Calculate the activation energy Ea in kilojoules per mole?
Using the Arrhenius equation, k=Ae^(-Ea/RT), where A is collision frequency Ea is activation energy R is a constant equal to 8.314 J/K *mol and T is temparature in Kelvin which becomes a linear/slope equation when its natural logarithm is taken, yielding ln k= ln A- Ea/RT, which when rearranged, ln k= (-Ea/R)(1/T)+ln A (Equation1) We plot this into a graph with the values: 2.76X10^ -5 then -10.497 then 298 then 0.00335 6.65 X10^-4 then -7.315 then 323 then 0.00309 NOTE: First row, k Second row, ln k 3rd row: Temp 4th row: Reciprocal You can get the slope, with 1/T at the x axis… slope= -10.497-(-7.315)/(0.00335-0.00309) You get: -12238.461 K multiply by R and you get: -101 750.569 J/mol Divide this by 100 and you get the kJ/mol value… Problem 2: Get the ln of A by substituting the value of the slope you found earlier (-12238.461 K), and the values of 1/T and k of one of the conditions into the linear equation (Equation 1). When you already know ln A, you can subsitute this value to
