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A gas mixture contains HBr, NO2, and C2H6 at STP
A gas mixture contains HBr, NO2, and C2H6 at STP.
If a tiny hole is made in the container, which gas will effuse fastest?
Which gas molecules have the highest average kinetic energy at this temperature?
Expert Solution
1)Rate of effusion is inversely proportional to square root of molar mass
rate = k*sqrt(1/M)
M is molar mass
Rate of effusion is inversely proportional to square root of molar mass
rate = k*sqrt(1/M)
M is molar mass
the one with lower molar mass will have higher rate of effusions
Lets list out molar mass of all given compounds
Molar mass of HBr = 80.908
Molar mass of NO2 = 46.01
Molar mass of C2H6 = 30.07
Increasing order of molar mass is:
C2H6
NO2
HBr
Same is the order of decreasing rate
From fastest to slowest
C2H6
NO2
HBr
Answer: C2H6
2)Kinetic energy depends on temperature.
At same temperature, all the mentioned gases will have same kinetic energy
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