Consider the reaction data.AproductsT (K) | k (s-1)3250.3838250.611What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, useat least three significant figures in all values.X1Yi =X2 =Y2 =Determine the rise, run, and slope of the line formed by these points.rise:run:slope:What is the activation energy of this reaction?EaJ/mol?II

The explanation is given below-

Answered: Consider the reaction data. A →…

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 66AP

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For the decomposition of Ag2O: 2Ag2O(s)4Ag(s)+O2(g)(a) Obtain an expression for G as a function of temperature. Prepare a table of G values at 100 K intervals between 100 K and 500 K. b) Calculate the temperature at which G =0.
For the given chemical equilibrium, these data are determined experimentally: T K 350K 3.76102 450K 1.86101 Determine H for this reaction.
Consider the system A(g)+2B(g)+C(g)2D(g)at 25C. At zero time, only A, B, and C are present. The reaction reaches equilibrium 10 min after the reaction is initiated. Partial pressures of A, B, and D are written as PA, PB, and PD. Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required). (a) PD at 11 min PD at 12 min. (b) PA at 5 min PA at 7 min. (c) K for the forward reaction K for the reverse reaction. (d) At equilibrium, K Q. (e) After the system is at equilibrium, more of gas B is added. After the system returns to equilibrium, K before the addition of B K after the addition of B. (f) The same reaction is initiated, this time with a catalyst K for the system without a catalyst the system with a catalyst. (g) K for the formation of one mole of D K for the formation of two moles of D. (h) The temperature of the system is increased to 35C. PB at equilibrium at 25C PB at equilibrium at 35C. (i) Ten more grams of C are added to the system. PB before the addition of C PB after the addition of C.
Zn Zn2+(1.0M) Cu2+ (1.00M) Cu Ecell meausremet 1.029 Ecell, reaction quotient, Eºcell
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Consider the reaction data. A⟶productsA⟶products ? (?)T (K) ? (?−1)k (s−1) 275275 0.3800.380 675675 0.7470.747 a)What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all value x1=? x2=? y1=? y2=? b)Determine the rise, run, and slope of the line formed by these points. c)What is the activation energy of this reaction?
Bromine, Br2, reacts with chlorine, Cl2, in a tetrachloromethane, CCI4, solution to form bromine monochloride, BrCI. At equilibrium, the concentrations of Br2, Cl2, and BrCI in a reaction mixture were found to be 0.048 mol dm-3, 0.037 mol dm-3, and 0.111 mol dm-3, respectively, at 298 K. Calculate the equilibrium constant in terms of concentration, Kc, at this temperature.
A. For a certain reaction, Kc = 4.48×106 and kf= 4.10×10−2 M−2⋅s-1 . Calculate the value of the reverse rate constant, kr, given that the reverse reaction is of the same molecularity as the forward reaction. Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋅s−1nclude ⋅⋅ (multiplication dot) between each measurement. B. For a different reaction, Kc = 97.7, kf=3.00×10^3s−1 and kf=3.00×10^3s−1 , and kr= 30.7 s−1. Adding a catalyst increases the forward rate constant to 1.37×106 s−1s−1 . What is the new value of the reverse reaction constant, kr, after adding catalyst? Express your answer with the appropriate units. Include explicit multiplication within units, for example to enter M−2⋅s−1 include ⋅ (multiplication dot) between each measurement.
Consider the reaction network of the gaseous isomerisation, decomposition anddimerisation reactions of the same reactant A:Isomerisation: A ⇆ IDecomposition: A ⇆ B + CDimerisation: 2A ⇆ DAt the reaction temperature, the equilibrium constants, expressed in terms of partial pressures, are:Isomerisation: KI = 5Decomposition: KDe = 0.5 barDimerisation: KDi = 5 bar-1At 1 bar, there is only 1 mol of A initially. Express the mole-fraction of each reaction component at equilibrium as function of the extents of the three reactions at equilibrium, ξI, ξDe, ξDi.Calculations resulted in the following values of the extents of the three reactions, isomerisation, decomposition and dimerization at equilibrium: ξI= 0.5400 mol, ξDe =0.2553 mol, ξDi= 0.0483 mol.Calculate the equilibrium mole-fractions of reaction components A, I, B, C and D and show that the equilibrium extent values are correct.
Consider the reaction data. A⟶products ? (?) k (s−1) 275 0.384 775 0.730 What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use at least three significant figures in all values.
Consider the reaction order. A ---->products T (K) k (s^-1) 275 0.370 725 0.685
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