Nitrous add HNO,) Slowly dtranaposce to NO, NO, 3 water by ttallMAng nd orderryn 2HNO,(A4) NO(4) +NOlg)+t Hall ces Voe me data belau to detemine the raare law 3 The ra e cansrant far This wn Time is) HNO) 0.1660 100 1500 2000 2600 U.1383 0.1345 0.1309 B000 1 Determine T rate Law For This renlDan rate= 2) Determine the rate canntTant fer thes Nm-1.1-+ Determine I nale like For the

Nitrous add HNO,) Slowly dtranaposce to NO, NO, 3 water by ttallMAng nd orderryn 2HNO,(A4) NO(4) +NOlg)+t Hall ces Voe me data belau to detemine the raare law 3 The ra e cansrant far This wn Time is) HNO) 0.1660 100 1500 2000 2600 U.1383 0.1345 0.1309 B000 1 Determine T rate Law For This renlDan rate= 2) Determine the rate canntTant fer thes Nm-1.1-+ Determine I nale like For the

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 53AP

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Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.
The oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) + ClO(aq) IO(aq) + Cl(aq) was studied at 25 C, and the following initial rates data (Y. Chia and R. E. Connick, Journal of Physical Chemistry, Vol. 63, p. 1518, 1959) were collected: (a) Determine the rate law for this reaction. (b) One mechanism that has been proposed for this reaction is the following: Show that the rate law predicted by this mechanism matches the experimentally determined rate law in part a. (Note that when writing the expression for K the equilibrium constant, [H2O] is not involved. See Chapter 15.)
The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
Show how equation 20.33 reduces to a simpler form of an integrated first-order rate law when the reverse reaction of an equilibrium is negligible.
Consider the following hypothetical reaction: 2AB2(g)A2(g)+2B2(g)A 500.0-mL flask is filled with 0.384 mol of AB2. The appearance of A2 is monitored at timed intervals. Assume that temperature and volume are kept constant. The data obtained are shown in the table below. (a) Make a similar table for the disappearance of AB2. (b) What is the average rate of disappearance of AB2 over the second and third 10-minute intervals? (c) What is the average rate of appearance of A2 between t=30 and t=50?
The gas-phase reaction between hydrogen and iodine H2(g)+I22HI(g)proceeds with a rate constant for the forward reaction at 700C of 138 L/moI s and an activation energy of 165 kJ/moI. (a) Calculate the activation energy of the reverse reaction given that H f for HI is 26.48 kJ/moI and H f for I2(g) is 62.44 kJ/mol. (b) Calculate the rate constant for the reverse reaction at 700C. (Assume A in the equation k=AeE a /RT is the same for both forward and reverse reactions.) (c) Calculate the rate of the reverse reaction if the concentration of HI is 0.200 M. The reverse reaction is second-order in HI.
For a certain reaction, Ea is 135 kJ and H=45 kJ. In the presence of a catalyst, the activation energy is 39% of that for the uncatalyzed reaction. Draw a diagram similar to Figure 11.14 but instead of showing two activated complexes (two humps) show only one activated complex (i.e., only one hump) for the reaction. What is the activation energy of the uncatalyzed reverse reaction?
For the reaction 2N2O5(g)4NO2(g)+O2(g) the following data were collected, where Rate=[N2O5]t Time (s) T = 338 K [N2O5] T=318K [N2O5] 0 1.00 101 M 1.00 101 M 100. 6.14 102 M 9.54 102 M 300 2.33 102 M 8.63 102 M 600. 5.41 1O3 M 7.43 102 M 900. 1.26 1O3 M 6.39 102 M Calculate Ea for tills reaction.
The rate of the reaction O(g)+NO2(g)NO(g)+O2(g) was studied at a certain temperature. a. In one experiment, NO2 was in large excess, at a concentration of 1.0 1013 molecules/cm3 with the following data collected: Time(s) [O](atoms/cm3) 0 5.0 109 1.0 102 1.9 109 2.0 102 6.8 108 3.0 102 2.5 108 What is the order of the reaction with respect to oxygen atoms? b. The reaction is known to be first order with respect to NO2 Determine the overall rate law and the value of the rate constant.
11.93 On a particular day, the ozone level in Milwaukee exceeded the EPAs 1-hour standard of 0.12 ppin by 10 ppb. How many ozone molecules would be present in 1 liter of air at the detection site?
Consider the reaction Mn+ + ne- ⇌ M. If ΔG*c = ΔG* + (1-α)nFE and η = E – Eeq, prove that ic = io exp[-(1-α)nFηa)/RT)].
In a study of the gas phase decomposition of hydrogen peroxide at 400 °CH2O2(g)H2O(g) + ½ O2(g)the concentration of H2O2 was followed as a function of time.It was found that a graph of 1/[H2O2] versus time in seconds gave a straight line with a slope of 1.03 M-1 s-1 and a y-intercept of 13.4 M-1.Based on this plot, the reaction is (frist, second, zero)__________ order in H2O2 and the rate constant for the reaction is _____________ M-1 s-1.