I got kc to be 0 but that has got be wrong

You're right, it's probably wrong. If you will post the problem and your work I'll find the trouble.

I see your post below.

To understand why the value of kc (or any other equilibrium constant) being zero might be incorrect, let's first review the concept of equilibrium.

In chemistry, equilibrium represents a state at which the rate of the forward reaction is equal to the rate of the reverse reaction. The equilibrium constant, kc, is a numerical value that quantifies the concentrations of reactants and products at equilibrium.

If kc is zero, it implies that the concentration of the products at equilibrium is zero, while the reactants' concentration may or may not be zero. This scenario suggests that the forward reaction does not occur at all or has an extremely low rate.

However, it is important to note that such occurrences are highly unlikely in practical chemical systems, as most reactions do not completely halt or have zero product concentration at equilibrium. Reactions usually have small, nonzero equilibrium constants, indicating that both the forward and reverse reactions are present to some extent.

If you have obtained a value of kc equal to zero, it is advisable to reevaluate your calculations or reassess the conditions of the reaction to ensure accuracy. Double-check the stoichiometry and concentration values used in the equilibrium expression and make sure you are considering all relevant species in the equilibrium equation.

If necessary, consult reliable sources, such as textbooks or credible online resources, to confirm the expected value or range for the equilibrium constant for the reaction you are studying.