An experimental determination of the rate law finds the following expression fc reaction rate. Rate = k [IO3] [H+]² Which of the following changes would have the LEAST effect on increasing the of this reaction? Add a catalyst to the reaction mixture. Double [1] while keeping [103] and [H*] constant. Double [103] while keeping [1] and [H*] constant. Heat the reaction chamber 60 °C hotter. Double [H*] while keeping [1] and [1037] constant.

An experimental determination of the rate law finds the following expression fc reaction rate. Rate = k [IO3] [H+]² Which of the following changes would have the LEAST effect on increasing the of this reaction? Add a catalyst to the reaction mixture. Double [1] while keeping [103] and [H] constant. Double [103] while keeping [1] and [H] constant. Heat the reaction chamber 60 °C hotter. Double [H*] while keeping [1] and [1037] constant.

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...

See similar textbooks

Similar questions

Which of the following statements is the best explanation of how activation energy affects the rate of a chemical reaction? A. A high activation energy means molecules have less kinetic energy and hence rate of reaction will be slower. B. A high activation energy means molecules must have more kinetic energy to overcome it, and hence rate of reaction will be faster. C. A high activation energy means molecules have a lot of kinetic energy and hence rate of reaction will be faster. D. A high activation energy means molecules must have less kinetic energy to overcome it, and hence rate of reaction will be slower. E. A high activation energy means molecules must have more kinetic energy to overcome it, and hence rate of reaction will be slower.
Consider a hypothetical chemical reaction: A+B C+D (In this equation A, B, C and D stand for some unknown chemical formulas.) Here is an energy diagram for the reaction: 400 300+ energy 200 - (k]/mol) C +D A +B 100 + reaction coordinate Use the energy diagram to answer these questions. | kJ/mol What is the heat of reaction? Exothermic Endothermic Is the reaction exothermic or endothermic? Neither it's kJ/mol Can you determine the activation energy? No. Yes, it's kJ/mol Can you determine the activation energy of the reverse reaction? Explanation Check © 2021 McGraw-Hill Education. All Rights Reserved.
Consider the following reaction and its associated rate law. A + B ----> C R = k[A]2 Which of the following will not increase the rate of the reaction? Group of answer choices adding a suitable catalyst. increasing the temperature of the reaction. increasing the concentration of reactant B. increasing the concentration of reactant A.
Which would likely increase the rate of a chemical reaction? A. Cooling the reaction mixture. B. Decreasing the concentration of the reactants. C. Decreasing the surface area of the reactants. D. Adding a catalyst to the reaction mixture.
The progress of a reaction is tracked by following the concentration of one reactant as it is consumed. The table gives the concentration of that reactant at several times. Time (s) [R] (mol/L) 5.00 × 10-3 4.32 × 10-3 3.66 × 10-3 3.03 × 10-3 2.44 x 10-³ 1.90 x 10-³ 1.39 × 10-3 0 10.5 22.3 35.7 51.1 69.3 91.6 120.4 160.9 230.3 299.6 -4 9.27 x 107 5.26 x 10-4 1.99 x 10-4 7.54 x 10-5 a Use graphing software to plot the data as [R] versus time, and determine the average rate for the first 15 s and the average rate from t = 100 to t = 125 s. Enter the rates as positive values. Rate (from t = 0 tot = 15 s) = Rate (from t = 100 to t = 125 s) = M/s M/s Previous Next
Consider the Energy diagram below. What does the variable "E" indicate? TS 2 E TS 1 e r g y U Reaction Progress energy of activation S -----> T energy of activation U -----> S free energy change U -----> S free energy change S ----> T
Based on the following mechanism write out the rate law for the overall reaction. Also identify any catalysts or intermediates. Step 1. A + B -› C Slow Step 2. B + C -› D Fast Step 3. 2D -› E Very Fast
Classify the actions based on how they could affect a reaction rate. Rate increases Rate decreases Rate is unaffected Answer Bank decrease the concentration of a reactant decrease the surface area of a solid reactant increase the temperature add a catalyst
7. Reactions A and B were studied and found to produce the given energy diagrams. 150 150 Energy 100 (kJ/mol) 100 Energy (kJ/mol) 50 50 Reaction progress Reaction progress Reaction A Reaction B A third reaction, C was studied with a measured activation energy of 55 KJ/mol. Assume all reactions take place at the same temperature. Reaction A is slowest a. b. Reaction B is slowest c. Reaction C is slowest d. All reactions happen at the same rate.
Chemistry: Fundamentals and Principles Davidson presented by Macmillan Le Reaction A has a high activation energy, whereas reacton B has a low activation energy. Which of the statements about reaction A and reaction B are true? Reaction A is more likely to occur at all than reaction B. Reaction B is likely to occur at a faster rate than reaction A. Reaction B is more likely to occur at all than reaction A. Reaction A is likely to occur at a faster rate than reaction B. O O O
⦁ 4. Make your own energy diagram for an exothermic reaction that does not include a catalyst and one with a catalyst (Be sure each line is a different color or labeled). Label the axis of the diagram. Then, state what a catalyst is and how a catalyst affects the reaction rate.
2ClO(g) ----> Cl2(g) + O2(g) Explain how you know that this is a very fast reaction.