If the reaction SO2(g) +0.5O2(g) <-> SO3(g) has the equilibrium constant Kc =56, then what is the Kc value for the following reaction?
2SO3 (g) <-> 2SO2 (g) + O2(g)
A. -112
B. 3.2 * 10^-4
C. 56
D. 8.9*10^-3
I think the answer would be C because the amount of reactants and products are equal and so the equilibrium constant should be the same. Can someone verify the answer please.
No, C is not correct for two reasons.
First, the reaction in the question is the reverse of that shown.
Second, the coefficients are different
Therefore you must make two corrections to the Kc = 56.
To correct for the fact that it is reversed the new Kc will be 1/Kc or 1/56.
Then to that you correct for the fact that the coefficients are twice the original you square that so the final answer is (1/56)^2. I'm guessing that will be B/
And to Double Pi if you're reading this, I should like to suggest that you cool it. If you don't answer a question we will know you don't know the answer. And for many of the ones you have answered you have done so incorrectly. So, to keep from cluttering the board with useless information, please refrain from answering unless you are positive you know the answer. Thank you.
You are correct. The equilibrium constant (Kc) for a reaction is determined by the ratio of the concentrations of the products to the concentrations of the reactants at equilibrium. In the given reaction, 2SO3 (g) <-> 2SO2 (g) + O2(g), the number of moles of reactants and products is the same, which means the equilibrium constant would be the same as the given reaction.
Therefore, the Kc value for the reaction 2SO3 (g) <-> 2SO2 (g) + O2(g) is also 56. Hence, the answer is C.
To find the equilibrium constant for the given reaction, you can use the fact that the equilibrium constant for a reverse reaction is the reciprocal of the equilibrium constant for the forward reaction.
For the given reaction: 2SO3 (g) <-> 2SO2 (g) + O2(g)
Since this reaction is the reverse of the reaction given in the question, the equilibrium constant for the given reaction will be the reciprocal of the equilibrium constant of the given reaction.
Given: Kc = 56
Therefore, the equilibrium constant for the given reaction will be 1/56.
Now, let's compare this value with the options provided:
A. -112: This value is the negative of the given equilibrium constant, so it is incorrect.
B. 3.2 * 10^-4: This value is not equal to 1/56, so it is incorrect.
C. 56: This value is the same as the given equilibrium constant, so it is incorrect since we are looking for the equilibrium constant of the reverse reaction.
D. 8.9*10^-3: This value is not equal to 1/56, so it is incorrect.
After evaluating all the options, the correct answer is not among the provided options. Therefore, none of the options are correct in this case.