4NH3(g)+5O2(g) yield 4NO(g)+6H2O(g)

Kc = (NO)^4(H2O)^6/(NH3)^4(O2)^5

What happens to Kc if the equation is multiplied by 2

The equilibrium constant expression for the reaction is determined by the concentrations of the products and the reactants at equilibrium.

In this case, the reaction is:

4NH3(g) + 5O2(g) ⇌ 4NO(g) + 6H2O(g)

The equilibrium constant expression is written as:

Kc = [NO]^4 [H2O]^6 / [NH3]^4 [O2]^5

Where [NO] represents the concentration of NO gas, [H2O] represents the concentration of H2O gas, [NH3] represents the concentration of NH3 gas, and [O2] represents the concentration of O2 gas. The exponents of the concentrations in the equilibrium constant expression are determined by the stoichiometric coefficients of the balanced chemical equation.

To deduce the equilibrium constant expression for the given reaction, we first need to understand the general format for writing equilibrium constant expressions.

The equilibrium constant expression for a chemical reaction is written using the concentrations (or partial pressures) of the reactants and products at equilibrium. It is denoted as K, followed by the equation for the reaction.

In the equation provided: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g), the stoichiometric coefficients represent the number of moles involved in the reaction. These coefficients are used to determine the powers to which the concentration terms are raised in the equilibrium constant expression.

Let's assume the equilibrium constant expression for this reaction is Kc. We can express it as follows:

Kc = [NO]^4 [H2O]^6 / [NH3]^4 [O2]^5

Here, the square brackets [ ] represent the concentration of each species in moles per liter (Molarity) at equilibrium. The stoichiometric coefficients are used as exponents to indicate the number of moles of each species involved in the reaction.

Therefore, the equilibrium constant expression for the given reaction is Kc = [NO]^4 [H2O]^6 / [NH3]^4 [O2]^5.