Need help with number 2 I know the answer is Ea18x102 kJ but

Activation Energy Using a graphing calculator (or co mputer below for the decomposition of iodoethane to ethane and hydrogen iodide. 680. make an aPproprate Arrhenius plot of the data gi en 660. 7.2 × 104 | 2.2 × 10s | 1.7 × 10-1 720. 760. 0.11 a) Determine the activation energy for the reaction. b) Predict the value of the rate constant at 400. The rate constant of the second-onder reaction 2 HI@-h@ +@ is 2.4 x10° L.mol si at 575. K and 6.0 × 10, Ltnols\" at 630. K. Calculate the Activation Energy for this reaction. The rate constant of the reaction between CO, and OH in aqueous solution to give bicarbonate ion, HOOs, is 1.5 x 101° L-mols at 25 °C. Determine the rate constant at normal blood temperature (3789 if the activation energy s 38 kJmol· For the reaction profile shown below a) 4. What species are represented at points A, B, and C How many steps are in the overall reaction? How many transition state complexes are produced during the course of the reaction? e) Is the reaction endo- or exothermic? What is the rate-determining step of the reaction? 5. For the reaction profile below for the isomerization of air to a) What energies are represented by the numbers 2, 3, and 4 c) How many steps in the reaction mechanism What species is represented at point 1? Which is the rate-determining step? What is the fastest step? Is the reaction endo- or exothermic?

Solution

2. Using Arrhenius relation,

ln(k2/k1) = Ea/R[1/T1 - 1/T2]

with,

k1 = 2.4 x 10^-6 L.mol.s-1

k2 = 6.0 x 10^-5 L.mol.s-1

T1 = 575 K

T2 = 630 K

R = gas constant

Ea = activation energy

we get,

ln(6.0 x 10^-5/2.4 x 10^-6) = Ea/9.314[1/575 - 1/630]

Ea = 180 kJ (rounded off)

     = 1.80 x 10^2 kJ