The apparatus shown consists of two glass bulbs connected by a tap which is clos
ID: 852434 • Letter: T
Question
The apparatus shown consists of two glass bulbs connected by a tap which is closed.
In the first bulb, volume 3.0 L, there is a sample of pure oxygen at 3.0 atm. In the second bulb, volume 2.0 L, there is a sample of pure nitrous oxide at a pressure of 5.0 atm. Maintaining a constant temperature throughout, the tap is opened, the gases are allowed to mix, and they react to produce nitrogen dioxide according to the equation written below. Assume that the reaction goes as far as possible to completion:
2 N2O (g) + 3 O2 (g) ? 4 NO2 (g)
At the end of the reaction, what is the partial pressure of NO2 and what is the total pressure in the apparatus? (Hint: Determine which gas is the limiting reactant first. You do not need to replace R and T with specific numbers; you can leave expression RT in each calculation step, if necessary.) Show detailed work to receive credit.
The apparatus shown consists of two glass bulbs connected by a tap which is closed. In the first bulb, volume 3.0 L, there is a sample of pure oxygen at 3.0 atm. In the second bulb, volume 2.0 L, there is a sample of pure nitrous oxide at a pressure of 5.0 atm. Maintaining a constant temperature throughout, the tap is opened, the gases are allowed to mix, and they react to produce nitrogen dioxide according to the equation written below. Assume that the reaction goes as far as possible to completion: 2 N2O (g) + 3 O2 (g) ? 4 NO2 (g) At the end of the reaction, what is the partial pressure of NO2 and what is the total pressure in the apparatus? (Hint: Determine which gas is the limiting reactant first. You do not need to replace R and T with specific numbers; you can leave expression RT in each calculation step, if necessary.) Show detailed work to receive credit.Explanation / Answer
P1V1/RT+P2V2/RT=(V1+V2)P/RT
3X3+2X5=(3+2)P
19=5P
P=3.8atm
number of moles of NO2 formed according to stoichiometry =2 X number of moles of N2O
=2X(9/RT)
mole fraction of NO2= number of moles of NO2/total number of moles
=(18/RT)/(19/RT)=0.947
partial pressure of NO2=0.947xP
=0.947X3.8
=3.6 atm
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