5. The above reaction was conducted at different initial concentrations of A and B and each time the initial rates of the reaction were determined (table 1) Table 1 Trial# 12 ● 3 [A] (M) 0.01 0.01 0.02 [B] (M) 181 (M) 0.02 0.04 0.01 The overall rate of the reaction = k [A]m [B]" Using the information on the table above explain: eta from which traits did you use and why? a) Is the reaction rate dependent on the concentration of A? the reaction By what factor the concentration of A changed? Overall rate (mol/sec) 0.001 0.004 0.002 0.002 . By what factor the overall reaction rate changed? • Is the reaction O-order with respect to A/is m =0? If not explain why? ils did you use? b) Is the reaction rate dependent on the concentration of B? down rate of the reaction= . By what factor the concentration of B changed? ● what factor the overall reaction rate changed? • Is the reaction 0-order with respect to B/is n = 0? If not explain why?

5. The above reaction was conducted at different initial concentrations of A and B and each time the initial rates of the reaction were determined (table 1) Table 1 Trial# 12 ● 3 [A] (M) 0.01 0.01 0.02 [B] (M) 181 (M) 0.02 0.04 0.01 The overall rate of the reaction = k [A]m [B]" Using the information on the table above explain: eta from which traits did you use and why? a) Is the reaction rate dependent on the concentration of A? the reaction By what factor the concentration of A changed? Overall rate (mol/sec) 0.001 0.004 0.002 0.002 . By what factor the overall reaction rate changed? • Is the reaction O-order with respect to A/is m =0? If not explain why? ils did you use? b) Is the reaction rate dependent on the concentration of B? down rate of the reaction= . By what factor the concentration of B changed? ● what factor the overall reaction rate changed? • Is the reaction 0-order with respect to B/is n = 0? If not explain why?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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In general, can we predict the effect of doubling the concentration of A on the rate of the overall reaction A+BC? Can we predict the effect if the reaction is known to be an elementary reaction?
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
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?
Why awe elementary reactions involving three or more reactants very uncommon?
7-35 A reaction has a high rate constant but a small equilibrium constant. What does this mean in terms of producing an industrial product?
The reaction H2SeO3(aq) + 6I-(aq) + 4H+(aq) Se(s) + 2I-3(aq) + 3H2O(l) was studied at 0C, and the following data were obtained: [H2SeO3]0 (mol/L) [H+]0 (mol/L) [I]0(mol/L) Initial Rate (mol/L s) 1.0 104 2.0 102 2.0 102 1.66 107 2.0 104 2.0 102 2.0 10-2 3.33 107 3.0 104 2.0 102 2.0 102 4.99 107 1.0 104 4.0 102 2.0 102 6.66 107 1.0 104 1.0 102 2.0 102 0.42 107 1.0 104 2.0 102 4.0 102 13.2 107 1.0 104 1.0 102 4.0 102 3.36 107 These relationships hold only if there is a very small amount of I3 present. What is the rate law and the value of the rate constant? (Assumethatrate=[H2SeO3]t)
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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?
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
For each of the following reaction diagrams, estimate the activation energy (Ea) of the reaction:
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.
The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.