A chemical reaction has an energy of activation Ea = 1∙104 J mol-1 at T = 300 K. The first-order rate constant for this reaction was found to be 15.0 s-1. In the presence of a catalyst, the activation energy is reduced to 1∙103 J mol-1. Calculate the pre-exponential factor in the Arrhenius equation

Answer : The pre-exponential factor in the Arrhenius equation is, 14.99  s⁻¹

Explanation :

Using Arrhenius equation,

Taking ln on both the sides, we get:

where,

K = rate constant =

Ea = activation energy = 1.104 J/mol

T = temperature = 300 K

R = gas constant = 8.314 J/mole.K

A = Arrhenius constant

Now put all the given values in the above formula, we get the value of \ln a.

Therefore, the pre-exponential factor in the Arrhenius equation is, 14.99  s⁻¹

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-

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