The balanced equation for the reaction of bromate ion with bromide in acidic solution is BrO+ 5Br^- + 6H⁺ $\rightarrow$ 3Br₂ + 3H₂O
At a particular instant in time, the value of - $\Delta$ [Br^-]/ $\Delta$ t is 2.0 * 10^-³ mol/L • s. What is the value of $\Delta$ [Br₂]/ $\Delta$ t in the same units?

Question

The balanced equation for the reaction of bromate ion with bromide in acidic solution is BrO+ 5Br^- + 6H⁺

\rightarrow

3Br₂ + 3H₂O
At a particular instant in time, the value of -

\Delta

[Br^-]/

\Delta

t is 2.0 * 10^-³ mol/L • s. What is the value of

\Delta

[Br₂]/

\Delta

t in the same units?

Quizplus · Accepted Answer

The stoichiometry of the reaction shows that 5 moles of Br⁻ produce 3 moles of Br₂. Therefore, the rate of formation of Br₂ is (3/5) times the rate of consumption of Br⁻, which is (3/5) * 2.0 × 10⁻³ mol/L•s = 1.2 × 10⁻³ mol/L•s.

The Balanced Equation for the Reaction of Bromate Ion with Bromide