The boiling point of bromine under a pressure of 75 kPa is approximately 58°C. At this pressure, the boiling point of bromine is lower than its usual boiling point of 58.8°C at standard atmospheric pressure.
The boiling point of a liquid decreases with decreasing pressure and increases with increasing pressure. This is because at higher pressures, more energy is required to overcome the external pressure and allow the liquid to change into a gas, resulting in a higher boiling point. Conversely, at lower pressures, less energy is needed, leading to a lower boiling point.
Abnormally low pressure decreases the boiling point of a compound because it reduces the pressure exerted on the liquid, making it easier for molecules to escape into the gas phase. This results in a lower energy requirement for the liquid to vaporize, lowering the boiling point.
The boiling point of NH3, which is ammonia, is -33.34°C (-28°F) at standard atmospheric pressure.
Nitrogen melts at 63.15 K or -210.00 °C or -346.00 °F. Nitrogen boils at 77.36 K or -195.79 °C or -320.3342 °F. Everything more you need can be found by using the link below. It will take you to the Wikipedia post on nitrogen, and knowledge is provided there for free.
The boiling point of oxygen at atmospheric pressure (1 atm) is -183 degrees Celsius.
salt or sugar would lower the melting point and raise the boiling point. The salt or sugar would reduce the partial pressure of water in the solution (essentially more competition), effectively raising the boiling point.
Chlorine has a higher boiling point than oxygen. Chlorine's boiling point is -34.6 degrees Celsius, while oxygen's boiling point is -183 degrees Celsius.
Boiling point is when the liquids pressure equals the pressure of the atmosphere.
Boiling is dependent on pressure because the pressure affects the boiling point of a substance. When the pressure is higher, the boiling point of a substance is also higher, and when the pressure is lower, the boiling point is lower. This is because pressure affects the vapor pressure of the substance, which needs to equal the atmospheric pressure for boiling to occur.
The boiling point of oxygen is -183 degrees Celsius.
The boiling point of a liquid depends on the pressure applied to it: higher pressure raises the boiling point and lower pressure decreases it. By reporting the boiling point along with the pressure, it allows for accurate comparison and reproducibility of experimental results, as different pressure conditions can affect the boiling point.
Oxygen has the lowest boiling point of these. It is far below the boiling points of the others.
Water - or other liquids - will evaporate at practically any temperature. Boiling is defined as the temperature at which the partial vapor pressure is equal to the atmospheric pressure. In practical terms, it means that the boiling water (or other liquid) can't get any hotter assuming the pressure doesn't change. You'll also see lots of bubbles rising from the boiling liquid (but before it is boiling, there will also be a few bubbles).
At low pressure the boiling point is lowered and inverse.
An increase in pressure raises the boiling point of a liquid because it takes more energy for the liquid molecules to escape the higher atmospheric pressure above them. Conversely, decreasing the pressure lowers the boiling point as it requires less energy for the molecules to overcome the reduced atmospheric pressure.
Air pressure also affects the boiling point of water. The higher the air pressure, the higher the boiling point.