Consider the energy profile- for the reaction X -Y - R - S which of the following deduction about reaction is not correct-

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Activation Energy

Consider the ...

Question

Consider the energy profile, for the reaction $X + Y \to R + S$ which of the following deduction about reaction is not correct?

The energy of activation for the backward reaction is 80 KJ

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The forward reaction is Endothermic

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Δ H

for the forward reaction is 20 kJ

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The energy of activation for forward reaction is 60 kJ

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Solution

The correct option is A The energy of activation for the backward reaction is 80 KJ
$E_{F R}^{} = 80 - 20 = 60 K J$
$E_{B . R}^{} = 80 - 40 = 40 K J$
so [A] is not correct.
Where F.R.= forward reaction and B.R.=Backward reaction

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Consider the energy profile, for the reaction X+Y→R+S which of the following deduction about reaction is not correct?

The correct option is A The energy of activation for the backward reaction is 80 KJE∗FR=80−20=60KJE∗B.R=80−40=40KJso [A] is not correct.Where F.R.= forward reaction and B.R.=Backward reaction

Consider the energy profile, for the reaction $X + Y \to R + S$ which of the following deduction about reaction is not correct?

The correct option is A The energy of activation for the backward reaction is 80 KJ
$E_{F R}^{} = 80 - 20 = 60 K J$
$E_{B . R}^{} = 80 - 40 = 40 K J$
so [A] is not correct.
Where F.R.= forward reaction and B.R.=Backward reaction