A solution initially contains 0.350 mol/L of A and 0.750 mol/L of B. A reaction occurs according to the equation

2 A(aq)+B(aq)<=> 3 C(aq)+D(s)
At equilibrium, [C] is found to be 0.100 mol/L. What is the value of Keq?

.........2A(aq) + B(aq) =>3C(aq) + D(s)

initial.0.350....0.750....0........0
change....-2x.....-x......+3x......x
equil...................0.100.......

If C is 0.100 M at equilibrium, then 3x = 0.100 and x = 0.100/3 = 0.0333
Then B must be 0.750-0.0333 = ? and A must be 0.350-2*0.0333 = ?
Keq = (B)/(A)^2*(B)
Substitute and solve for Keq. Note that D is not included because it is a solid.

thank-you so much for the help

To find the value of Keq, we need to know the equilibrium concentrations of A, B, C, and D.

Let's assume that the equilibrium concentration of C is x mol/L, and the concentration of D is y mol/L.

Using the stoichiometry of the balanced equation, we know that the concentration of A at equilibrium is (0.350 - 2x) mol/L (since 2 moles of A react to form 3 moles of C).

Similarly, the concentration of B at equilibrium is (0.750 - x) mol/L (since 1 mole of B reacts to form 3 moles of C).

The equilibrium constant expression for the given reaction is:

Keq = [C]^3/[A]^2[B]

Plugging in the equilibrium concentrations we stated above:

Keq = (x^3)/((0.350 - 2x)^2 * (0.750 - x))

Since we know that [C] at equilibrium is 0.100 mol/L, we can substitute this value into the equation:

Keq = (0.100^3)/((0.350 - 2*0.100)^2 * (0.750 - 0.100))

Simplifying this expression will give us the value of Keq.

To determine the value of Keq (the equilibrium constant) for the given reaction, we need to use the concentrations of the reactants and products at equilibrium. The equilibrium constant expression for the reaction is given by:

Keq = [C]^3[D] / [A]^2[B]

Given that [C] is 0.100 mol/L, we can substitute this value into the expression:

Keq = (0.100 mol/L)^3[D] / [A]^2[B]

However, to solve this equation, we still need the value of [D], which is the concentration of the solid product. In this case, since it is a solid, its concentration remains constant and does not affect the equilibrium constant. Therefore, we can assume that [D] is a constant value.

So, the equilibrium expression can be simplified as:

Keq = (0.100 mol/L)^3 / [A]^2[B]

Now, we need to determine the concentration of A and B at equilibrium. However, we are only given their initial concentrations, not their equilibrium concentrations. To find their equilibrium concentrations, we need additional information.

This additional information can either be the values of Ksp (the solubility product constant) for any of the reactants or products, or the value of the reaction quotient Q at equilibrium. With either of these values, we can determine the equilibrium concentrations by using an ICE (Initial, Change, Equilibrium) table and solving for the unknowns.

Please provide either the Ksp values or reaction quotient Q, and the solubility or concentrations of any relevant components so that we can determine the equilibrium concentrations of A and B and ultimately calculate Keq.