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Based on their activation energies and energy changes and assuming that all collision factors are the same, which of the following reactions would be fastest in the reverse direction?

A) Ea= Ea3 = 54 kJ/mol , ΔE= ΔE3 = 8 kJ/mol .
B) Ea= Ea2 = 36 kJ/mol , ΔE= ΔE2 = -10 kJ/mol .
C) Ea= Ea1 = 45 kJ/mol , ΔE= ΔE1 = -25 kJ/mol .
D) Ea= 36 kJ/mol , ΔE= ΔE2 = -10 kJ/mol and Ea= 54 kJ/mol , ΔE= ΔE3 = 8 kJ/mol

Respuesta :

pstnonsonjoku

The reaction that has the fastest rate of reverse  reaction is the one in which Ea= Ea3 = 54 kJ/mol , ΔE= ΔE3 = 8 kJ/mol (Option A).

What is activation energy?

The term activation energy refers to the minimum energy that reactants must possess in order for their collision to result in a chemical reaction.

The higher the activation energy, the faster the reverse reaction. Hence the reaction that has the fastest rate of reaction is the one in which Ea= Ea3 = 54 kJ/mol , ΔE= ΔE3 = 8 kJ/mol (Option A).

Learn more about activation energy: https://brainly.com/question/11334504

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