Answer:
[R] = [Z] > Q
Explanation:
Given the equilibrium:
X(g) + 2 Q(g) ⇄ R(g) + Z(g)
The equilibrium constant will be given by:
Kc = 1.3 x 105 at 50ºC = [R] x [Z] / ( [X] x [Q]² )
This value is telling us that at equilibrium the products quantities will be much higher than the reactants.
Looking at the answer choices we see that (a) is false since this is an equilibrium not a areaction that goes to completion;(b) is is false because again this is an equilibrium and it would also imply that Kc is one; (c) is false because in the reaction the ratio is 1X : 2Q.
The last choice is the true statement since the equilibrium constant favors the products. This statement would haven true if Kc had been much less than one.
The concentration of the products are greater than the concentration of the reactants.
The correct answer to the question is [R] = [Z] > Q
Equilibrium constant, K is simply defined as the ratio of the concentration of the products raised to their coefficients to the concentration of the reactants raised to their coefficients.
We can write the equilibrium constant for the reaction as follow:
X(g) + 2Q(g) ⇄ R(g) + Z(g)
K = [R][Z] / [X] [Q]²
From the question given above, we were told that the equilibrium constant has a value of 1.3×10⁵ i.e
K = [R][Z] / [X] [Q]²
1.3×10⁵ = [R][Z] / [X] [Q]²
From the above, we can see that the equilibrium constant has a higher value. This simply means that the concentration of the products is greater than the concentration of the reactants at equilibrium.
Thus, correct answer to the question is:
[R] = [Z] > Q
Learn more about equilibrium constant:
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