Question

When the following reaction comes to equilibrium, will the concentrations of the reactants or products be greater?A(g)+B(g)⇌2C(g)Kc=1.4×10−5the concentrations of the reactantsthe concentrations of the products

Answer 1

Answer:

The concentration of the reactants.

Explanation:

When a reversible reaction reaches the equilibrium, the velocity of the formation of the products is the same as the velocity of the formation of the reactants, and then, the concentrations of the substances remain constant.

The equilibrium can be represented by the equilibrium constant, which for a generic reaction:

aA + bB ⇄ cC + dD

$Kc = \frac{[C]^c*[D]^d}{[A]^a*[B]^b}$

The solids components and the water are not included in the equation.

So, for the reaction given:

Kc = [C]²/([A]*[B]

Because Kc has a small value (1.4x10⁻⁵), the value of [A]*[B] must be huge, thus the concentrations of the reactants are greater.