The reaction x-y is an exothermic reaction . Activation energy of the reaction for x into y is 150kjmol^--1 enthalpy of reaction os 135kjmol^-1 . The activation energy for the reverse reaction y-x will be
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In the case of an exothermic reaction, the activation energy of the forward reaction will always be smaller than the activation energy of the reverse reaction.
In your case, the forward reaction will look like this
A→B+heat
Since heat is released during the reaction, the product will have a lower energy than the reactant. You go from a higher energy level, as was the cse for A, to a lower energy level, as is the case for B.
The difference in energy between A and B will the enthalpy change of the reaction, ΔH.
Hope it will help you
In your case, the forward reaction will look like this
A→B+heat
Since heat is released during the reaction, the product will have a lower energy than the reactant. You go from a higher energy level, as was the cse for A, to a lower energy level, as is the case for B.
The difference in energy between A and B will the enthalpy change of the reaction, ΔH.
Hope it will help you
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Answer:
Explanation:
sarthaks.com/204757/an-endothermic-reaction-has-an-activation-energy-of-175-kj-mol-and-the-heat-of-reaction-is-85
This explains the best..I don't have much time...so I've put the link..
Don't mind..We all just want the answer..Not the source UwU
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