Question required to be answered: 'For Practice 13.8' with step-by-step solution. ANS: 6.13*10^-4 L/mol s

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EXAMPLE 13.8 USING THE TWO-POINT FORM OF THE ARRHENIUS EQUATION Consider the reaction between nitrogen dioxide and carbon monoxide: NO2(g)+CO(g)NO(g)+CO2(g) The rate constant at 701K is measured as 2.57Lmol1s1 and that at 895K is measured as 567Lmol1s1. Find the activation energy for the reaction in kJmol1. FIND: Ea STRATEGIZE Use the two-point form of the Arrhenius equation, which relates the activation energy to the given infor- mation and R (a constant). EQUATION lnk1k2=REa(T21T11) SOLVE Substitute the two rate peratures into the equation. Solve the equation for Ea, the activation energy, and convert to kJmol1. SOLUTIONln2.57LmOl1s1567LmOl1s1=REa(895K1701K1)5.40=REa(K3.09104) Ea=5.40(3.09104K)R=5.40(3.09104K)8.314molKJ=1.45105Jmol1=145kJmol1 CHECK The magnitude of the answer is reasonable. Activation energies for most reactions range from tens to hundreds of kilojoules per mole. FOR PRACTICE 13.8 Use the results from Example 13.8 and the given rate constant of the reaction at either of the two temperatures to predict the rate constant at 525K