A reaction with the activation energy Ea= 25.00 kJ/mol, has a rate constant k = 6.300 x 10-4 at 492.00 Kelvin. Determine the temperature required to increase the rate constant 3 times . R = 8.314 J K-1mol-1. Answer with the proper number of significant figures.

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Bunny GreenfelderLv2

20 Apr 2019

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Use the following equation and chart to make a graph and obtain E_a in kJ/mol for this data. [My main problem is setting up and solving the equation mostly because I don't know where A is comming from and I don't know what to put.]

ln(k)=(-E_a/R)(1/T)+ln(A)

k=rate constant

E_a=activation energy

R=gas constant, 8.314 J/(mol K)

T=temperature in Kelvin

A=Arrhenius constant

T(Kelvin)	k1(sec^-1)	k2(sec^-1)	k average(sec^-1)
300	71	67	69.0
320	112	99	105.5
290	59	58	58.5

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