Recall the relationship between the equilibrium constant for a forward reaction and that for a reverse reaction. The equilibrium constant for the reverse reaction is the of the equilibrium constant for the forward reaction.

Reciprocal

Explanation:

To buttress the point we are driving at, let’s consider the following hypothetical chemical reaction.

A + B <——-> C + D

In the forward reaction, we can calculate the equilibrium constant as the following. Let’s represent this by Kf

Kf = [C][D]/[A][B]

For the backward reaction, that is A+B as reactant, giving C+D as product. Let’s represent the equilibrium constant for the backward reaction as Kb

Kb = [A][B]/[C][D]

What we see here is that if we multiply the values of the equilibrium constant for the forward reaction by the value of the equilibrium constant for the backward reaction, we get a value of 1. Hence, we can conclude that the value of the chemical equilibrium for the forward reaction is a reciprocal of the value of the chemical equilibrium for the backward reaction.

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation:

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.