Question

A gaseous mixture of 1.0 mol of 12 and 1.0 mol of H2 was placed in an empty vessel that has a
volume of 2.0 L. The system was allowed to reach dynamic equilibrium at 300°C.
a) State briefly what happened to the initial concentration of 12 and H2 as the reaction reaches
equilibrium
b) Does the reaction stoop at equilibrium? Why?​

Answer 1

Answer:

See detailed explanation.

Explanation:

Hello!

In this case, for the reaction:

$I_2+H_2\rightleftharpoons 2HI$

It is known that the equilibrium constant tends to be greater than 1; therefore, it is a reaction that tends to go rightwards towards the formation of hydrogen iodide.

a) Here, since the reaction tends to form the product, it is clear that the initial concentration of iodine and hydrogen will decrease as the reaction reaches equilibrium in order to increase the concentration of hydrogen iodide.

b) Yes, it stops at the point in which the following expression:

$\frac{[HI]^2}{[I_2][H_2]}$

Equals the equilibrium constant.

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