The equilibrium constant for the following reaction is 5.0 at 100c. If an equilibrium mixture contains [No2]=0.50 M, what is the [N2O4]?
2No2(g) <--> N2O4 (g)
I do not understand if the Kc is 100c or where that plays in!
keq= x/(.5)^2
x= .25*5=1.25moles/liter
Thank you!
Can you explain to me where the 0.25 comes from?
Did you look at the answer? What is (.5)2?
Sorry I had a moment! I didn't process before I typed!
That's ok. I do that too. Yesterday I TRIED to balance my check book. The trouble is my brain kept telling me the number was wrong but the computer said the number was right. It took two hours for me to convince my brain that the computer really was right all along.:-).
In this question, the given information is the equilibrium constant (Kc) for the reaction and the concentration of one of the species in the equilibrium mixture at a certain temperature of 100°C.
The equilibrium constant (Kc) is a measure of the extent to which a reaction reaches equilibrium. It tells us the ratio of the concentration of products to the concentration of reactants at equilibrium. In this case, the reaction is 2NO2(g) ⇌ N2O4(g), and the given Kc value is 5.0 at 100°C.
To find the concentration of N2O4 in the equilibrium mixture, you will use the equilibrium expression for the reaction:
Kc = [N2O4] / ([NO2]^2)
Where [N2O4] represents the concentration of N2O4 and [NO2] represents the concentration of NO2. The square brackets indicate concentrations measured in molarity (M).
Since you are given the concentration of NO2 in the equilibrium mixture as 0.50 M, you can substitute this value into the equilibrium expression:
5.0 = [N2O4] / (0.50^2)
Simplifying the equation:
5.0 = [N2O4] / 0.25
Multiply both sides of the equation by 0.25:
5.0 * 0.25 = [N2O4]
1.25 = [N2O4]
Therefore, the concentration of N2O4 in the equilibrium mixture is 1.25 M.