The formula is pV=k; this is the Boyle-Mariotte law. If the pressure increase in a closed system the volume decrease.
It is an important gas law.
Charles's Law states that (Volume)/(Temperature) is constant, assuming constant pressure and moles of gas. This means that (V1)/(T1) = (V2)/(T2). So if the volume of the gas increases, V2 is bigger than V1; to keep the ratio constant, T2 must also increase, which represents an increase in temperature.
It is called homeostasis (internal environment maintained at a constant level) or thermostasis (internal heat maintained at a constant temperature). The overall name for the processes by which temperature is controlled is thermoregulation.
Temperature Programming (from what i learned in Quantitative Analysis)
A region that covers two states and has a similar pressure and temperature is called an air mass.
salinity
Charles' Law says that as pressure on a gas decreases, its volume increases. Charles' Law is an example of an inverse relationship.t It is not Charle's law It is Boyle's law Charles law states at constant volume, pressure is proportional to kelvin temperature And at constant pressure volume is proportional to kelvin temperature But Boyle's law states that at constant temperature pressure is inversely related to volume
The process in which change in volume and temperature takes place at a constant pressure is called an isobaric process
You can use Boyle's law to calculate pressure and volume changes at a constant temperature. Boyle's law is an experimental gas law that is sometimes called Boyle-Mariotte law.
That is correct. it's called Charles's law. it shows the connection between a gases temperature and its volume. in order to maintain constant pressure you must increase the volume of the container holding the gas if you increase the temperature of the gas.
Volume will increase. Think of it this way. If you heat a gas, it gets hotter. When a gas gets hotter, the atoms/molecules are "more active" and the pressure and/or the volume will go up. If your experiment with heating this gas sample must have a constant pressure, then volume will have to increase to give all those "more active" atoms/molecules more play room to prevent the pressure from going up.
Diastolic pressure
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.
The initial pressure is halved. Use Boyle's law that relates pressure & volume at a constant temperature. P1V1 = P2V2 In this case the V1(initial volume) is doubled so V2 = 2V1 P2 = P1V1/V2 = P1V1/2V1 P2 = (1/2)*P1
You can use the ideal gas law: PV=RTn, where: P is the pressure V is the volume R is the proportionality constant, the so-called "gas constant" T is the absolute temperature n is the number of moles
YES it is called "pressure temperature relationship" temperature rises so does the pressure
Yes it is possible, for example when water freezes there is a point when the temperature remains constant however energy is released as the water condenses.