Question #193533

Draw an energy diagram for a reaction that starts with reactions whose energy is 20.0

kJ and has a ΔH of 20.0 kJ. The activation energy for the reaction is 35.0 kJ

1
2021-05-17T04:09:30-0400

Let make two coordinate in which horizontal one represent the Reaction coordinate and the vertical one represent the Energy (KJ)

Mark 0,10,20,30,40,50,60 on the vertical coordinate

Now draw a horizontal line at 0 KJ for the product.(Named as Product)

As the reaction starts from 20 KJ so draw a horizontal line at 20 KJ .(Named as Reactants)

As activation energy is 35 KJ SO make horizontal line 35 KJ above the Reactant line i.e draw a horizontal line at 55 KJ. (Named as Transition state.)

Now the difference between reactant and product line is "\\Delta H_r=20 kJ"

And difference between reactant and transition state is "\\Delta E_{act}=35kJ" .

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