A mixture of SO3,SO2 and O2 gases is maintained in 10litre flask at which the Kc for reaction is 100 . If number of moles of SO2 and SO3 are equal then how many moles of O2 present.
0.1
To solve this problem, we'll first set up the balanced chemical equation for the reaction:
2SO2 + O2 ⇌ 2SO3
Let's assume that the initial number of moles of both SO2 and SO3 is x. Therefore, the initial number of moles of O2 can be represented as y.
At equilibrium, we can use the equation Kc = [SO3]^2 / ([SO2]^2 * [O2]), where [A] represents the concentration of substance A.
Since the number of moles of both SO2 and SO3 is x at the start, their concentrations will be equal to their respective number of moles divided by the volume of the flask:
[SO2] = [SO3] = x / 10
Using the given value of Kc = 100, we can plug in the concentrations to the equilibrium expression:
100 = ([SO3]^2) / ([SO2]^2 * [O2])
Substituting the concentrations, we get:
100 = (x/10)^2 / ((x/10)^2 * y)
Simplifying the equation, we have:
100 = 1 / y
Cross-multiplying, we find:
y = 1/100
Therefore, the number of moles of O2 present is 1/100.
The Kc is 100 for what reaction? Is it
2SO3 ==> 2SO2 + O2 or the reverse?