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The reversible liquid phase reaction A+BB+B (Equation 1) obeys the following rate equation rA=k(CACBKecBCs) (Equation 2) It is known that the value of equilibrium constant Ke for the reaction is 500@100 C and that the value of heat of reaction (HR)is 60kJmol1 and is constant between 30C and 300C, with R=8.314JK1mol1. It is known that the value of the rate constant k is 0.050Lmol1h1@100C (where h is hours) and that the rate constant has an activation energy of 80kJmol1. (a) Write the Van't Hoff equation used to compute Ke as a function of T. [2 mark] (b) Using this equation, calculate the value of the equilibrium constant calculate the rate constant between 50C and 250C in steps of 50C. Show the results in a table for the different temperatures. [5 marks] (c) Using a derivation, show that for a rate equation of the form shown in Equation 1,Ke is related to the equilibrium conversion, XAe, by the following equations: (i) Ke=(1XAe)2(XAe)2 (Equation 3) [3 marks] from which we can obtain the following relationship (ii) XAe=(1+Ke)Ke (Equation 4) [4 marks] (d) Using values of K at different temperatures, calculate the equilibrium conversion constant 50C and 250C in steps of 50C. Show the results in a table for the different temperatures. [5 marks] (e) Is the reaction exothermic or endothermic? Justify your answer. [2 marks] (f) Does the behaviour of K and XAe support the enthalpy changes of the reaction? Explain your answer. [4 marks]