If the value of Kc for the reaction is 434, what is the concentration of C at equilibrium if initial concentrations of A and B are both 0.500 M. (Hint: Everthing is squared after you set-up the equilibrium expression with the values given.

The question is incomplete, here is the complete question:

A(aq) + B(aq) → 2C(aq)

If the value of Kc for the reaction is 434, what is the concentration of C at equilibrium if initial concentrations of A and B are both 0.500 M. (Hint: Everything is squared after you set-up the equilibrium expression with the values given.

The concentration of C at equilibrium is 0.912 M

Explanation:

We are given:

Initial concentration of A = 0.500 M

Initial concentration of B = 0.500 M

The given equation follows:

Initial:               0.5   0.5

At eqllm:        0.5-x   0.5-x         2x

The expression of for above equation follows:

We are given:

Putting values in above equation, we get:

Neglecting the value of x = 0.553 M because the equilibrium concentration of A and B will become negative, which is not possible

So, equilibrium concentration of C = 2x = 2(0.456) = 0.912 M

Hence, the concentration of C at equilibrium is 0.912 M

they are all solids.