NH4HS(s) <-> NH3(g) + H2S(g)
An equilibrium mixture of this reaction at a certain temperature was found to have (NH3)=.268 and (H2S)=.360
What is the value of the equilibrium constant at this temperature?
Two questions.
1. What units?
2. Why aren't the two values the same?
To find the value of the equilibrium constant (K) at a given temperature, we need to use the expression of equilibrium constant based on the concentrations of the reactants and products.
The equation for the reaction is:
NH4HS(s) ⇌ NH3(g) + H2S(g)
The equilibrium constant expression for this reaction is:
K = ([NH3] * [H2S]) / [NH4HS]
We are given the concentrations of NH3 and H2S, but not the concentration of NH4HS. However, since NH4HS is a solid, its concentration remains constant and is not included in the equilibrium constant expression. Thus, we can assume its concentration is 1.
Plugging in the given values:
[NH3] = 0.268
[H2S] = 0.360
[NH4HS] = 1
K = (0.268 * 0.360) / 1
K = 0.09648
Therefore, the value of the equilibrium constant (K) at this temperature is approximately 0.09648.