Problem: For the first-order reaction 1/2 N2O4(g) → NO2(g); ∆H = 28 kJ/molthe activation energy is 53 kJ/mol. What is the activation energy for the reverse reaction?A) -25 kJ/molB) 81 kJ/molC) –53 kJ/molD) 25 kJ/molE) 53 kJ/mol

FREE Expert Solution

We’re being asked to determine the activation energy for the reverse reaction.


We’re given the following information:

ΔH = 28 kJ/mol: Recall that the change in enthalpy (ΔH) is the difference in energy between products and reactants. ΔH for the reaction is positive, which means we have an endothermic reaction. This signifies that the products are higher in energy than the reactants.

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Problem Details

For the first-order reaction 1/2 N2O4(g) → NO2(g); ∆H = 28 kJ/mol

the activation energy is 53 kJ/mol. What is the activation energy for the reverse reaction?

A) -25 kJ/mol

B) 81 kJ/mol

C) –53 kJ/mol

D) 25 kJ/mol

E) 53 kJ/mol

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What scientific concept do you need to know in order to solve this problem?

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