1) 2A B + C Two trials of the above reaction are run with the same initial conce

Question

1) 2A B + C

Two trials of the above reaction are run with the same initial concentration of A. The first trial is performed at 25oC and the second at 35oC. If the rate constant at 25oC is 0.537 M/min, what is the rate constant in the second trial if the reaction has an activation energy of 31.3 kJ/mol?

2

Consider the following reaction: NO2(g) + CO(g) NO(g) + CO2(g) a

Two trials of the above reaction are run with the same initial concentrations.

The first trial is performed at 700. K and the second at 800. K. If the rate constant at 700 K is 1.09 1/Ms and at 800 K is 23.3 1/Ms, what is the activation energy in kJ/mol?

Explanation / Answer

Bothe the questions are based on Arrhenius equation k = A e-Ea/RT

and in logarithmic form log (k2/k1) = (Ea /2.303R) [1/T1 -1/T2]

Q1) substituting T1= 25 C = 298K , T2 = 35C = 308 K , Ez = 31.3kJ = 31.3 x1000J

and k1 = 0.537 M/min

we have log (k2/0.537) = 31.3x1000J/(2.303x8.314J) [10/298x308]

= 0.1781

and k2 = 0.8092 M/min

Q2)

Here T1= 700k T2= 800K and k1 = 1.091 and k2 = 23.31

log (23.31/1.09) = Ea /(8.314x2.303)[100/700x800]

thus Ea = 142575.7 J

= 142.58kJ/mol

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