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Question

4 g of an ideal gas was introduced into a bulb of volume of 0.821 dm3 at certain pressure, P and temperature T. The above bulb was placed in a thermostat maintained at temperature (T+125)K. 0.8 gm of the gas was leaked to keep the original pressure. Calculate the pressure in atm. [Molar mass of the gas is 40 gmol1 and R value is 0.0821 lit-atm-k1mol1]


Solution

Initial number of moles =440=0.1
Final number of moles =3.240=0.08
Since P and V are constant
n1T1=n2T2
0.1T1=0.08(T1+125)
T1=500 K
from PV=nRT
P=0.1×0.082×5000.821=5 atm

Chemistry

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