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Reactant A can participate in both of these reactions:
1) A + B  C + D   Grxn = –15.6 kJ
2) A + E  F + G    Grxn = –20.5 kJ
Reaction 1 has a much higher rate than Reaction 2 under the same reaction conditions. Explain this observation in terms of activation energy.

Reactant A can participate in both of these reactions1 A B C D Grxn 156 kJ2 A E F G Grxn 205 kJReaction 1 has a much higher rate than Reaction 2 under the same class=

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The activation energy is the amount of energy required to initiate a certain reaction. The activation energy may considered as an "energy barrier" that has to be overcome in order for a reaction to begin. If a reaction has a lower activation energy, then it will occur more easily and at a faster rate than a reaction with a higher activation energy. Therefore, the reason that reaction 1 is faster than reaction 2 is because it has a lower activation energy than reaction 2.

The rate of reaction 1 is higher than the rate of reaction 2 because the activation energy of reaction 1 is lower than reaction 2.

Activation energy can be described as the energy required to initiate the reaction. The activation energy of the reaction is required to transmit the energy level of the substrate to convert into the product.

The value of activation energy has been independent of [tex]\rm \Delta G[/tex].

Thus for the reaction, the rate of reaction is higher, i.e. lower level of energy has been required to convert the reactant into the product. Thus, the activation energy of the reaction is lower.

The lower rate of reaction is because of the higher activation energy values.

Thus, the rate of reaction 1 is higher than the rate of reaction 2, because the activation energy of reaction 1 is lower than reaction 2.

For more information about the activation energy, refer to the link:

https://brainly.com/question/12558986

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