Question

At a certain temperature, the equilibrium constant for the chemical reaction shown is 1.60×10−3 . At equilibrium, the concentration of AB is 1.825 M, the concentration of BC is 1.625 M, and the concentration of AC is 0.130 M. Calculate the concentration of B at equilibrium. AB(aq)+BC(aq)↽−−⇀AC(aq)+2B(aq) AB ( aq ) + BC ( aq ) ↽ − − ⇀ AC ( aq ) + 2 B ( aq ) [B] =

Answer 1

Answer: Thus the concentration of B at equilibrium is 0.191 M

Explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as $K_c$

For the given chemical reaction:

$AB(aq)+BC(aq)\rightarrow AC(aq)+2B(aq)$

The expression for $K_c$ is written as:

$K_c=\frac{[B]^2\times [AC]}{[BC]\times [AB]}$

$1.60\times 10^{-3}=\frac{(B)^2\times (0.130)}{(1.625\times 1.825)}$

$B=0.191M$

Thus the concentration of B at equilibrium is 0.191 M