-1S8. A first-order reaction is performed twice at two different temperatures. The first run wasperformed at 40 K and was found to have a rate constant of 1.01 x 10-¹0 s¹. The second runwas performed at 300 K and was found to have a rate constant of 3.45 x 10-2 s¹. What is theactivation energy (in kJ molto two decimal places) for this reaction?SA: 7.54

Answered: Image /qna-images/answer/21433570-4eb8-4000-a1f2-7530b137bf3f.jpg

8. A first-order reaction is performed twice at two different temperatures. The first run was performed at 40 K and was found to have a rate constant of 1.01 x 10-10 s-1. The second run was performed at 300 K and was found to have a rate constant of 3.45 x 10-2 s-¹. What is the activation energy (in kJ mol-¹ to two decimal places) for this reaction? S -1

8. A first-order reaction is performed twice at two different temperatures. The first run was performed at 40 K and was found to have a rate constant of 1.01 x 10-10 s-1. The second run was performed at 300 K and was found to have a rate constant of 3.45 x 10-2 s-¹. What is the activation energy (in kJ mol-¹ to two decimal places) for this reaction? S -1

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.1: Reaction Rate

Problem 11.2CE: Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of...

See similar textbooks

Similar questions

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 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.
Given the 1st order rxn A(g) --- > B(g) + C(g) + 3D(g) with a rate constant of 6.0x10-4 s-1 at 298 K. With a starting mol of 1.00 mol of A(g), how long in seconds does it decrease to 0.500 mol?
The rate of a first-order reaction is followed by spectroscopy,monitoring the absorbance of a colored reactant at 520 nm.The reaction occurs in a 1.00-cm sample cell, and the onlycolored species in the reaction has an extinction coefficientof 5.60 x 103 M-1 cm-1 at 520 nm. (a) Calculate the initialconcentration of the colored reactant if the absorbance is0.605 at the beginning of the reaction. (b) The absorbancefalls to 0.250 at 30.0 min. Calculate the rate constant inunits of s - 1. (c) Calculate the half-life of the reaction.(d) How long does it take for the absorbance to fall to 0.100?
The rate constant for the fi rst-order decomposition of N2O5 in the reaction 2 N2 O5(g) → 4 NO2(g) + O2(g) with v = kr[N2O5] is kr = 3.38 x 10-5 s-1 at 25 oC. What is the ha lf- life of N2O5? What w ill be the total pressure, init ial ly 78.4 kPa for the pure N2O5 vapour, (a) 5.0 s, (b) 5.0 min after init iation of the reaction?
Why may some gas-phase reactions show fi rst-order kinetics?
The recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 1.7E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.22E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2kt Give the answer to 3 significant figures
A first-order reaction A → products is to be carried out in a CMFR.The reaction rate constant was determined to be 1.0 h−1. What is the residence time required for 90 percent conversion of the reactantprovided there are no changes in temperature and density of thesystem?
2A + B -> products, rate = k[A]-1 what is the derived expression for half-life with respect to A in terms of ? and [A]o?
How long would it take for a first-order reaction with a rate constant of5.30 X 10-4 s-1 to reach 70% completion?
For a type II second-order reaction, the reaction is 60% complete in 60 seconds when [A]0 =0.1 M and [B]0 = 0.5 M.a) What is the rate constant for this reaction?b) Will the time for the reaction to reach 60% completion change if the initial reactantconcentrations are decreased by a factor of two?
An irreversible unimolecular reaction (A -> B) has a rate constant (k) equal to 0.46 s-1. What is the half-time (t1/2)? If at time “zero” the concentration of A is 28 mM, what is the concentration at 1.5 seconds? At 2.17 seconds? Specify your units. t1/2 = [A] at t1/2 = [A] = at t = 2.17 s