Ideal gas equation
- Created by: Bellaboo1424
- Created on: 19-11-20 13:45
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- IDEALGAS EQUATION
- KINETIC THEORY
- There is no such thing as an ideal gas but many gases behave as if they were ideal at ordinary working temperatures and pressures.
- The assumptions are:
- 1.Gases are made up of molecules which are in constant random motion in straight lines.
- 2.The molecules behave as rigid spheres.
- 3.Pressure is due to collisions between the molecules and the walls of the container.
- 4.All collisions, both between the molecules themselves, and between the molecules and the walls of the container, are perfectly elastic. (That means that there is no loss of kinetic energy during the collision.)
- The temperature of the gas is proportional to the average kinetic energy of the molecules.
- key assumptions
- 1.There are no (or entirely negligible) intermolecular forces between the gas molecules.
- 2.The volume occupied by the molecules themselves is entirely negligible relative to the volume of the container.
- IDEAL GAS EQUATION
- pV = nRT
- PRESSURE Pa. kPa to Pa = x100,000
- VOLUME, M^3. 1m3= 1000dm3= 1000,000cm3
- NUMBER OF MOLES, pV= mass/mass 1 mole xRT
- R = 8.31 JK-1 mol
- N= PV/RT
- v= P/nRT
- T= pV/nR
- THE MOLAR VOLUME
- 1 mole of any gas occupies 22.4 dm3 at stp (standard temperature and pressure, taken as 0°C and 1 atmosphere pressure)
- value of 24.0 dm3 at room temperature and pressure (taken as about 20°C and 1 atmosphere).
- FINDING THE RELATIVE FORMULA MASS OF A GAS FROM ITS DENSITY
- You are given the atmospheric pressure in g per dm 3 and its temperature in Celsius
- The atmospheric pressure is the same as the weight, g.
- The temperature is always 293K
- Then put them into the equation pV= mass/mass 1 mole xRT
- KINETIC THEORY
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