Calculate The Equilibrium Constant for The Following Reaction Fe Ni

What is an equilibrium constant?

The equilibrium constant (K_eq) is a numerical value that describes the position of a chemical equilibrium. For a general reaction:

The equilibrium constant is defined as:

Where [A], [B], [C], and [D] represent the molar concentrations of the reactants and products at equilibrium. The value of K_eq indicates the extent to which the reaction favors products or reactants.

How to calculate the equilibrium constant

To calculate the equilibrium constant for the reaction Fe + Ni ⇌ FeNi, you'll need to know the concentrations of all species at equilibrium. The calculation involves:

1. Determining the stoichiometry of the reaction
2. Measuring or estimating the concentrations of all species at equilibrium
3. Applying the equilibrium constant expression

The equilibrium constant for this reaction is typically expressed as:

Where [FeNi] is the concentration of the formed intermetallic compound, and [Fe] and [Ni] are the concentrations of the reactants.

Example calculation

Let's consider an example where we have 0.1 M Fe and 0.1 M Ni initially, and after reaching equilibrium, we find:

• Final [Fe] = 0.05 M
• Final [Ni] = 0.05 M
• Final [FeNi] = 0.05 M

Using the equilibrium constant expression:

This means the reaction strongly favors the formation of FeNi at equilibrium.

Interpreting the equilibrium constant

The value of K_eq tells you about the reaction's equilibrium position:

• K_eq > 1: The reaction favors products
• K_eq = 1: The reaction is at equilibrium with equal concentrations of reactants and products
• K_eq < 1: The reaction favors reactants

For the Fe-Ni reaction, a high K_eq value indicates that the intermetallic compound FeNi is stable and forms readily from its elements.