Given the following reaction:
XBO3(s) <--> XO(s) + BO2(g)
If the concentration of BO2 at equilibrium was 2.0 M, what is the equilibrium constant (K)?
Select one:
a. Not enough information is given
b. 1.0 M
c. 2.0 M
d. 0.50 M
To determine the equilibrium constant (K) for the given reaction:
XBO3(s) <--> XO(s) + BO2(g)
The equilibrium constant expression can be written as:
K = [XO] * [BO2] / [XBO3]
However, the concentration of XO and XBO3 are not specified in the question. Therefore, we do not have enough information to calculate the equilibrium constant (K). The correct answer is:
a. Not enough information is given
To find the equilibrium constant (K) for the given reaction, you need the concentrations of all the species in the reaction at equilibrium. However, the concentration of BO2 at equilibrium is given as 2.0 M. This information alone is not sufficient to determine the equilibrium constant.
The equilibrium constant (K) is calculated by dividing the concentration of the products by the concentration of the reactants, with each concentration raised to the power equal to its coefficient in the balanced chemical equation.
Since we do not have the concentrations of XO and XBO3 at equilibrium, it is not possible to calculate the equilibrium constant (K) based on the given information. Therefore, the answer is (a) Not enough information is given.
Solids don't enter into the equilibrium constant expression; therefore, ignoring those the expression is
Keq = (BO2)
Since the (BO2) at equilibrium is given as 2.0 M in the problem, then K must be .....?