1: Consider the loss of ozone in a dilute, low pressure Os/O2 gas mixture in the steady state at standard (room) temperature due to the reactions, Os + O2 0+202 Ka (1) O+0 K2, 202 (2) 1.1 Write down the net reaction of reactions (1) & (2). Hence state the relative rate of Os destruction to that of Oz creation. State the net rate of O destruction. 1.2 Write down the reaction rates (i.e. d/dt) for each of the three species. 1.3 Hence show that, K,no,nos K2NO, + Kan no

1: Consider the loss of ozone in a dilute, low pressure Os/O2 gas mixture in the steady state at standard (room) temperature due to the reactions, Os + O2 0+202 Ka (1) O+0 K2, 202 (2) 1.1 Write down the net reaction of reactions (1) & (2). Hence state the relative rate of Os destruction to that of Oz creation. State the net rate of O destruction. 1.2 Write down the reaction rates (i.e. d/dt) for each of the three species. 1.3 Hence show that, K,no,nos K2NO, + Kan no

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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Chlorine dioxide (ClO₂) is a disinfectant used in municipal water treatment plants. It dissolves in basic solution producing ClO3 and ClO₂": 2 CLO₂(g) + 2 OH (aq) → ClO3(aq) + ClO₂ (aq) + H₂O(l) › The following kinetic data were obtained at 298 K for the reaction. Experiment [CIO₂]0 (M) [OH-]o (M) Initial Rate (M/s) 1 0.060 0.030 0.0248 2 0.020 0.030 0.00827 3 0.020 0.090 0.0247 Determine the rate law by indicating the values of "x" and "y" in the general rate law below. Rate = K[ClO₂]X[OH-]Y X = 1 = 1 y = OB b. Calculate the rate constant for this reaction at 298 K. Sig. Figs. are important. M-1. S-1 Rate constant, k = 184.4
3 - Consider the gas phase decomposition of acetic acid at 1200 K. It proceeds via two parallel reactions: CH:COOH → CH+ + CO: ki = 3.74 s CH:COOH – CH:co + H2O k2 = 4.65 s'! (a) What is the maximum percentage yield of the ketene CH:CO at this temperature? (b) What is the concentration of the ketene when the extent of reaction when is 0.5 (50%)? (c) To favor the second reaction, should you increase or decrease temperature?
Suppose the reduction of nitric oxide proceeds by the following mechanism: step elementary reaction rate constant 1 H,(g) + 2 NO(g) → N,0(g) + H,0(g) k1 2 H2(9) + N,0(9) → N2(9) + H,O(g) Suppose also k, «k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k U Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k.1 and k-2 for k = the reverse of the two elementary reactions in the mechanism.
The following mechanism for the gas phase decomposition of oxygen difluoride is consistent with the observed rate law. step 1 fast: 2 OF2=0;F4 step 2 slow: 0,F4¬0; +2 F; (1) What is the cquation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. (2) Enter the formula of any species that acts as a reaction intermediate? If none leave box blank: (3) Complete the rate law for the overall reaction that is consistent with this mechanism. Use the form k[A]"|B]". , where 'I' is understood (so don't write it if it's a 'l') for m, n etc.
The gas phase reaction between hydrogen and iodine is proposed to occur as follows: step 1: 12 →21 step 2: step 2 H₂ + 2 I (a) Identify the molecularity of each step in the mechanism. step 1 → 2 HI + (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + (c) Identify any intemediates in this mechanism. Intermediate: Enter formula. If none, leave box blank:
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In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g)2 NO,(g) + ½ O2(g) the concentration of N2O5 was followed as a function of time. It was found that a graph of In[N,O3] versus time in seconds gave a straight line with a slope of -7.38×10-3 s and a y-intercept of -3.13. Based on this plot, the reaction is | order in N2O5 and the half life for the reaction i | seconds.
In a study of the gas phase decomposition of dinitrogen pentoxide at 335 K N2O5(g) 2 NO2(g) + ½ O2(g) the concentration of N,O5 was followed as a function of time. It was found that a graph of In[N½O5] versus time in seconds gave a straight line with a slope of -7.29×103 s and a y-intercept of -1.44. Based on this plot, the reaction is v order in N,Og and the rate constant for the reaction is Submit Answer Try Another Version 2 item attempts remaining
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Chlorine dioxide, Cl02, is a reddish-yellow gas that is soluble in water. In basic solution it gives Cl03- and CIO2 ions. 2C1O:(aq) + 20н (ад) —> СIО3 (aд) + CIO, (aq) + H;0(1) To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Initial Concentration Initial Concentration Initial Rate of Cl02 (mol/L) of OH (mol/L) (mol(L's) Exp. 1 0.21 1.6 x 10-2 0.162 Exp. 2 7.0 x 10-2 1.6 x 10-2 1.80 x 10-2 Exp. 3 7.0 x 10-2 4.8 x 10-2 5.39 х 10-2 a Obtain the rate law. (Use k for the rate constant.) Rate law =
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