ALT Transcribed Text: (2,\mathrm{NO_2(g)} + \mathrm{F_2(g)} \rightarrow 2,\mathrm{NO_2F(g)}) It is proposed that the reaction represented above proceeds via the mechanism represented by the two elementary steps shown below. Step I: (\mathrm{NO_2 + F_2 \rightarrow NO_2F + F}) (slow) Step II: (\mathrm{NO_2 + F \rightleftharpoons NO_2F}) (fast reversible) 1.) Which of the following is the most likely rate law for this proposed mechanism? (A) (\mathrm{rate = k[NO_2F][F]}) (B) (\mathrm{rate = k[NO_2]^2[F_2]}) (C) (\mathrm{rate = k[NO_2F]}) (D) (\mathrm{rate = k[NO_2][F]^2})

ALT Questions 2 & 3 refer to the proposed mechanism below Nitrogen dioxide, NO₂(g), is produced as a by-product of the combustion of fossil fuels in internal combustion engines. At elevated temperatures NO₂(g) decomposes according to the equation below. 2 NO₂(g) → 2 NO(g) + O₂(g) Below is a proposed mechanism for this reaction Step 1: NO₂(g) + NO₂(g) → NO(g) + NO₃(g) slow Step 2: NO₃(g) → NO(g) + O₂(g) fast 2.) Which of the diagrams below most likely represents an effective collision for the first step of this mechanism to occur? Nitrogen Oxygen (A) Shows an alignment between two Oxygen atoms on the two NO₂ molecules (B) Shows an alignment between two Nitrogen atoms on the two NO₂ molecules (C) Shows an alignment between the Nitrogen atom on the one of the NO₂ molecules with the Oxygen atom on the the other (D) Shows an alignment between the Nitrogen atom on the one of the NO₂ molecules with an Oxygen on a molecule of O₂

ALT Transcribed Text: 3.) What is the intermediate for the proposed mechanism? (A) NO(g) (B) NO₂(g) (C) NO₃(g) (D) O₂(g)