The reaction 2NO(g)+ O₂(g)$\rightarrow$2NO₂(g)has $\Delta$H_r $\circ$ = -114 kJ.mol^-1.A possible mechanism for this reaction is 2NO(g) →N₂O₂(g) Rapid equilibrium,K N₂O₂(g)+ O₂(g)$\rightarrow$2NO₂(g) Slow,k If the activation energy for the reverse reaction is 225 kJ.mol^-1,what is the activation energy for the forward reaction?

Question

Quizplus · Accepted Answer

The activation energy for the forward reaction is equal to the difference between the activation energy for the reverse reaction and the enthalpy change for the reaction. Therefore, the activation energy for the forward reaction is 225 kJ.mol^-1 - 114 kJ.mol^-1 = 111 kJ.mol^-1.

The Reaction 2NO(g)+ O2(g) →\rightarrow→ 2NO2(g)has Δ\DeltaΔ Hr ∘\circ∘ = -114 KJ →\rightarrow→ 2NO2(g) Slow,k If the Activation Energy for the Reverse Reaction

The Reaction 2NO(g)+ O₂(g) $\rightarrow$ 2NO₂(g)has $\Delta$ H_r^$\circ$= -114 KJ $\rightarrow$ 2NO₂(g)
Slow,k
If the Activation Energy for the Reverse Reaction