Consider the balanced chemical equation. H2O2 (aq) + 3I - (aq) + 2H + (aq) →I3 - (aq) + 2H2O (l) In the first 15.0 s of the reaction, the concentration of I - drops from 1.000 M to 0.871 M. Part A Predict the rate of change in the concentration of H2O2 (Δ[H2O2]/Δt). Express the rate to three significant figures and include the appropriate units. Δ[H2O2]/Δt Δ [ H 2 O 2 ] / Δ t =

Part B Predict the rate of change in the concentration of I3 - (Δ[I3-]/Δt). Express the rate to three significant figures and include the appropriate units. Δ[I3-]/Δt Δ [ I 3 - ] / Δ t =

Question

Wilson Burns

Chemistry

16 November, 00:13

Consider the balanced chemical equation. H2O2 (aq) + 3I - (aq) + 2H + (aq) →I3 - (aq) + 2H2O (l) In the first 15.0 s of the reaction, the concentration of I - drops from 1.000 M to 0.871 M. Part A Predict the rate of change in the concentration of H2O2 (Δ[H2O2]/Δt). Express the rate to three significant figures and include the appropriate units. Δ[H2O2]/Δt Δ [ H 2 O 2 ] / Δ t =

Part B Predict the rate of change in the concentration of I3 - (Δ[I3-]/Δt). Express the rate to three significant figures and include the appropriate units. Δ[I3-]/Δt Δ [ I 3 - ] / Δ t =

+3

Answers (1)

Know the Answer?

Marin Melendez · Answer 1

Part A. 8.60 * 10⁻³ M/s

Part B. 8.60 * 10⁻³ M/s

Explanation:

Let's consider the following balanced chemical equation.

H₂O₂ (aq) + 3 I⁻ (aq) + 2 H⁺ (aq) → I₃⁻ (aq) + 2 H₂O (l)

Part A

The rate of change in the concentration of H₂O₂ is:

-Δ[H₂O₂]/Δt = - (0.871 M - 1.000 M) / 15.0 s = 8.60 * 10⁻³ M/s

Part B

The molar ratio of H₂O₂ (aq) to I₃⁻ (aq) is 1:1. The rate of change in the concentration of I₃⁻ is:

8.60 * 10⁻³ mol H₂O₂/L. s * (1 mol I₃⁻/1 mol H₂O₂) = 8.60 * 10⁻³ mol I₃⁻/L. s = 8.60 * 10⁻³ M/s