39.0
The temperature of the water is 100 degrees celsius.
(P at 1 atm)/(P at 2.5 atm)=(100+273)/Temperature at 2.5 atm932.5 k
The four classical phase changes in matter depend on pressure and temperature. Solids need the lowest amount of pressure and temperature, followed by liquid, then gas, then plasma needing the most. (There are other non-classical states of matter eg. superfluids) The amount of temperature and pressure (or just enthalpy) required to make the phase change depends on the molecular structure of the molecules.
240 Assuming ideal gas behavior, doubling the pressure means reducing the volume by a factor of 2.
urine sample should be between 98-100 degrees F, I got this info at a store that sells pass urineproducts test
False
The temperature of the water is 100 degrees celsius.
100 g Steam at high temperature (>100°C) and pressure (>1 Bar)
(P at 1 atm)/(P at 2.5 atm)=(100+273)/Temperature at 2.5 atm932.5 k
The density of water at standard temperature and pressure is 1 gram/milliliter. The size of the sample is irrelevant. If the sample is pure, then one drop of it has the same density as a tankerful of it has.
The four classical phase changes in matter depend on pressure and temperature. Solids need the lowest amount of pressure and temperature, followed by liquid, then gas, then plasma needing the most. (There are other non-classical states of matter eg. superfluids) The amount of temperature and pressure (or just enthalpy) required to make the phase change depends on the molecular structure of the molecules.
No. Pure water boils at 100 degrees Celsius or less.
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
240 Assuming ideal gas behavior, doubling the pressure means reducing the volume by a factor of 2.
The density of water at standard temperature and pressure is 1 gram/milliliter. The size of the sample is irrelevant. If the sample is pure, then one drop of it has the same density as a tankerful of it has.
Even if the pressure inside a container is equal to the pressure outside a container, there is still pressure. It's like pushing a friend one way while he pushes you back. Neither of you may be moving, but you're still pushing. The sample of gas would exert exactly one atmosphere of pressure (or 100 kPa) on the container. The question then becomes whether the container can withstand that pressure.
As the temperature of the water increases, the amount of solute (in this case NH4Cl) that can be dissolved increases.