Consider the equilibrium, A + B <--> C, with K=32.217 and initial concentrations of A,B, and C, of 3.665M, 0.883M, and 3.925M, respectively. What is the equilibrium concentration of B

3.665 0.883 3.925
A + B = C
Keq=(C)/(A)*(B)= 32.217
Q = (3.025)/(3.665)*(0.883)=1.21
Q < Keq; therefore, the reaction must proceed to the right.
Let y = amount of C formed.
At equilibrium,
(A) = 3.665-y
(B) = 0.883-y
(C) = 3.925+y)
Solve for y and the concentration of each. Post your work if you get stuck.

To find the equilibrium concentration of B, we need to solve for the value of y using the given equilibrium constant (Keq) and the initial concentrations of A, B, and C.

Given:
Initial concentration of A = 3.665 M
Initial concentration of B = 0.883 M
Initial concentration of C = 3.925 M
Equilibrium constant (Keq) = 32.217

Using the equation for Keq, we can rewrite it in terms of concentrations:
Keq = (C)/(A)*(B)

Plugging in the given values:
32.217 = (3.925 + y)/(3.665)*(0.883)

Now, we need to calculate the reaction quotient (Q) using the initial concentrations:
Q = (A)/(B)*(C) = (3.665)/(0.883)*(3.925) = 16.269

Since Q < Keq, the reaction must proceed to the right.

Now, let's substitute the expressions for the concentrations at equilibrium:
(A) = 3.665 - y
(B) = 0.883 - y
(C) = 3.925 + y

Plugging these expressions into the equation for Keq:
32.217 = (3.925 + y)/(3.665 - y)*(0.883 - y)

Solve this equation to find the value of y, which represents the amount of C formed at equilibrium.

Please let me know if you need further assistance with solving this equation.