A vessel initially contains pure A at a pressure of 1.0 bar. The total pressure of all gases at equilibrium is 1.5 bar. What is K for this reaction?
A (g) <--> B (g) + C (g)
0.5
To find the equilibrium constant (K) for the given reaction A (g) <--> B (g) + C (g), you need to know the equilibrium concentrations or partial pressures of the gases involved.
In this case, the vessel initially contains pure A, so the concentration or partial pressure of A at the start is 1.0 bar. At equilibrium, the total pressure of all the gases is 1.5 bar.
Since the total pressure at equilibrium is higher than the initial pressure of A, it suggests that the reaction has shifted to the right (towards the products) to increase the total pressure.
Let's denote the equilibrium concentrations or partial pressures as follows: [A], [B], and [C].
Using the given information, we can say that [A] = 1.0 bar, [B] = ? and [C] = ?
To determine the equilibrium concentrations or partial pressures of B and C, we need more information. This could be in terms of a balanced chemical equation, the stoichiometry of the reaction, or additional data about the reaction conditions.
Once you have the equilibrium concentrations or partial pressures of all the species involved, you can use the expression for the equilibrium constant (K) to calculate its value. For the given reaction, the expression for K would be:
K = ([B] * [C]) / [A]
However, since we don't have the necessary information to determine the equilibrium concentrations or partial pressures, we cannot calculate the value of K at this point.