Question

The equilibrium constant for this reaction is Keq =3.0×103 . The reaction mixture at equilibrium contains [A] = 1.0×10−4 M . What is the concentration of B in the mixture? A(g)⇌B(g)

Answer 1

To find the equilibrium concentration of B in a reaction where Keq = 3.0×103 and [A] = 1.0×10⁻⁴ M, the formula [B] = Keq × [A] is used to obtain [B] = 0.3 M.

Step-by-step explanation:

The question concerns the equilibrium concentration of B when the equilibrium constant (Keq) is known and the equilibrium concentration of A is given. To calculate B's concentration, we use the given Keq and the expression Keq = [B] / [A]. Knowing that Keq is 3.0×103 and [A] is 1.0×10⁻⁴ M, we can rearrange this to [B] = Keq × [A] and calculate the concentration of B.

Substituting the given values into the formula yields:

[B] = (3.0×103) × (1.0×10⁻⁴ M)

The concentration of B at equilibrium is therefore calculated to be [B] = 0.3 M.

Answer 2

The concentration of B in the mixture is 0.3 M.

What is equilibrium concentration?

The concentration of reactants and products in a chemical reaction system at the equilibrium point is referred to as equilibrium concentration. Reactants are changed into products in a chemical reaction, but the reaction need not proceed to its fullest extent.

The equilibrium concentrations are often denoted by square brackets.

We know that;

Keq = [B]/[A]

3.0 *
`10^3` = [B]/[1.0 *
`10^{-4`]

[B] = 3.0 *
`10^3` * 1.0 *
`10^{-4`

= 0.3 M