Question

The reaction represented by the equation: xA + yB ---> productsis started by mixing 1.00 mol of A with 2.00 mol of B in a 1.00 L container at a certain temperature. These concentrations are measured after a certain time.Substance Concentration, M[A] 0.875[B] 1.81Which is the x/y ratio in this reaction?

Answer 1

The x/y ratio of the reaction is 0.68

Step-by-step explanation:

Hi there!

The rate of dissapearence of A and B can be expressed as follows:

rate A = -Δ[A] /Δt

rate B = -Δ[B] / Δt

Where:

Δ[A] = change in the concentration of A (final [A] - initial [A])

Δ[B] = change in the concentration of B (final [B] - initial [B])

Δt = elapsed time.

These rates are equal if we divide each of them by their respective estechiometric coefficient:

1/x · (-Δ[A] /Δt) = 1/y · (-Δ[B] / Δt)

Let´s multiply by x each side of the equation:

-Δ[A] /Δt = x/y · (-Δ[B] / Δt)

now, let´s divide each side of the equation by (-Δ[B] / Δt)

(-Δ[A] /Δt) · (- Δt / Δ[B]) = x/y

Δ[A] / Δ[B] = x/y

Δ[A] = final [A] - initial [A] = 0.875 M - 1.00 M = -0.13 M

Δ[B] = final [B] - initial[B] = 1.81 M - 2.00 M = -0.19 M

-0.13 M / -0.19 M = x/y

x/y = 0.68

The x/y ratio of the reaction is 0.68