Gases Flashcards
What is a gas
A gas is a substance that don not have well defined boundaries but diffuses rapidly to fill any container in which it is placed.
What is boyles law
At constant temperature the volume of fixed mass of gas is inversely proportional to its pressure.
What is Charles law
At constant pressure the volume of a fixed mass of gas is direct proportional to its temperature on the Kelvin scale.
What is guy lussac’s law of combining volumes
In a relation between gases the volumes of reacting gases and products are inversely proportional to the ratio of small whole numbers provided the volumes are measured at the same temperature and pressure.
What is avogadro’s law
Avogadro’s law states that equal volumes of gases contain equal numbers of molecules under the same conditions of temperature and pressure.
What are the assumptions of kinetic theory
- Gases are made of particles that are in continuous motion
- There are no attractive or repulsive forces between the molecules.
- Actual volume of gas negligible compared with the space the gas occupies.
- Collisions between the molecules are perfectly elastic
- The average kinetic energy of the molecules in a sample of gas is proportional to the temperature measured on the absolute scale.
The kinetic theory of gases was developed by who
James clerk maxwell and Ludwig Boltzmann
What are the limitations of kinetic energy.
- There are attractive and repulses forces between molecules.
- The volume of the molecules is not negligible compared with the space they occupy.
What is an ideal gas
Is one gas that obeys all the gas laws and under all conditions of temperature and pressure.
No such gases exit but real gases behave most like an I………….ga…….at h…….t……….and l………pr….
Ideal gas at high temperature and low pressure
Why do real gases deviate
Intermolecular forces are present ( such as dipole- dipole ), van dear waals)
Collisions are not perfectly elastic
What is the formula for ideal gas
PV=nRT
What does the letter in the formula stands for ?
P,V,n,R,T
P = pressure (Nm)
n= no. of moles
V = volume (m3)
T = temperature (k)
R = universal gas constant ( 8.31) [Nm mol -1 k-1]
To convert kPa to Pa
Multiply by 1000
To convert Celsius to kelvin
Add 273
To convert 1 liter to meter cube
Divide by 1000
To convert meter cube to litre
Multiply by 1000
To find moles formula
Moles = mass in grams / relative molecular mass of the compound
To convert centimetre cube to meter cube
Multiply by 10(-6)
