Explanation The equation that describes the relationship between the concentration of the reactants and the rate of the reaction is often termed as the rate law. The equation representing the formation of HBr or hydrogen bromide is provided below: Br 2 ( g ) ⇌ k − 1 k 1 2Br ( g ) Fast Br ( g ) + H 2 ( g ) → k 2 HBr ( g ) + H ( g ) Slow H ( g ) + Br 2 → k 3 HBr ( g ) + Br ( g ) Fast The rate of a reaction is given by the following equation, wherein k refers to the rate constant, [A] represents the reactant’s concentration, and n represents the order of the reaction: Rate = k [ A ] n Furthermore, at equilibrium, the rate of the forward and the backward reaction is same; thus, the concentration of bromine can be calculated using the rate as follows: k 1 [ Br 2 ] = k − 1

Masteringchemistry With Pearson Etext -- Valuepack Access Card -- For Principles Of Chemistry: A Molecular Approach

3rd Edition

ISBN: 9780133890686

Author: Tro

Publisher: PEARSON

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Chapter 13, Problem 105E

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To describe: The rate law corresponding to the given reaction mechanism.

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Chapter 13, Problem 104E

Chapter 13, Problem 106E

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Masteringchemistry With Pearson Etext -- Valuepack Access Card -- For Principles Of Chemistry: A Molecular Approach

Ch. 13 - Q1. This graph shows the concentration of the...Ch. 13 - Q2. Dinitrogen monoxide decomposes into nitrogen...Ch. 13 - Q3. This plot shows the rate of the decomposition...Ch. 13 - Prob. 4SAQ Ch. 13 - Prob. 5SAQ Ch. 13 - Prob. 6SAQ Ch. 13 - Prob. 7SAQ Ch. 13 - Prob. 8SAQ Ch. 13 - Prob. 9SAQ Ch. 13 - Prob. 10SAQ

