The pressure is 68,3 kPa.
As the gas warms it will want to expand and as the pressure is constant it is being allowed to do so. This means that the same number of molecules (the original mass) is/are now taking up a bigger volume and as density is a measure of mass over volume ie:- Density = Mass/volume it is obvious what the density will do because the mass is constant and the volume is increasing. Mass = 10 Volume 1 = 20 Volume 2 = 40 State 1 Mass/Volume 1 = 10/20 = density 0.5 State 2 Mass/Volume 2 = 10/40 = density 0.25
it is very awesome if you see it
Its possible, if a gas can escape it can minutely change volume. If the container is closed and none of the gas that is being given off is allowed to leave then the pressure might change, which possibly can altar the temperature. But overall these minute changes usually aren't significant to be accounted for. Also, it depends on what kind of insulation the container has, like a water bottle will lose heat very quickly, but a thermos will hold heat in, thus keeping the liquid warm : )
This depends upon how high the temperature is increased. To make food cook quicker, when water is placed in a pressure cooker it is allowed to heat up to a much higher temperature than its normal boiling point of 212 degrees Fahrenheit at sea-level. But, at a certain preset pressure, the pressure relief valve will open and release steam. Without this valve the cooker would explode. The same is true for a water heater in your home.
If you increase the temperature of a gas, its particles (atoms or molecules) will speed up. If it is in a closed container, the pressure will also increase.
Isothermal is where pressure and/or volume changes, but temperature remains constant. Pressure, Volume, and Temperature are related as: PV = nRT =NkT for an ideal gas. Here, we see that since a balloon's volume is allowed to change, its pressure remains relatively constant. Whenever there is a pressure change, it'll be offset by an equivalent change in volume, thus temperature is constant.
This is the Gay-Lussac law: at constant volume of a gas the temperature increase when the pressure increase.
This cannot be answered without an initial volume or pressure. But the final pressure of an expansion of a gas can be determined by the following formula. PV/T = P'V'/T' where P = pressure absolute V = volume T = temperature absolute ( ' ) indicates the new pressure, volume and temperature because the temperature is constant this can be reduced to PV = P'V' or P' = PV/V'
If I remember correctly it is a little more complicated than that. The general equation PV=nRT for an ideal gas is elementary knowledge. The fact is that when you increase temperature many things can happen. It depends on how you treat your system. In general if you increase temperature in an open system the pressure will remain fairly constant, but the volume will increase. If it is a closed system in which the volume is not allowed to expand the pressure will increase with increased temperature. You also have to remember chemical properties also such as phase changes. Hope that rambling mess helps lol.
In science, as in real life sometimes several 'factors' effect the outcome of an experiment. In order to make the problem easier to study one or more of these is 'held constant' or not allowed to change in order to see the effect of the other variables. EX. Gas volume can be effected by both pressure and temperature. In order to understand the effect of pressure, Boyle kept the temperature constant. He then changed the pressure to see what happened to the volume of a gas. This gave him what is now called Boyle's Law: The volume of a gas varies inversely as the pressure when the temperature is held constant.
In science, as in real life sometimes several 'factors' effect the outcome of an experiment. In order to make the problem easier to study one or more of these is 'held constant' or not allowed to change in order to see the effect of the other variables. EX. Gas volume can be effected by both pressure and temperature. In order to understand the effect of pressure, Boyle kept the temperature constant. He then changed the pressure to see what happened to the volume of a gas. This gave him what is now called Boyle's Law: The volume of a gas varies inversely as the pressure when the temperature is held constant.
It doesn't change- Apex
It means that if the gas is allowed to expand into a larger volume, the pressure - inside the container that contains the gas - will be less.
The pressure of a gas would be reduced by half if the volume of the container doubled, provided that no other change occurred. Pressure and volume are inversely proportional. The relationship between the two is known as Boyle's law. In brief, the volume of a gas changes inversely with the pressure of the gas if the temperature and quantity of gas remain constant.
This is the reduction of volume to one-third.
As the gas warms it will want to expand and as the pressure is constant it is being allowed to do so. This means that the same number of molecules (the original mass) is/are now taking up a bigger volume and as density is a measure of mass over volume ie:- Density = Mass/volume it is obvious what the density will do because the mass is constant and the volume is increasing. Mass = 10 Volume 1 = 20 Volume 2 = 40 State 1 Mass/Volume 1 = 10/20 = density 0.5 State 2 Mass/Volume 2 = 10/40 = density 0.25
it is very awesome if you see it