Asked by TJ
A mixture containing the same number of moles of SO2 and O2 is placed in a 2L container at 900K. The initial pressure is 1.90Atm. A reaction occurs leading to the formation of SO3: 2SO3 + O2 <--> 2SO3 After equilibrium is established the TOTAL pressure drops to 1.60 Atm. What is the equilibrium constant, Kp, at 900K?
Answers
Answered by
DrBob222
Equal moles means equal pressures; therefore, initial pressure SO2 = 0.95 atm and initial pressure O2 = 0.95 atm. (You can go through PV = nRT to confirm this if you wish.).
2SO2 + O2 ==> 2SO3
initial:
SO2 = 0.95
O2 = 0.95
SO3 = 0
change:
SO2 = -2x
O2 = -x
SO3 = +2x
equilibrium:
SO2 = 0.95-2x
O2 = 0.95-x
SO3 = 2x
total pressure = 1.6 = 0.95-2x+0.95-x+2x and solve for x. Substitute these into the above ICE chart to find individual concns, substitute into Ka expression and solve for Kp.
2SO2 + O2 ==> 2SO3
initial:
SO2 = 0.95
O2 = 0.95
SO3 = 0
change:
SO2 = -2x
O2 = -x
SO3 = +2x
equilibrium:
SO2 = 0.95-2x
O2 = 0.95-x
SO3 = 2x
total pressure = 1.6 = 0.95-2x+0.95-x+2x and solve for x. Substitute these into the above ICE chart to find individual concns, substitute into Ka expression and solve for Kp.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.