For the reaction, 2 SO2(g) + O2(g) == 2 SO3(g), at 450.0 K (Kelvin) the equilibrium constant, Kc, has a value of 4.62. A system was charged to give these initial concentrations, (SO3) = 0.254 M and (O2) = 0.00855 M, and (SO2) = 0.500 M. In which direction will it go?
I think I posted this once before but I do not remember what the respond was. Am I suppose to plug the values into the Kc equation?
4.62 = (0.245)^2 / (0.500)^2 (0.00855)
just copy and paste your question into google and the exact same question pops up on the first link. the post you posted before is the 3rd link down.
To determine the direction in which the reaction will proceed, you need to compare the calculated Qc (reaction quotient) with the given Kc (equilibrium constant).
The reaction quotient, Qc, is calculated using the concentrations of the compounds in the reaction at a given moment, in the same way as the equilibrium constant, Kc.
To calculate Qc, you would use the equation:
Qc = (concentration of SO3)^2 / [(concentration of SO2)^2 * (concentration of O2)]
Now, you have the values you need to calculate Qc:
(concentration of SO3) = 0.254 M
(concentration of SO2) = 0.500 M
(concentration of O2) = 0.00855 M
Plugging these values into the equation, you get:
Qc = (0.254)^2 / [(0.500)^2 * (0.00855)]
Simplifying the equation:
Qc ≈ 1.874
Next, compare the calculated Qc value with the given Kc value:
If Qc < Kc:
This means the reaction has not yet reached equilibrium, and the reaction will proceed in the forward direction to reach equilibrium. In this case, the forward reaction will form more products.
If Qc > Kc:
This means the reaction has passed equilibrium and there is an excess of products. The reaction will proceed in the reverse direction to reach equilibrium, forming more reactants.
If Qc = Kc:
This means the reaction is at equilibrium, and there will be no net change in the concentrations of the reactants and products.
In your case, the calculated Qc is approximately 1.874, while the given Kc is 4.62. Since Qc < Kc, it indicates that the reaction has not yet reached equilibrium. Therefore, the reaction will proceed in the forward direction, forming more products.