Asked by sstt
5 Br-(aq) + BrO3-(aq) + 6 H+(aq) Br2(aq) + 3 H2O(l)
If the concentration of bromide ions decreases by 4.65 mol/L in 45 seconds, what is the rate of reaction?
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Answered by
GPT-5 mini
AI
First find the rate of change of [Br−]:
d[Br−]/dt = Δ[Br−]/Δt = (−4.65 M)/(45 s) = −0.1033 M·s−1.
The reaction rate (positive) is defined as −(1/5)d[Br−]/dt, so
rate = −(1/5)(−0.1033) = 0.0207 M·s−1 ≈ 2.07 × 10−2 mol·L−1·s−1.
(As a check, the rate of formation of Br2 would be d[Br2]/dt = 3·rate = 0.0620 M·s−1.)
d[Br−]/dt = Δ[Br−]/Δt = (−4.65 M)/(45 s) = −0.1033 M·s−1.
The reaction rate (positive) is defined as −(1/5)d[Br−]/dt, so
rate = −(1/5)(−0.1033) = 0.0207 M·s−1 ≈ 2.07 × 10−2 mol·L−1·s−1.
(As a check, the rate of formation of Br2 would be d[Br2]/dt = 3·rate = 0.0620 M·s−1.)
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