Graham's law states that the gas with the smaller molar mass will effuse faster _____.?
You have a 2-liter bottle of soda. You empty the soda from the bottle and want to fill the bottle with nitrous oxide (N2O) at 20 degrees C and 1 atm. How many grams of N2O would you need
A.371
B.529
C.3.7
D.83
The temperature of a gas increases from 100 degrees C to 200 degrees C. The volume and number of moles remains the same. The pressure of the gas has increase by a factor of _____.
A.2
B.1.3
C.0.5
D.1.8
One balloon is filled with helium, and another balloon is filled with carbon monoxide (CO). Both gases have the same energy. If an identical hole is punched in each balloon, the ____ gas will effuse faster by a rate of _____
A.helium...2.6
B.carbon monoxide...2.6
C.helium...14
D.carbon monoxide...14
(1)
PV = nRT
(1 atm)(2 L) = n (0.08206 L atm / K mol)(293 K)
n = 0.0831 moles
n = grams N2O / molecular weight N2O
0.0831 = x / 44.013
x = 3.7 grams
Therefore, the answer is C.
(2)
At constant volume and number of moles:
P1 / T1 = P2 / T2
(P1 / T1) T2 = P2
(T2 / T1) P1 = P2
T2 / T1 = P2 / P1
473 K / 373 K = P2 / P1
P2 / P1 = 1.3
The pressure of the gas will increase by a factor of 1.3.
Therefore, the answer is B.
(3)
Graham's law:
r1 / r2 = √MW2 / √MW2
where r1 and r2 are the rates of effusion for the gases and MW1 and MW2 are their molecular weights.
r He / r CO = √MW2 / √MW2
r He / r CO = √28 / √4
r He / r CO = √7
r He / r CO = 2.6
The helium gas will effuse 2.6 times faster than the carbon monoxide gas.
Therefore, the answer is A.
Hope this helps...good luck!
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