The equation obtained from excel is: y=-4698.7x+27.872 The activation energy = 3

Question

The equation obtained from excel is: y=-4698.7x+27.872

The activation energy = 39.1 kJ/mol

I only need help with PART B: determining the rate constant for the reaction at temperature 34 C (using the information already obtained). Please answer question in units of M^-1 s^-1.

Thank you.

Part A The reaction between chlorine dioxide and ozone is relevant to the study of atmospheric ozone destruction. The value of the rate constant for the reaction was measured at four temperatures. The results are as follows: Calculate the activation energy for this reaction. (Hint: use Excel) T(K) Ik(M-1 s-1) 193 198 203 208 34.0 62.8 112.8 196.7 39.1 kJ/mol ous Answers Completed Part B Use the data generated in part A to answer part B Determine the rate constant for the reaction at 34 °C M-1s-1

Explanation / Answer

as per Arhenius equation, K = A*e(-E/RT), E is the activation energy , R = gas constant= 8.314 J/mole.K

A is frequency factor, T is temperature in Kelvin. K is the rate constant

taking ln, the equation becomes, lnK = lnA- E/RT, so a plot of lnK vs 1/T gives straight line whose slope is -E/R and intercept is lnK. from the given data, which can be interpreted as y= mx+C, where y is lnK, m is the slope -E/R and slope is C=lnA

given Equation becomes

the given equation y= -4698.7*1/T+27.872

the slope is -E/R= -4698.7, E= 4698.7*8.314 J/mole=39064 J/mole, 1000J= 1Kj, E= 39064/1000 Kj/mole= 39.1 Kj/mole

at T= 34 deg.c, converting this into K, T= 34+273= 307K

lnK(y)=-4687.7*1/307+27.872, K= 297142.6 /M.sec

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