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The rate constant of a reaction is 4.50x10⁻⁵ L/mols at 195°C and 3.20 × 10⁻³L/mol.s at 258°C. What is the activation energy of the reaction?

Respuesta :

The rate constant of a reaction is 4.50x10⁻⁵ L/mols at 195°C and 3.20 × 10⁻³L/mol. is at 258°C. Therefore, the activation energy of the reaction would be 3.82 J/mol

Here we have to calculate the activation energy.

Step 1

The activation energy (Ea) can be calculated by using the equation,

Given:

k1 = 0.76 s-1      t1 = 727°C = 273 +727 = 1000 K

k2 = 0.87 s-1      t2 = 757o C = 273+757 = 1030 K

Ea = ?

Now substitute all the values in the above equation,

Ea = 3.82 J/mol.

Thus the activation energy is found to be 3.8103 J/mol .

To learn more about activation energy here

brainly.com/question/11334504

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