Ch. 13 - Q11. The mechanism shown is proposed for the gas...Ch. 13 - Q12. Which statement is true regarding the...Ch. 13 - Q13. These images represent the first-order...Ch. 13 - Prob. 14SAQ Ch. 13 - Prob. 15SAQ Ch. 13 - Prob. 1E Ch. 13 - Prob. 2E Ch. 13 - Prob. 3E Ch. 13 - 4. Why is the reaction rate for reactants defined...Ch. 13 - Prob. 5E Ch. 13 - Prob. 6E Ch. 13 - Prob. 7E Ch. 13 - 8. For a reaction with multiple reactants, how is...Ch. 13 - 9. Explain the difference between the rate law for...Ch. 13 - 10. Write integrated rate laws for zero-order,...Ch. 13 - Prob. 11E Ch. 13 - 12. How do reaction rates typically depend on...Ch. 13 - Prob. 13E Ch. 13 - 14. What is an Arrhenius plot? Explain the...Ch. 13 - Prob. 15E Ch. 13 - Prob. 16E Ch. 13 - 17. In a reaction mechanism, what is an elementary...Ch. 13 - 18. What are the two requirements for a proposed...Ch. 13 - 19. What is an intermediate within a reaction...Ch. 13 - Prob. 20E Ch. 13 - 21. Explain the difference between homogeneous...Ch. 13 - Prob. 22E Ch. 13 - Prob. 23E Ch. 13 - Prob. 24E Ch. 13 - 25. Consider the reaction: 2 HBr(g) → H2(g) +...Ch. 13 - 26. Consider the reaction: 2 N2O(g) → 2 N2(g) +...Ch. 13 - 27. For the reaction 2 A(g) + B(g) → 3 C(g), a....Ch. 13 - 28. For the reaction A(g) + B(g) → 2 C(g), a....Ch. 13 - 29. Consider the reaction: Cl2(g) + 3 F2(g) → 2...Ch. 13 - Prob. 30E Ch. 13 - Prob. 31E Ch. 13 - Prob. 32E Ch. 13 - 33. Consider the reaction: H2(g) + Br2(g) ? 2...Ch. 13 - 34. Consider the reaction: 2 H2O2(aq) ? 2 H2O(l) +...Ch. 13 - Prob. 35E Ch. 13 - Prob. 36E Ch. 13 - Prob. 37E Ch. 13 - 38. This reaction is first order in N2O5: N2O5(g)...Ch. 13 - Prob. 39E Ch. 13 - Prob. 40E Ch. 13 - Prob. 41E Ch. 13 - 42. Consider the data showing the initial rate of...Ch. 13 - 45. The tabulated data were collected for this...Ch. 13 - 46. The tabulated data were collected for this...Ch. 13 - 47. Indicate the order of reaction consistent with...Ch. 13 - 48. Indicate the order of reaction consistent with...Ch. 13 - 49. The tabulated data show the concentration of...Ch. 13 - Prob. 48E Ch. 13 - 51. The tabulated data show the concentration of...Ch. 13 - 52. The reaction A → products was monitored as a...Ch. 13 - Prob. 51E Ch. 13 - Prob. 52E Ch. 13 - Prob. 53E Ch. 13 - Prob. 54E Ch. 13 - 57. The half-life for the radioactive decay of...Ch. 13 - 58. The half-life for the radioactive decay of...Ch. 13 - 5957. The diagram shows the energy of a reaction...Ch. 13 - Prob. 58E Ch. 13 - Prob. 59E Ch. 13 - Prob. 60E Ch. 13 - Prob. 61E Ch. 13 - Prob. 62E Ch. 13 - 65. The data shown here were collected for the...Ch. 13 - Prob. 64E Ch. 13 - 67. The tabulated data were collected for the...Ch. 13 - 68. The tabulated data show the rate constant of a...Ch. 13 - 69. A reaction has a rate constant of 0.0117/s at...Ch. 13 - 70. A reaction has a rate constant of 0.000122/s...Ch. 13 - Prob. 69E Ch. 13 - Prob. 70E Ch. 13 - Prob. 71E Ch. 13 - Prob. 72E Ch. 13 - Prob. 73E Ch. 13 - Prob. 74E Ch. 13 - Prob. 75E Ch. 13 - Prob. 76E Ch. 13 - 79. Many heterogeneous catalysts are deposited on...Ch. 13 - 80. Suppose that the reaction A → products is...Ch. 13 - 81. Suppose that a catalyst lowers the activation...Ch. 13 - Prob. 80E Ch. 13 - Prob. 81E Ch. 13 - Prob. 82E Ch. 13 - Prob. 83E Ch. 13 - Prob. 84E Ch. 13 - Prob. 85E Ch. 13 - Prob. 86E Ch. 13 - Prob. 87E Ch. 13 - Prob. 88E Ch. 13 - 91. Iodine atoms combine to form I2 in liquid...Ch. 13 - 9290. The hydrolysis of sucrose (C12H22O11) into...Ch. 13 - 9391. The reaction AB(aq) ? A(g) + B(g) is second...Ch. 13 - Prob. 92E Ch. 13 - Prob. 93E Ch. 13 - Prob. 94E Ch. 13 - 97. The desorption (leaving of the surface) of a...Ch. 13 - Prob. 96E Ch. 13 - 99. The kinetics of this reaction were studied as...Ch. 13 - Prob. 98E Ch. 13 - Prob. 99E Ch. 13 - 102100. Consider the two reactions: a. Why is...Ch. 13 - 103. Anthropologists can estimate the age of a...Ch. 13 - 104. Geologists can estimate the age of rocks by...Ch. 13 - Prob. 103E Ch. 13 - 106104. Consider the reaction: 2 NH3(aq) +...Ch. 13 - Prob. 105E Ch. 13 - Prob. 106E Ch. 13 - Prob. 107E Ch. 13 - Prob. 108E Ch. 13 - Prob. 109E Ch. 13 - Prob. 110E Ch. 13 - 113. In this chapter we have seen a number of...Ch. 13 - 1124. The first-order integrated rate law for the...Ch. 13 - 115. The previous exercise shows how the...Ch. 13 - Prob. 114E Ch. 13 - Prob. 115E Ch. 13 - Prob. 116E Ch. 13 - Prob. 117E Ch. 13 - 120118. Consider the reaction: CHCl3(g) + Cl2(g) ?...Ch. 13 - Prob. 119E Ch. 13 - Prob. 120E

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