The overall reaction of hydroxide radical with hydrogen gas occurs as follows: OH'(g) + H2(g) - H2O(g) + H'(g) and plays a significant role in the chemistry of the earth's atmosphere by converting OH to HO2 through the subsequent reaction of H with O2. HO2 is involved in the destruction of stratospheric ozone (J. Phys. Chem. A, 2006, 110, 6978). Below is a table of initial rates for this reaction at 431 K. Table of initial rates at T-431 K for the reaction of hydroxide radical with hydrogen. [OH] / mol L-1 [H2] / mol L-1 initial rate / mol L-1 s-1 5.75x10-5 3.85x10-7 7.52x10-4 5.75x10-5 5.90x10-7 1.15x10-3 4.60x10-5 8.70x10-7 1.36x10-3

The overall reaction of hydroxide radical with hydrogen gas occurs as follows: OH'(g) + H2(g) - H2O(g) + H'(g) and plays a significant role in the chemistry of the earth's atmosphere by converting OH to HO2 through the subsequent reaction of H with O2. HO2 is involved in the destruction of stratospheric ozone (J. Phys. Chem. A, 2006, 110, 6978). Below is a table of initial rates for this reaction at 431 K. Table of initial rates at T-431 K for the reaction of hydroxide radical with hydrogen. [OH] / mol L-1 [H2] / mol L-1 initial rate / mol L-1 s-1 5.75x10-5 3.85x10-7 7.52x10-4 5.75x10-5 5.90x10-7 1.15x10-3 4.60x10-5 8.70x10-7 1.36x10-3

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.33QE

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The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a catalyst? b. Which species is an intermediate? c. Ea for the uncatalyzed reaction O3(g)+O(g)2O2(g) is 14.0 kJ. Ea. for the same reaction when catalyzed is 11.9 kJ. What is the ratio of the rate constant for the catalyzed reaction to that for the uncatalyzed reaction at 25C? Assume that the frequency factor A is the same for each reaction.
Consider the following representation of the reaction 2NO2(g) 2NO(g) + O2(g). Determine the time for the final representation above if the reaction is a. first order b. second order c. zero order
For the reaction of crystal violet with NaOH(aq), the measured rate of reaction is 1.27 106 mol L1 s1 when the concentration of crystal violet cation is 4.13 105 mol/L. (a) Estimate how long it will take for the concentration of crystal violet to drop from 4.30 105 mol/L to 3.96 105 mol/L. (b) Could you use the same method to make an accurate estimate of how long it would take for the concentration of crystal violet to drop from 4.30 105 mol/L to 0.43 105 mol/L? Explain why or why not.
For a first order gas phase reaction A products, k = 7.2 104s1 at 660. K and k = 1.7 102s1 at 720. K. If the initial pressure of A is 536 torr at 295C, how long will it take for the pressure of A to decrease to 268 torr?
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.
The annual production of HNO3 in 2013 was 60 million metric tons Most of that was prepared by the following sequence of reactions, each run in a separate reaction vessel. (a) 4NH3(g)+5O2(g)4NO(g)+6H2O(g) (b) 2NO(g)+O2(g)2NO2(g) (C) 3NO2(g)+H2O(l)2HNO3(aq)+NO(g) The first reaction is run by burning ammonia in air over a platinum catalyst. This reaction is fast. The reaction in equation (c) is also fast. The second reaction limits the rate at which nitric acid can be prepared from ammonia. If equation (b) is second order in NO and first order in O2, what is the rate of formation of NO2 when the oxygen concentration is 0.50 M and the nitric oxide concentration is 0.75 M? The rate constant for the reaction is 5.8106 L2/mol2/s.
The Raschig reaction produces the industrially important reducing agent hydrazine, N2H4, from ammonia, NH3, and hypochlorite ion, OCl−, in basic aqueous solution. A proposed mechanism is Step 1: Step 2: Step 3: What is the overall stoichiometric equation? Which step is rate-limiting? What reaction intermediates are involved? What rate law is predicted by this mechanism?
Cobra venom helps the snake secure food by binding to acetylcholine receptors on the diaphragm of a bite victim, leading to the loss of function of the diaphragm muscle tissue and eventually death. In order to develop more potent antivenins, scientists have studied what happens to the toxin once it has bound the acetylcholine receptors. They have found that the toxin is released from the receptor in a process that can be described by the rate law Rate = k [acetylcholine receptortoxin complex] If the activation energy of this reaction at 37.0C is 26.2 kJ/mol and A = 0.850 s1. what is the rate of reaction if you have a 0.200M solution of receptor-toxin complex at 37.0C?
Ozone, O3, in the Earths upper atmosphere decomposes according to the equation 2 O3(g) 3 O2(g) The mechanism of the reaction is thought to proceed through an initial fast, reversible step followed by a slow, second step. Step 1: Fast, reversible O3(g) O2(g) + O(g) Step 2: Slow O3(g) + O(g) 2 O2(g) (a) Which of the steps is rate-determining? (b) Write the rate equation for the rate-determining step

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