Question

How will the following stresses affect this equilibrium system (iron thiocyanate system): Fe+3 {pale yellow} + SCN- FeSCN+2 {red} + heatA) Add KSCN (a source of adding SCN- ions in solution)?

Answer 1

The addition of KSCN to the system will shift the arrow to the product sides

Step-by-step explanation

Firstly, we need to define the term chemical equilibrium.

Chemical equilibrium can be defined as the state in which the reactants and the products are present in concentration and do not have a tendency to change with time.

To determine the shift of the chemical equilibrium in the reaction provided, state the le Chatelier's principle

Le Chatelier's principle states that when external constraints such as temperature, pressure, concentration, etc system in chemical equilibrium, the equilibrium arrow shifts so as to annul the effect of the external constraints.

From the reaction provided

`\text{ Fe}^(+3)\text{ + SCN}^-\text{ }\rightleftarrows\text{ FeSCN}^(+2)\text{ + heat}`

The above equation shows that the reaction is an exothermic reaction because heat is liberated to the surroundings.

When one of the reactants is supplied to the system constantly, more of its product is formed. Hence, the equilibrium arrow shifts to the right-hand side of the reaction.

Hence, the addition of KSCN to the system will shifts the arrow to the product sides