Question
A vessel of volume V = 5 litre contains 1.4gm of N2 at temperature 1800K. If at this high temperature, 30% of the gas dissociates into atoms, then find the pressure of gas.
Solution
Given,
Volume of the vessel, V = 5
Molecular weight of nitrogen = 28 g
Temperature, T = 1800 K
Number of moles in 1.4 gm of N2 is,
Volume of the vessel, V = 5
Molecular weight of nitrogen = 28 g
Temperature, T = 1800 K
Number of moles in 1.4 gm of N2 is,
Also, given that at high temperature 30% of the gas dissociates into atoms.
Number of moles of gas dissociated into atoms is,
Number of moles of atomic nitrogen is,
Number of moles of molecular nitrogen is,
Thus total number of moles of nitrogen gas is given by n = n1 + n2 = 0.065 moles
Now, using the ideal gas equation,
PV = nRT
We have, n = 0.065
T = 1800 K
V = 5 litre = 5 m3
Therefore,
Number of moles of atomic nitrogen is,
Number of moles of molecular nitrogen is,
Thus total number of moles of nitrogen gas is given by n = n1 + n2 = 0.065 moles
Now, using the ideal gas equation,
PV = nRT
We have, n = 0.065
T = 1800 K
V = 5 litre = 5 m3
Therefore,
