The value of the equilibrium constant?

Question

The following reaction occurs:

_A(g)  + B_(g) ↔  C_(g) + D_(g)

The initial concentrations of A_(g) and B_(g)  are both 2.10 mol/L. At equilibrium, A_(g) has a concentration of 1.74.

The value of the equilibrium constant Kc is a.bcd

Write your answer for a.bc in the blank, including the decimal.

Your Answer:

Answer 1

A + B <==> C + D

2.1....2.1.........0.........0...initial

-0.36....-0.3...+0.36....+0.36...change

1.74..174..... 0,36....0.36...equilibrium

K = [C][D]/[A][B] = (0.36)(0.36)/(1.74)(1.74) = 0.0428