Answer:
Explanation:
Hello!
In this case, since the given reaction is:
Whereas the equilibrium constant is:
![K=\frac{[C][D]^{5/2}}{[A][B]^2} =4.0](https://tex.z-dn.net/?f=K%3D%5Cfrac%7B%5BC%5D%5BD%5D%5E%7B5%2F2%7D%7D%7B%5BA%5D%5BB%5D%5E2%7D%20%3D4.0)
However, the new target reaction reverses and doubles the initial reaction to obtain:
Whereas the equilibrium constant is:
![K'=\frac{[A]^2[B]^4}{[C]^2[D]^5}](https://tex.z-dn.net/?f=K%27%3D%5Cfrac%7B%5BA%5D%5E2%5BB%5D%5E4%7D%7B%5BC%5D%5E2%5BD%5D%5E5%7D)
Which suggest the following relationship between the equilibrium constants:
So we plug in to obtain:
Best regards!
The correct response is A. The inner she'll contains 2 electrons and the outer shell contains 4 electrons.
D. The reaction occurring in the forward direction is favored.
<span>In a reversible reaction, both the forward and reverse reactions take place (at equilibrium) </span>
<span>A. at the same rate </span>
<span>Which of the following is untrue concerning a reversible reaction? (at equilibrium) </span>
<span>D. The reaction could spend more time in the reverse direction than in the forward direction. </span>
<span>A reversible reaction </span>
<span>C. always starts off in the forward direction. </span>
<span>All reversible reactions will reach chemical _____. </span>
<span>D. equilibrium</span>
