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)

law of conservation of mass

o.5

To determine the equilibrium constant (K) for the given reaction, you need to know the partial pressures of all the gases involved in the equilibrium.

In this case, the vessel initially contains only pure A at a pressure of 1.0 bar, so the initial partial pressure of A is 1.0 bar.

At equilibrium, the total pressure of all the gases is 1.5 bar. Since A is the only gas initially present, the additional pressure must come from the gases B and C. Therefore, the partial pressures of B and C at equilibrium are (1.5 - 1.0) bar = 0.5 bar each.

Now you can write the expression for the equilibrium constant (K) using the partial pressures of the gases:

K = (P(B) * P(C)) / P(A)

Plugging in the values, K = (0.5 * 0.5) / 1.0 = 0.25.

So, the equilibrium constant (K) for this reaction is 0.25.