Question

1. Write a rate law from the image below: TRANSITION STATES Ea(step 2) Ea(step 1) slow fast Potential energy NO2F+ F+NO2 2NO2 + F2 REACTANTS ΔΗ 'nxn <0 2NO2F PRODUCT Reaction progress A. Rate = k [NO2] B. Rate = k [NO2][F2] C. Rate = k [NO212[F2]

Answer 1

Option (B) is correct.

Remember from potential energy and reaction progress graph, Rate determining step will be that which have the highest activation energy. Step 1 is the slow step while step 2 is fast so step 1 will have more activation energy and it will be the rate determining step. Here in step1 transition state, there is collision between NO₂ and F₂ only so the rate law be,

Rate = K [ NO₂ ]¹ [F₂ ]¹ .

Hope you Understand the answer, basically what we had done is just look at that transition state which have highest activation energy, and note those compounds which are reacting at that state, and that will be filled in rate law.

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