posted by Rob on .
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
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.
(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.