What cause the pressure to increase?
Is caused by the increase in the number of collisions of molecules of air with the inside walls of the object
Is defined as the force per unit area on a surface.
The SI unit for force, it is the force that will increase the speed of a one-kilogram mass by one meter per second each second that the force is applied.
A device used to measure atmospheric pressure.
Used to measure the pressure of an enclosed gas sample.
Millimeters of mercury
The common unit of pressure, symbolized mm Hg.
Atmosphere of pressure
Is defined as being exactly equivalent to 760 mm Hg.
Defined as the pressure exerted by a force of one newton acting on an area of one square meter.
The pressure of each gas in a mixture, of that gas.
Dalton's law of partial pressures
states that the total pressure of a gas mixture is the sum of the partial pressures of the component gases.
States that the volume of a fixed mass of gas varies inversely with the pressure at constant temperature. PV=PV
The temperature -273.15C is given a value of zero in the Kelvin scale.
States that the volume of a fixed mass of gas at constant pressure varies directly with the Kelvin temperature. V/T=V/T
The pressure of a fixed mass of gas at constant volume varies directly with the Kelvin temperature P/T=P/T
Combined gas law
expresses the relationship between pressure, volume, and temperature of a fixed amount of gas. PV/T=PV/T
Gay-Lussac's law of combining volumes of gases
at constant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole number.
equal volumes of gases at the same temperature and pressure contain equal numbers of molecules
Standard molar volume of a gas
The volume occupied by one mole of a gas at STP, it has been found to be 22.41410L
Ideal gas law
The mathematical relationship among pressure, volume, temperature, and the number of moles of a gas. PV=nRT
Ideal gas constant
the constant R, its value depends on the units chosen for pressure, volume, and temperature.
The gradual mixing of two or more gases due to their spontaneous, random motion.
the process whereby the molecules of a gas confined in a container randomly pass through a tiny opening in the container.
Graham's law of effusion
States that the rates of effusion of gases at the same temperature and pressure are inversely proportional to the square roots of their molar masses.