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(A) From the given energy profile diagram:$1$. Energy of reactants $(E_R)$ = $20 \, kJ$$2$. Energy of products $(E_P)$ = $40 \, kJ$$3$. Threshold ener

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The energy of activation for the backward reaction is $80 \, kJ$

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(A) From the given energy profile diagram:$1$. Energy of reactants $(E_R)$ = $20 \, kJ$$2$. Energy of products $(E_P)$ = $40 \, kJ$$3$. Threshold energy $(E_T)$ = $80 \, kJ$Calculations:- Activation energy for forward reaction $(E_{a(f)})$ = $E_T - E_R = 80 - 20 = 60 \, kJ$- Activation energy for backward reaction $(E_{a(b)})$ = $E_T - E_P = 80 - 40 = 40 \, kJ$- Enthalpy change $(\Delta H)$ = $E_P - E_R = 40 - 20 = 20 \, kJ$Since $\Delta H > 0$,the reaction is endothermic.Evaluating the options:- Option $(A)$: $E_{a(b)} = 40 \, kJ$. The statement says $80 \, kJ$,which is incorrect.- Option $(B)$: Correct,as $\Delta H > 0$.- Option $(C)$: Correct,$\Delta H = 20 \, kJ$.- Option $(D)$: Correct,$E_{a(f)} = 60 \, kJ$.Therefore,the incorrect statement is $(A)$.

$Step$	$Rate\ Constant\ /\ Activation\ energy$
$Step\ 1$	$k_1, E_{a_1} = 180\ kJ/mol$
$Step\ 2$	$k_2, E_{a_2} = 80\ kJ/mol$
$Step\ 3$	$k_3, E_{a_3} = 50\ kJ/mol$

Consider the following energy profile for the reaction $X + Y \rightarrow R + S$. Which of the following deductions about the reaction is not correct?

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