The burning of ethane produces both CO2 and H2O. If 200 mL of CO2 is produced at 20°C and 750 torr, what volume of water vapor would be produced at 24°C and 790 torr?
C2H6 + O2 —> CO2 + H2O (need to balance)
Answer:
On balancing the equation yields :
C2H6 + (3.5)O2 ----> 2CO2+ 3H2O
So, the ratio of moles in the ratio are 2:3.
Use the ideal gas equation
PV = nRT
n = PV/RT
Thus, we have n directly proprtional to PV/T (as R is constant)
The number of moles of CO2 = (750*200/293*R)
The number of moles of H2O produced = 3/2*(750*200/293*R)
Use the universal gas equation again.
PV = nRT
V = nRT/P
V = 3/2*(750*200/293*R) * R * 297 / 790
V = 3*750*200*R*297/(2*293*790*R)
V = 288.6983 mL
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