An evacuated bulb of unknown volume is filled with a sample of H2 gas at a temperature T. The pressure of the gas in the bulb is 756 mm Hg. A portion of the H2 gas is transferred to a different flask and found to occupy a volume of 40.0 mL at 1.00 atm and the same temperature T. The pressure of the H2 gas remaining in the original bulb drops to 625 mm Hg at the same temperature T. Assuming H2 is an ideal gas, what is the volume of the bulb?
Asked by aditipodaralla
8th July 2018,
11:13 AM
Answered by Expert
Answer:
For ideal gas, equation of state is given by , p×v = n×R×T , where p is pressure,
v is volume occupied by n moles of gas, R is gas constant and T is Temperature in kelvin.
Let V be the volume of bulb and n1 moles are there initially, then we have the initial state equation as,
756×V = n1×R×T ....................(1)
let n2 moles are transferred to flask,then we have
760×40 = n2×R×T ......................(2)
now we have remaining (n1-n2) moles in the bulb at presuure 625 mm of Hg.
hence we have, 625×V = (n1-n2)×R×T = n1×R×T - n2×R×T .............(3)
by substituting for n1×R×T from (1) and for n2×R×T from (2) in eqn.(3), we can solve the eqn.(3) to get V = 232 mL
Answered by Expert
8th July 2018,
1:00 PM
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