Answer:
2.95
Step-by-step explanation:
To find K for the reaction C ⇌ B, we need to use the equilibrium constant expression for this reaction, which is:
K = [B]/[C]
We can relate the concentrations of B and C to the concentration of A using the equilibrium constants K1 and K2 and the law of mass action, which states that the product of the concentrations of the products raised to their stoichiometric coefficients divided by the product of the concentrations of the reactants raised to their stoichiometric coefficients is equal to the equilibrium constant for the reaction. Using this law, we can write:
K1 = [B]/[A]
K2 = [C]/[A]
We can rearrange these equations to solve for [A] in terms of [B] and [C]:
[A] = [B]/K1
[A] = [C]/K2
Setting these two expressions for [A] equal to each other and solving for [B]/[C], we get:
[B]/[C] = K1/K2
Substituting this expression for [B]/[C] into the expression for K, we get:
K = [B]/[C] = K1/K2
Plugging in the values for K1 and K2, we get:
K = 5.90/2.00 = 2.95
Therefore, the equilibrium constant for the reaction C ⇌ B is 2.95.