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Particle Molecule Deposition
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Tt
total temperature
total distance
Td
Spacial atmosphere
Atmospheric atmosphere ·
Surface atmosphere
Magnetic atmosphere ·
Magnetic core
Core temperature
the approximate temperature ranges for each layer of the Earth:
Crust:
Surface: 0°C to 30°C (32°F to 86°F)
Increases with depth: about 200°C (392°F) at the base.
Mantle:
Upper Mantle: Approximately 500°C to 900°C (932°F to 1,652°F).
Lower Mantle: Approximately 1,000°C to 3,500°C (1,832°F to 6,332°F).
Core:
Outer Core: Approximately 4,000°C to 6,000°C (7,232°F to 10,832°F).
Inner Core: Approximately 5,000°C to 7,000°C (9,032°F to 12,632°F).
These temperatures can vary based on specific locations and conditions within each layer.
Check atmosphere
Boiling Point: 212°F (100°C)
Pressure: 14.7 psi (101.3 kPa)
Boiling Point: ~202°F (94°C)
Pressure: ~12.2 psi (84 kPa)
Boiling Point: ~158°F (70°C)
Pressure: ~4.3 psi (30 kPa)
Boiling Point: Not applicable (water would rapidly evaporate or sublimate)
Pressure: Near vacuum, much lower than at sea level
Temperature: Can exceed 2,000°F (1,100°C)
59 200 218 df
Tt
total temperature
Comparison of Boiling Points: Space vs. Artificial Atmospheres
Boiling Point Basics
The boiling point of a liquid is defined as the temperature at which its vapor pressure equals the surrounding atmospheric pressure. Variations in atmospheric pressure can significantly impact this temperature.
Boiling Point in Space
In the vacuum of space:
Pressure: Near zero, creating a vacuum environment.
Boiling Point: Liquids can boil at very low temperatures. For example, water can boil at room temperature.
59 degrees f
Vaporization: Any exposed liquid rapidly vaporizes, potentially leading to freezing or other phase changes.
Boiling Point in Artificial Atmospheres
In controlled environments, such as laboratories or spacecraft:
1. Increased Pressure
When pressure is increased:
Boiling Point: The boiling point of liquids rises. For example, water can boil at temperatures above 100°C (212°F) in a pressure cooker.
Applications: Useful for cooking, sterilization, and industrial processes that require higher temperatures.
2. Decreased Pressure
When pressure is decreased:
Boiling Point: The boiling point of liquids drops. In a vacuum chamber, water might boil at temperatures below room temperature.
Applications: Techniques like freeze-drying and studying material properties in low-pressure conditions.
3. Stability and Control
Artificial atmospheres allow for:
Precise Adjustments: Pressure and temperature can be finely controlled to achieve desired boiling points.
Consistency: Unlike natural atmospheric conditions, which can vary, artificial settings provide stable environments for experiments and industrial applications.
Understanding how boiling points vary between space and artificial atmospheres highlights the importance of atmospheric pressure in determining the behavior of liquids. Controlled environments allow for significant manipulation of these physical properties, facilitating a range of scientific and practical applications.
Atmospheric pressure decreases with elevation due to the thinning of the air as you go higher. At sea level, the pressure is about 14.7 psi (101.3 kPa). As altitude increases, there are fewer air molecules above exerting pressure, leading to lower atmospheric pressure.
In Colorado, at 5,280 feet (1,609 meters), the pressure drops to about 12.2 psi (84 kPa). This reduction in pressure affects the boiling point of water; lower pressure means water boils at a lower temperature. Hence, water boils at around 202°F (94°C) in Colorado.
At the summit of Mount Everest, at 29,032 feet (8,848 meters), the pressure is significantly lower, around 4.3 psi (30 kPa). This further drop causes the boiling point of water to decrease to approximately 158°F (70°C). The relationship between pressure and boiling point is essential for understanding cooking and weather patterns at high altitudes.
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