An atmospheric chemist studying the pollutant SO2 places a mixture of SO2 and O2 in a3.03 L container at 885.2 K and 2.65 atm. When the reaction occurs, gaseous SO3 forms, and the pressure falls to 1.17 atm. How many moles of SO3 form?
Answer:
Given,
To determine the SO3 moles
Let us consider the reaction which is given as follows
2SO3 + O2 ----> 2 SO3 gaseous form
From the reaction we can say that,
2 moles of SO2 reacts with one mole of oxygen to give 2 moles of SO2. that is 2 moles of SO2 produces 2 moles of SO3.
Now,
2SO3 + O2 ----> 2 SO3
initial moles x y 0 Total moles = (x+y)
after reaaction 0 y-x x total moles = y
Thus before reaction occurs,
Consider,
PV = nRT
So number of moles (n) = PV/RT
Substitute the known values in above formula
n = 2.65 atmx3.03L/( 0.0821L.atmx 885.2K)
n = 0.110485 moles
After reaction,
Here now P = 1.17 atm
number of moles n = PV/RT = 1.17atmx 3.03L / 0.0821 x 885.2
= 0.04878 moles
Now,
y= 0.04878 &
x + y = 0.110485 moles
Hence,
Moles of SO2 reacted = moles of SO3 formed = 0.110485 - 0.04878
Therefor moles of SO3 formed = 0.061705 moles
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