Final answer:
The rate at which Br⁻(aq) disappears when the rate of disappearance of BrO₃⁻(aq) is 0.020 M/s can be calculated using stoichiometry to be 0.100 M/s, based on the 5:1 molar ratio from the balanced equation.
Step-by-step explanation:
The question asks for the rate at which Br-(aq) disappears in a chemical reaction given the rate of disappearance of BrO₃⁻(aq) is 0.020 M/s. To find this rate, we look at the stoichiometry of the reaction. The balanced equation is: 5Br⁻(aq) + BrO₃⁻(aq) + 6H+¹ (aq) → 3Br₂(aq) + 3H₂O(l).
From the equation, we see that for every 1 mole of BrO₃⁻(aq) that reacts, 5 moles of Br⁻(aq) are consumed. If the rate of disappearance of BrO₃⁻(aq) is 0.020 M/s, then the rate of disappearance of Br⁻(aq) can be calculated by multiplying the given rate of BrO₃⁻(aq) disappearance by the molar ratio of Br⁻(aq) to BrO₃⁻(aq), which is 5:1. Therefore, the rate of disappearance of Br⁻(aq) is 0.020 M/s * 5 = 0.100 M/s.