Answer:
relative rate of diffusion is 1.05
Explanation:
According to Graham's law of difussion:
Rate of diffusion is inversely proportional to the square root of molecular weight of a molecule.
For two given molecules:
The given molecules are
Water = 18.01
Heavy water =20.03
Thus the relative rate of diffusion will be:
Answer:
the average molar mass of this air sample can be calculated as
addition of the product of the average molar weights of the component gases and their percentage compositions
1. Average Molar mass of Air = 0.7803 x 28 + 0.2099 x 32 + 0.00033 x 44 = 28.58g/mol
2. The partial pressures of N2, O2, and CO2 in atm.
From Ideal gas law, at stp, Volume of air V=22.4L/mol
PV =nRT
Since, at constant temperature and pressure, the volume of a gas is directly proportional to the number of moles of the gas
Total Pressure P=1atm
Partial Pressure p = mol fraction x P
Volume of N2 = 0.7803 x 22.4L = 17.47L, Partial Pressure = 0.7803atm
Volume of O2 = 0.2099 x 22.4L = 4.68L Partial Pressure = 0.209atm
Volume of CO2 = 0.00033 x 22.4L = 0.00739L, Partial Pressure = 0.033atm
Hydrogen bonds are approximately 5% of the bond strength of covalent C-C or C-H bonds.
Hydrogen bonds strength in water is approximately 20 kJ/mol, strenght of carbon-carbon bond is approximately 350 kJ/mol and strengh of carbon-hydrogen bond is approximately 340 kJ/mol.
20 kJ/350 kJ = 0,057 = 5,7 %.
