The initial pressure for the compounds involved in the reaction displayed were determined to be P(SO2(g)) = 0.5932 atm, P(O2(g)) = 0.4886 atm, P(SO3(g)) = 0.09287 atm. Calculate the value of the equilibrium constant (Kp) at 1000 K if the equilibrium pressure of O2(g) was 0.4924 atm.
2SO2(g)+O2(g) = 2SO3(g)
so you said that SO3 is decreased by 2*.0038, O2 is increased by .0038 but shouldnt SO2 increased by 2x.0038 since it has 2 moles
(.08527)^2/(.4924x.6008^2)
Of course. 0.6008 is correct for pSO2. If I didn't type in the 2 it was a miscue on my part. What you have looks ok to me.
To calculate the value of the equilibrium constant (Kp) for the given reaction, we first need to determine the equilibrium pressures of all the compounds involved in the reaction. We are given the initial pressures, which are:
P(SO2(g)) = 0.5932 atm
P(O2(g)) = 0.4886 atm
P(SO3(g)) = 0.09287 atm
We are also given the equilibrium pressure of O2(g), which is 0.4924 atm. Based on the stoichiometry of the reaction, we can determine the changes in pressure for each compound:
2SO2(g) + O2(g) -> 2SO3(g)
For O2(g), its pressure increased by (equilibrium pressure - initial pressure) = 0.4924 atm - 0.4886 atm = 0.0038 atm.
For SO2(g), its pressure changed by (2 × change in O2 pressure) = 2 × 0.0038 atm = 0.0076 atm, because there are two moles of SO2 in the balanced equation.
For SO3(g), its pressure decreased by (2 × change in O2 pressure) = 2 × 0.0038 atm = 0.0076 atm, because there are two moles of SO3 in the balanced equation.
Now, we can calculate the equilibrium pressures of SO2(g), O2(g), and SO3(g):
Equilibrium pressure of SO2(g) = Initial pressure of SO2(g) + Change in SO2 pressure
= 0.5932 atm + 0.0076 atm
= 0.6008 atm
Equilibrium pressure of O2(g) = Initial pressure of O2(g) + Change in O2 pressure
= 0.4886 atm + 0.0038 atm
= 0.4924 atm
Equilibrium pressure of SO3(g) = Initial pressure of SO3(g) - Change in SO3 pressure
= 0.09287 atm - 0.0076 atm
= 0.08527 atm
Finally, we can calculate the value of the equilibrium constant (Kp) using the equilibrium pressures:
Kp = (P(SO3(g)))^2 / (P(SO2(g)))^2 × (P(O2(g)))
= (0.08527 atm)^2 / (0.6008 atm)^2 × (0.4924 atm)
= 0.001169 / 0.21749
≈ 0.005374
So, the value of the equilibrium constant (Kp) at 1000 K is approximately 0.005374.
Note: Make sure to double-check the calculations and data provided to ensure accuracy.