### Question 9 of 36---#### Problem Statement:**What is the rate at which Br-(aq) disappears in the reaction below if the rate of disappearance of BrO3-(aq) is 0.020 M/s?**The chemical reaction is as follows:BrO3- + 5 Br- + 6 H+ → 3 Br2 + 3 H2O---This problem involves understanding and applying the concept of reaction rates in chemistry, specifically in a balanced chemical equation.- **Given Data:** - The rate of disappearance of BrO3-(aq) = 0.020 M/s- **Objective:** - To determine the rate at which Br-(aq) is disappearing.**Solution:**The rate of reaction can be related to the change in concentration of each reactant and product over time using the stoichiometric coefficients from the balanced equation.From the balanced equation:\[ BrO_3^- + 5 Br^- + 6 H^+ \rightarrow 3 Br_2 + 3 H_2O \]For a general reaction of the form:\[ aA + bB \rightarrow cC + dD \]The rates are related by:\[ \frac{-1}{a}\frac{d[A]}{dt} = \frac{-1}{b}\frac{d[B]}{dt} = \frac{1}{c}\frac{d[C]}{dt} = \frac{1}{d}\frac{d[D]}{dt} \]Applying this to the given reaction:\[ \frac{-d[BrO_3^-]}{dt} = \frac{1}{1} \]\[ \frac{-d[Br^-]}{dt} = \frac{1}{5} \]Therefore, the rate of disappearance of Br2- relates to the rate of disappearance of BrO3- as follows:\[ \frac{-d[Br^-]}{dt} = 5 \times \frac{-

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Answered: What is the rate at which Br"(aq)…

What is the rate at which Br"(aq) disappears in the reaction below if the rate of disappearance of BrO3"(aq) is 0.020 M/ s? BrOg + 5 Br" + 6 H* → 3 Br, + 3H;0

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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For the reaction BrO, + 5Br + 6H* → 3Br, + 3H,0, the rate of disappearance of BrO is 0.015 M/s at 25°C at a particular instant. What is the rate of disappearance of H* (in M/s) at the same instant?
NTERACTIVE EXAMPLE Reaction Rate Chloromethane reacts with iodide ion to yield iodomethane and chloride ion. CH;C1 +r- CH;I + CF A way to determine the rate of the reaction of chloromethane with iodide ion is to measure the disappearance of T from the solution. Suppose that the concentration of I was 0.21 mol IL at the start of the reaction. At the end of 20 min, the concentration dropped to 0.13 mol L. This difference is equal to a change in concentration of -0.08 mol IL. QUESTION What is the rate of reaction with respect to iodide ion? |× molIL'min
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4. The rate law for the reaction H:(g) + F2(g) 2HF(g) at 298 K is rate = k [H.][F-]. %3D Predict the effect of each of the following changes on the initial rate of the reaction. * increase decrease no change Addition of H2 at constant temperature and volume Increase in volume of the reaction vessel Addition of a catalyst O O O O O O O O O
2. At 325°C, N0,(g) reacts with CO(g) to yield NO(g) and CO,(g). The reaction is: NO,(g) + CO(g) I NO(g) + CO,(g) It is observed that the reaction rate does not depend upon the concentration of CO, and t\so the reaction rate law does not involve [CO]. The rate does depend upon [NO,], however, and the following data is obtained. Determine the rate law and the value of the rate constant. Rate ( M sec ') NO,] 1. 1 X 10 -2 0.15 4.5 X 10-2 0.3 1.8 X 10- 4.0 X 10-13 0.6 0.9