4$, using water $K_b=0.512$, and $i=2$ for salt $ceNaCl$
$b$ is the molality, and as an estimation $b=4$ and it is the number $ceNaCl$ moles per kilogram of solution. Then $$fracg_salt100 g_H2O=fracbtimes100(1000-btimes PM_salt), PM_salt$$ $fracg_NaCl100 g_H2O=frac4times100(1000-4times 58.5)*58.5=30.55$ (results).
$i$ of Different salts can be found (some examples here).
edited Jun 4 at 4:07
Nilay Ghosh
9,8371046109
answered Jun 3 at 18:26
santimirandarpsantimirandarp
1,275524
$endgroup$
add a comment |
$begingroup$
Boiling point elevation of water by adding salt can be predicted with the formula:
$$Delta T_b= K_b, b_solute , i$$
We look for $Delta T_b=4$, using water $K_b=0.512$, and $i=2$ for salt $ceNaCl$
$b$ is the molality, and as an estimation $b=4$ and it is the number $ceNaCl$ moles per kilogram of solution. Then $$fracg_salt100 g_H2O=fracbtimes100(1000-btimes PM_salt), PM_salt$$ $fracg_NaCl100 g_H2O=frac4times100(1000-4times 58.5)*58.5=30.55$ (results).
$i$ of Different salts can be found (some examples here).
edited Jun 4 at 4:07
Nilay Ghosh
9,8371046109
answered Jun 3 at 18:26
santimirandarpsantimirandarp
1,275524
$endgroup$
Boiling point elevation of water by adding salt can be predicted with the formula:
$$Delta T_b= K_b, b_solute , i$$
We look for $Delta T_b=4$, using water $K_b=0.512$, and $i=2$ for salt $ceNaCl$
$b$ is the molality, and as an estimation $b=4$ and it is the number $ceNaCl$ moles per kilogram of solution. Then $$fracg_salt100 g_H2O=fracbtimes100(1000-btimes PM_salt), PM_salt$$ $fracg_NaCl100 g_H2O=frac4times100(1000-4times 58.5)*58.5=30.55$ (results).
$i$ of Different salts can be found (some examples here).
edited Jun 4 at 4:07
Nilay Ghosh
9,8371046109
answered Jun 3 at 18:26
santimirandarpsantimirandarp
1,275524
edited Jun 4 at 4:07
Nilay Ghosh
9,8371046109
edited Jun 4 at 4:07
Nilay Ghosh
9,8371046109
edited Jun 4 at 4:07
Nilay Ghosh
9,8371046109
9,8371046109
answered Jun 3 at 18:26
santimirandarpsantimirandarp
1,275524
answered Jun 3 at 18:26
santimirandarpsantimirandarp
1,275524
answered Jun 3 at 18:26
santimirandarpsantimirandarp
1,275524
1,275524
add a comment |
add a comment |
$begingroup$
A pressure cooker will allow boiling temperature to increase to 115 degrees or so by pressuring the cooking space. Its not quite salt, but you could find one in a kitchen.
Commonly set to HIGH or LOW using a weight on the vent
Setting LOW would be 0.4~0.55 bar and HIGH would be 0.9~1 bar so double atmospheric pressure. Readings are on top of the 1 bar normal atmospheric pressure of the room.
By comparison, a car tyre would be about 2.2 bar, so just over triple normal room pressure air.
0.5 bar would be a boiling point of 112 degrees C
1.0 bar would boil at 120 degrees C
2.6 bar would be 140 degrees C, but good luck getting such pressures in the kitchen.
Disclaimer, even 0.5 bar is a lot of pressure, and any rupture will cause significant damage.
answered Jun 3 at 16:49
CriggieCriggie
1114
New contributor
Criggie is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
2
$begingroup$
Maybe you should mention that these values refer to gauge pressure, and not to absolute pressure which is normally used in chemistry.
$endgroup$
– Loong♦
Jun 3 at 17:03
add a comment |
$begingroup$
A pressure cooker will allow boiling temperature to increase to 115 degrees or so by pressuring the cooking space. Its not quite salt, but you could find one in a kitchen.
