water boils when the vapour pressure becomes equal to the external pressure. So if we increase the pressure, the rate of boiling will increase. Think of the vapor pressure as the pressure that is needed to force a bubble to the surface.
it lowers
Pressure times Volume = Number of moles times Gas constant times Temperature
The constant will not change. The number of moles is assumed not to change in a closed container. The volume unchanging, if pressure increases then the temperature would theoretically have to increase, though artificially increasing pressure without changing the volume of the container, adding energy, or introducing additional matter is very difficult, if not impossible.
If pressure increases and temperature remains the same, then the water would stop boiling.
If pressure decreases and temperature remains the same, then the water would boil more and more ferochiously.
As water transforms to steam, this process takes up a lot of energy and this regulates the actual temperature of the water boiling. Water boiling at 1 Atm pressure will "never" be hotter than 100 degrees Celsius. This is the point where excess energy is transforming parts of the water into steam hence discouraging the temperature of the water to go beyond 100 degrees Celsius.
By increasing the atmospheric pressure, the temperature needed in order to transform water into steam also increases accordingly
Increasing the pressure the boiling point is increased (and inversely).
as pressure decreases water boils at lower temperatures. as pressure increases water boils at higher temperatures. Only at sea level does water boil at exactly 100 degrees C.
the pressure decreases the pressure increases
the air pressure changes because gas paticles are farther apart and air pressure decreases
This would actually be a simple answer: Pressure decreases. Simply because of the fact that as altitude increases, the less air there is on top of you, and the lower the pressure would be.
As particle size in increases, capillarity decreases
The boiling point of water is 100 degrees C, but only at sea level, or in other words, at an atmospheric pressure of 1013.2 millibars. As the altitude increases (or the pressure decreases, same thing), the boiling point goes down. This happens at the rate of about 1 degree C for every thousand feet of altitude gained or for every 35 millibars of pressure lost. The boiling point of pure water is 100 0C at 760 mm col. Hg. ((101.325 kPa of atmospheric pressure). This is not a coincidence. The Celsius scale was originally defined around the boiling and freezing points of water.
density decreases as air pressure increases
the pressure decreases the pressure increases
increases
Pressure decreases.
The boiling point of water is dependent on environmental factors and the presence of solutes. In this case the pressure of the system on the water serves to increase the boiling point of water. The higher pressures increase boiling points while lowering pressure decreases it.
As altitude increases, pressure decreases, so boiling point decreases, so the liquid would boil at a lower temperature and would not be able to get as hot and remain a liquid. As pressure is increased, boiling point increases, meaning the liquid could get hotter than normal and remain a liquid.PV=nRT - pressure x volume = the number of moles x constant x temperature
Pressure decreases
The speed increases and the pressure decreases.
The speed increases and the pressure decreases.
The temperature decreases. For example if you want to boil and egg on top of a mountain then it will take longer.
The boiling point of a liquid increases when atmospheric pressure is increased.
As you go above sea level, the atmospheric pressure decreases, and so the boiling point also decreases to below 100ºC.