Hello!
<span>The position of the equilibrium for a system where k = 4.6 × 10-15 can be described as being favored to the left; the concentration of products is relatively small.
For a reaction where A produces B, the chemical equation is the following:
A </span>⇄ B
The equilibrium constant expression is the following:
![k= \frac{[B]}{[A]}](https://tex.z-dn.net/?f=k%3D%20%5Cfrac%7B%5BB%5D%7D%7B%5BA%5D%7D%20)
From this equation, we can see that when the constant is small, as in the case of the exercise, the concentration of products is also small, and the equilibrium is favored to the left.
Have a nice day!
<span>The position of the equilibrium for a system where k = 4.6 × 10-15 can be described as being favored to the left; the concentration of products is relatively small.
For a reaction where A produces B, the chemical equation is the following:
A </span>⇄ B
The equilibrium constant expression is the following:
From this equation, we can see that when the constant is small, as in the case of the exercise, the concentration of products is also small, and the equilibrium is favored to the left.
Have a nice day!