Question

Given the following balanced equation, determine the rate of reaction with respect to [SO3]. If the rate of O2 loss is 3.56 x 10^-3 M/s, what is the rate of formation of SO3?

2 SO2(g) + O2(g) = 2 SO3(g)

Answer 1

The general chemical reaction as follows:

2A+B→2C+D

rate of reaction =

−1 / 2 Δ[A] / Δt=−Δ[B] / Δt=1 / 2 Δ[C] / Δt=Δ[D] / Δt

Similar for this reaction

2 SO2(g) + O2(g) = 2 SO3(g)

−1 / 2 Δ[SO2 ] / Δt=−Δ[O2 ] / Δt=1 / 2 Δ[SO3 ] / Δt

Given that

the rate of O2 loss = 3.56 x 10^-3 M/s

therefore;

+1 / 2 Δ[SO3 ] / Δt=−Δ[O2 ] / Δt

Negative sign indicate the decrease in concentration

Positive sign indicate the increases in concentration

Δ[SO3 ] / Δt= 2 *[ Δ[O2 ] / Δt ]

Δ[SO3 ] / Δt= 2 *[ 3.56 x 10^-3 M/s ]

= 7.12 x 10^-3 M/s