A vessel of volume 8.0x10-3 m3 contains an ideal gas at 300K and 200kPa. The gas is allowed to leak till pressure falls to 125kPa the amount of the gas (in moles) leaked assuming tht the temp remains constant is ?????
1.0 litre of N2 and 7/8 litre of O2 at the same temperrature and pressre were mixed together. what is the relation b/w the masses of the two gases in the mixture ????
A mixture of two gases A and B in the mole ratio 2:3 is kept in a 2 litre vessel. A second 3 ltre vessel has the same two gases in the mole ratio 3:5 . both gas mixtures has the same temp and the same total presurre . they r allowed to intermix and the final temp and the total presure are the same as the initial values , the final volume bieng 5 litres . given tht the molar masses are MA and MB the mean molar mass of the final mixture is ????
the vol of the H2gas effuses through a hole in a container in 5 seconds. the time taken fr the effusion of the same volume ofthe specified gas under identical conditions is ?????
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We know that PV=nRT
= PV/RT =n
So from given values we have
P = 200 kPa
V= 8.0x10-3 m3 = 0.008
R = 8.314
T = 300K
Therefore n = 200 x 0.008/ 8.314 x 300
= 6.414 x 10-4 ----- initial no. of moles ---(A)
Now we as the pressure has dropped to 125 kPa but all other parameters are constant
n = 125 x 0.008/ 8.314 x 300
n = 4 x 10-4 ----- volume after leak ---(B)
Amount of gas leaked is A-B = 2.414 x 10-4