Catalyzed: In the catalyzed reaction an iodine radical attacks the double bond a

ID: 1050757 • Letter: C

Question

Catalyzed:

In the catalyzed reaction an iodine radical attacks the double bond and breaks the pi bond by forming a C-I bond. The molecule now has a C-C single bond. Rotation around single bonds occur spontaneously at room temperature. The molecule assumes the trans configuration, because this is sterically the more stable configuration. Trans-2-butene forms by giving off an iodine radical which recombines with another one to form iodine.

Mark each of the following statements either True or False.

True False  In the diagram above, 4 indicates the activation energy of the uncatalyzed reverse reaction.

True False  The position indicated by the number 5 shows the energy of an intermediate.

True False  The catalyzed reaction has a lower activation energy, because the reaction takes a different pathway.

True False  The free energy change is the same for both reaction pathways.

True False  The difference between the activation energies of the uncatalyzed forward and reverse reactions is equal to the difference between the free energies of products and reactants.

True False  The activation energy of the uncatalyzed forward reaction is about 280 kJ/mol.

300T catalyzed reaction Energy (kJimol) 4 uncatalyzed reaction 3 2 5 cis-C4H8 + ½ 12 trans-C4H8 + ½ 12 reactants products reaction coordinate

Explanation / Answer

The uncatalyzed reacation having the high activation energy whereas the catalysed reactions have less activation energy.

3 indicates the activation energy of the uncatalyzed forqard reaction

4 indicates the activation energy of the uncatalyzed reverse reaction.

hence, the given statement is TRUE.

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The position indicated by the number 5 shows the energy of an intermediate.