Explanation:

Units of KP and KC:

The equilibrium constant, KP, is used to express the equilibrium constant in terms of partial pressures of the reactants and products. The units of KP are typically expressed in atmospheres (atm) or pascals (Pa).

On the other hand, the equilibrium constant, KC, is used to express the equilibrium constant in terms of the molar concentrations of the reactants and products. The units of KC are typically expressed in moles per liter (mol/L) or molar (M).

Why the statement is false:

The statement "The units of KP and KC are equal" is false. KP and KC have different units because they are based on different properties - partial pressures and molar concentrations.

Example:

Let's consider the reaction:

A(g) + B(g) ⇌ C(g)

The equilibrium constant for this reaction can be expressed as KP or KC.

If we express the equilibrium constant as KP, it would be:

KP = (PC / P A * P B)

where PC, PA, and PB are the partial pressures of C, A, and B, respectively.

If we express the equilibrium constant as KC, it would be:

KC = (C / [A] * [B])

where C, [A], and [B] are the molar concentrations of C, A, and B, respectively.

Conclusion:

In conclusion, KP and KC have different units because they are based on different properties - partial pressures and molar concentrations. Therefore, the statement "The units of KP and KC are equal" is false.