Numbericals:
1.
A mixture of Helium and Hydrogen
is confined in a 12dm3 flask at 30oC if 0.2 mole of the
Helium is present. Find out the partial pressure of each gas where the pressure
of mixture of gases is 2atm.
2. The
volume of the Oxygen gas collected over water at 24oC and 762 torr
(mm of Hg)
pressure
is 128 ml volume. Calculate the mass Oxygen gas
3.
13.2g of gass occupies a volume of
0.918dm3 at 25oC and 8atm pressure. Calculate the
molecular mass of the gas
4. 400cm3 of Helium gas take to
effuses from a porous container in 20 second. How long will be SO2
gas take to effuses from same container?
5.
A quantity of gas measure 500ml at
35oC and 600mm (Hg).
What would be the volume of the as at
45oC and 800mm (Hg)?
6
. 1.4dm3 volume of gas
measure at temperature of 27oC. and pressure 900 torr was
found to a mass
of gas 2.273g. Calculate the molecular mass of gas.
Three
container of equal volume are filled as follows.
a)2 mole of H2 gas at 0oC
b)1 mole of N2 gas at 273
K c) 3 mole of O2 gas at 27oC
7.
Calculate the molecular mass of a
gas whose rate of diffuse in twice of that of CH4
8. 380 cm3 of hydrogen gas was
collected over water at 23oC and 613 torr: find the volume of dry
hydrogen at S.T.P. (vapour pressure of water at 23oC is 21 torr.)
9. What is the volume of 2.5 mole of N2 gas at S.T.P.?
10. State the Dalton’s law of partial
pressure. A mixture of .2 mole of gas “A” and 1.1 gm of anther gas “”B” (mol.
Mass = 44) exerts a pressure of 750 torr: calculate the partial pressure of the
two gases.
11. A 500cm3 vessel contains H2
gas at 400 torr and another 1.0dm# Vessel contains O2
gas at 600 torr. If these gases are transferred to 2dm3 empty
vessel, calculate the total pressure of the mixture of the gases.
12. A given mass of a gas occupies 76 cm3
at 16oC and 760 torr pressure; calculate its volume at S.T.P.
13. A 100 cm3 gas, cylinder
filled with chlorine under 160 torr pressure is connected by stop-cock with another cylinder of 400
cm3 filled with nitrogen under pressure of 200 torr. What will be the total pressure
when stop cock is opened?
A mixture 2.0 mole of a gas "A" and 1.1gm of gas "B" (mole mass=44) exerts a pressure of 750 torr; calculate the partial pressure of two gases
ReplyDelete(can anyone solve this?)
mole of =1.1g/44g/mol=0.025 mol
Deletetotal mole of mixture =2.0+0.025=2.025mol
Partial pressure of A = Total pressure x mole of Gas A /total mole of mixture
= 750 x 2.0 /2.025
=740.7 torr
Total Pressure =Partial pressure Gas A +Partial pressure of
Gas B
750 torr = 740.7 torr + Partial pressure of Gas B