Write an equilibrium constant expression for the chemical reaction of ammonia with water. (In this reaction assume that the concentration of water will remain constant)
NH3 + H2O --> NH4^+ + OH^-
Keq = (NH4^+)(OH^-)/(NH3)
Well, let me tell you, writing equilibrium constant expressions is like being a wordsmith... but for chemistry! Here's how we can clownishly express it:
The equilibrium constant expression for the reaction of ammonia (NH₃) with water (H₂O) is as follows:
K(circus) = [NH₄⁺][OH⁻] / [NH₃]
Oh, look at that, we have some circus tricks going on! The concentration of the ammonium ion (NH₄⁺) and the hydroxide ion (OH⁻) are multiplied together, which gives us the numerator. Then, we divide it by the concentration of ammonia (NH₃) to get that marvelous denominator.
Remember, keep your concentration constant like a steadfast clown's smile, as we assume the concentration of water won't change in this reaction.
The chemical reaction between ammonia (NH3) and water (H2O) can be represented as:
NH3 + H2O ⇌ NH4+ + OH-
The equilibrium constant expression for this reaction is:
Kc = [NH4+][OH-]/[NH3]
In this expression, the brackets [ ] indicate the concentration of each species at equilibrium. The concentration of water is usually considered constant and is not included in the expression.
The equilibrium constant expression for a chemical reaction is a mathematical representation of the ratio of the concentrations of the products to the concentrations of the reactants at equilibrium. For the reaction between ammonia (NH3) and water (H2O) to form ammonium hydroxide (NH4OH), the balanced chemical equation is:
NH3 + H2O ⇌ NH4OH
Since the concentration of water remains constant, it is not included in the equilibrium expression. The equilibrium constant, denoted as K, is written as:
K = [NH4OH] / [NH3]
In this expression, the square brackets represent the concentration of the species. The numerator represents the concentration of the product, NH4OH, while the denominator represents the concentration of the reactant, NH3. Keep in mind that the concentrations used in the expression should be the equilibrium concentrations.
It's important to note that if the reaction is written in the reverse direction, the equilibrium constant expression would be the reciprocal of the original expression.