4.The Reaction below should be used for questions 4 and 5.105 + 51- + 6H* → 312+ 3H2OThe oxidation of iodide ions by iodate ions in acidic aqueous solutionoccurs according to the stoichiometry shown above. The experimentallydetermined rate law of the reaction israte = k[IO3] [I]According to the rate law for the reaction, an increase in the concentrationof hydrogen ion has what effect on this reaction?(a) The rate of reaction increases.(b) The rate of the reaction decreases.(c) The value of the rate law constant increases.(d) Neither the rate nor the value of the rate law constant is changed.

The given balanced chemical reaction is- IO3- + 5I- + 6H+→3I2 + 3H2O The experimentally determined…

4. The Reaction below should be used for questions 4 and 5. 10, + 51- + 6H* - 312 + 3H20 The oxidation of iodide ions by iodate ions in acidic aqueous solution occurs according to the stoichiometry shown above. The experimentally determined rate law of the reaction is rate = k[10,"] [1"] According to the rate law for the reaction, an increase in the concentration of hydrogen ion has what effect on this reaction? (a) The rate of reaction increases. (b) The rate of the reaction decreases. (c) The value of the rate law constant increases. (d) Neither the rate nor the value of the rate law constant is changed.

4. The Reaction below should be used for questions 4 and 5. 10, + 51- + 6H* - 312 + 3H20 The oxidation of iodide ions by iodate ions in acidic aqueous solution occurs according to the stoichiometry shown above. The experimentally determined rate law of the reaction is rate = k[10,"] [1"] According to the rate law for the reaction, an increase in the concentration of hydrogen ion has what effect on this reaction? (a) The rate of reaction increases. (b) The rate of the reaction decreases. (c) The value of the rate law constant increases. (d) Neither the rate nor the value of the rate law constant is changed.

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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2. Consider the reaction that occurs when a CIO2 solution and a solution containing hydroxide ions (OH) are mixed at 0°C, shown in the following equation. 2CIO2(aq) + 2OH (aq) → Cl03° (aq) + CIO2° (aq) + H2O (1) When solutions containing CIO2 and OH- in various concentrations were mixed at 0 oC, the following rate data were obtained: Determination Initial concentration Initial concentration of Initial rate for formation number of ClO2, mol/L OH", mol/L of CIO3¯ mol/Ls 1.25x10-2 1.30x10-3 2.33x10-4 2.50x10-2 1.30x10-3 9.34x104 3 2.50x10-2 2.60x103 1.87x10-3 a) Use the method of initial rates to find the order of the reaction with respect to CIO2 and with respect to OH. Write the rate equation for the reaction of CIO2 and OH´ at 0°C. b) Calculate the rate constant, k, for the reaction of clO2 and OH at 0°C. c) Calculate the reaction rate for the reaction CIO2 and OH at 0°C when the initial ClO2 and OH concentrations are 8.25x10-3 mol/L and 5.35x 10-² mol/L, respectively. 1.
Use the information about the rate law to answer the questions below.
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