For the following two reactions,which stateme | vedclass

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(A) $1$. The rate of a reaction is inversely proportional to the activation energy $(E_a)$. $A$ lower activation energy means a faster reaction rate.$

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Reaction $A$ is faster and less exergonic than $B$

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(A) $1$. The rate of a reaction is inversely proportional to the activation energy $(E_a)$. $A$ lower activation energy means a faster reaction rate.$2$. From the provided energy profile diagrams,it is clear that the activation energy for reaction $A$ $(E_{a1})$ is lower than the activation energy for reaction $B$ $(E_{a2})$,i.e.,$E_{a1} $3$. Exergonic reactions are those where the free energy of the products is lower than that of the reactants (negative $\Delta G$). Both reactions are exergonic as the energy of the products is lower than the reactants.$4$. Comparing the overall energy change $(\Delta E)$,the drop in energy for reaction $B$ is greater than for reaction $A$,making reaction $B$ more exergonic than reaction $A$.$5$. Thus,reaction $A$ is faster,but reaction $B$ is more exergonic. This implies that reaction $A$ is faster and less exergonic than reaction $B$.

For the following two reactions,which statement is true?

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