Commonly set to HIGH or LOW using a weight on the vent
Setting LOW would be 0.4~0.55 bar and HIGH would be 0.9~1 bar so double atmospheric pressure. Readings are on top of the 1 bar normal atmospheric pressure of the room.
By comparison, a car tyre would be about 2.2 bar, so just over triple normal room pressure air.
0.5 bar would be a boiling point of 112 degrees C
1.0 bar would boil at 120 degrees C
2.6 bar would be 140 degrees C, but good luck getting such pressures in the kitchen.
Disclaimer, even 0.5 bar is a lot of pressure, and any rupture will cause significant damage.
answered Jun 3 at 16:49
CriggieCriggie
1114
New contributor
Criggie is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
2
$begingroup$
Maybe you should mention that these values refer to gauge pressure, and not to absolute pressure which is normally used in chemistry.
$endgroup$
– Loong♦
Jun 3 at 17:03
add a comment |
$begingroup$
A pressure cooker will allow boiling temperature to increase to 115 degrees or so by pressuring the cooking space. Its not quite salt, but you could find one in a kitchen.
Commonly set to HIGH or LOW using a weight on the vent
Setting LOW would be 0.4~0.55 bar and HIGH would be 0.9~1 bar so double atmospheric pressure. Readings are on top of the 1 bar normal atmospheric pressure of the room.
By comparison, a car tyre would be about 2.2 bar, so just over triple normal room pressure air.
0.5 bar would be a boiling point of 112 degrees C
1.0 bar would boil at 120 degrees C
2.6 bar would be 140 degrees C, but good luck getting such pressures in the kitchen.
Disclaimer, even 0.5 bar is a lot of pressure, and any rupture will cause significant damage.
answered Jun 3 at 16:49
CriggieCriggie
1114
New contributor
Criggie is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
$endgroup$
A pressure cooker will allow boiling temperature to increase to 115 degrees or so by pressuring the cooking space. Its not quite salt, but you could find one in a kitchen.
Commonly set to HIGH or LOW using a weight on the vent
Setting LOW would be 0.4~0.55 bar and HIGH would be 0.9~1 bar so double atmospheric pressure. Readings are on top of the 1 bar normal atmospheric pressure of the room.
By comparison, a car tyre would be about 2.2 bar, so just over triple normal room pressure air.
0.5 bar would be a boiling point of 112 degrees C
1.0 bar would boil at 120 degrees C
2.6 bar would be 140 degrees C, but good luck getting such pressures in the kitchen.
Disclaimer, even 0.5 bar is a lot of pressure, and any rupture will cause significant damage.
answered Jun 3 at 16:49
CriggieCriggie
1114
New contributor
Criggie is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
edited Jun 3 at 17:30
answered Jun 3 at 16:49
CriggieCriggie
1114
New contributor
Criggie is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
answered Jun 3 at 16:49
CriggieCriggie
1114
answered Jun 3 at 16:49
CriggieCriggie
1114
1114
New contributor
Criggie is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
New contributor
Criggie is a new contributor to this site. Take care in asking for clarification, commenting, and answering.
Check out our Code of Conduct.
2
$begingroup$
Maybe you should mention that these values refer to gauge pressure, and not to absolute pressure which is normally used in chemistry.
$endgroup$
– Loong♦
Jun 3 at 17:03
add a comment |
2
$begingroup$
Maybe you should mention that these values refer to gauge pressure, and not to absolute pressure which is normally used in chemistry.
$endgroup$
– Loong♦
Jun 3 at 17:03
2
2
$begingroup$
Maybe you should mention that these values refer to gauge pressure, and not to absolute pressure which is normally used in chemistry.
$endgroup$
– Loong♦
Jun 3 at 17:03
$begingroup$
Maybe you should mention that these values refer to gauge pressure, and not to absolute pressure which is normally used in chemistry.
$endgroup$
– Loong♦
Jun 3 at 17:03
add a comment |
