The following data were obtained for the reaction2 CIO₂(aq) + 2 OH(aq) → CIO3(aq) + ClO₂ (aq) + H₂O(l)[CIO₂]0[OH-]oInitial Rate(mol/L)(mol/L)(mol L-1 s-¹)0.0540.1086.21X10-20.1080.1082.48X10-10.1080.0541.24X10-1What is the numerical value for the rate constant?

Given :- The given reaction is: 2ClO2 (aq) + 2OH- (aq) → ClO3- (aq) + ClO2- (g) + H2O (l)…

The following data were obtained for the reaction 2 CIO2(aq) + 2 OH (aq) → CIO3(aq) + ClO₂ (aq) + H₂O(l) [CIO₂]0 [OH-]o Initial Rate (mol/L) (mol/L) (mol L-¹ s-¹) 0.054 0.108 6.21X10-2 0.108 0.108 2.48X10-¹ 0.108 0.054 1.24X10-1 What is the numerical value for the rate constant?

The following data were obtained for the reaction 2 CIO2(aq) + 2 OH (aq) → CIO3(aq) + ClO₂ (aq) + H₂O(l) [CIO₂]0 [OH-]o Initial Rate (mol/L) (mol/L) (mol L-¹ s-¹) 0.054 0.108 6.21X10-2 0.108 0.108 2.48X10-¹ 0.108 0.054 1.24X10-1 What is the numerical value for the rate constant?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.32PAE: 11.32 The following experimental data were obtained for the reaction 2A + 3 B—C + 2D [A](mol L 1)...

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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?
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.
Experimental data are listed here for the reaction B: Time (s) IB] (mol/L) 0.00 0.000 10.0 0.326 20.0 0.572 30.0 0.750 40.0 0.890 Prepare a graph from these data, connect the points with a smooth line, and calculate the rate of change of [B] for each 10-s interval from 0.0 to 40.0 s. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. How is the rate of change of [AJ related to the rate of change of [B] in each time interval? Calculate the rate of change of [AJ for the time interval from 10.0 to 20.0 s. What is the instantaneous rate, A[B]/Ar, when [BI = 0.750 mol/L?
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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.
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Give the Arrhenius equation. Take the natural log of both sides and place this equation in the form of a straight-line equation (y = mx + b). What data would you need and how would you graph those data to get a linear relationship using the Arrhenius equation? What does the slope of the straight line equal? What does the y-intercept equal? What are the units of R in the Arrhenius equation? Explain how if you know the rate constant value at two different temperatures, you can determine the activation energy for the reaction.