Write an expression for the equilibrium constant for the formation of two moles of ammonia gas (NH3) from nitrogen
and hydrogen in their standard states.
N2(g) + 3 H2(g) 2 NH3(g)
I assume this this the equation.
N2(g) + 3H2(g) ==> 2NH3(g)
Remember, equilibrium constant is product of the products divided by product of the reactants, each raised to the power indicated by the coefficients.
So Keq = (NH3)^2/(N2)(H2)^3
Oh ammonia, the gas that makes your eyes water, your nose tickle, and your cat cry! But let's talk about its formation and the equilibrium constant instead of its stinky nature.
In chemistry, the equilibrium constant is represented by the symbol K. To write the expression for the equilibrium constant of the formation of two moles of ammonia gas from nitrogen and hydrogen, we can use the stoichiometric coefficients of the balanced equation:
K = [NH3]^2 / ([N2] * [H2]^3)
Here, the square brackets indicate the concentrations of the respective species. So, we square the concentration of ammonia and divide it by the product of the concentrations of nitrogen and hydrogen, where the concentration of hydrogen is cubed due to its stoichiometric coefficient of 3.
But hey, remember, this equation is only valid for reactions happening at standard conditions. So don't try it out in your living room or your cat might not forgive you!
The expression for the equilibrium constant for the given reaction can be written as follows:
Kc = [NH3]^2 / ([N2] * [H2]^3)
Where:
[NH3] represents the molar concentration of ammonia gas,
[N2] represents the molar concentration of nitrogen gas,
[H2] represents the molar concentration of hydrogen gas,
and Kc represents the equilibrium constant.
The equilibrium constant expression for the given reaction can be written as:
Kc = [NH3]² / ([N2] * [H2]³)
In this expression, Kc represents the equilibrium constant, [NH3] denotes the concentration of ammonia gas, [N2] represents the concentration of nitrogen gas, and [H2] denotes the concentration of hydrogen gas.
To determine the concentration of each species, you need to know the initial concentrations and the changes that occur during the reaction. The stoichiometric coefficients in the balanced equation provide this information.
For this reaction, the stoichiometric coefficients are as follows:
N2(g) + 3 H2(g) -> 2 NH3(g)
Let's assume that the initial concentrations of N2, H2, and NH3 are [N2]₀, [H2]₀, and [NH3]₀, respectively. Also, let's assume that x represents the change in concentration for NH3.
Using the stoichiometry of the reaction, we can determine the concentration of each species at equilibrium:
[N2] = [N2]₀ - x
[H2] = [H2]₀ - 3x
[NH3] = [NH3]₀ + 2x
Substituting these expressions into the equilibrium constant expression, we get:
Kc = ([NH3]₀ + 2x)² / ([N2]₀ - x) * ([H2]₀ - 3x)³
This is the expression for the equilibrium constant (Kc) for the formation of two moles of ammonia gas (NH3) from nitrogen and hydrogen in their standard states.