Consider the following chemical equation: Overall Reaction: A2 + B2 → 2 AB  The proposed mechanism is as follows: A2 ⇋  2A  (fast) 2A + B2 → 2AB (slow) What is the rate law

Consider the following reaction for chlorine reacting with chloroform, Cl2 (g) + CHCIl3 (g) HС (g) + СCla (g) a) based on the initial rate data provided (in the table below), determine the rate law for this reaction. b) The following is a proposed mechanism for this reaction. Cl2 (g) = 2 CI (g) CI (g) + CHCI: (g) → HCI (g) + CCl: (g) (slow) CCl: (g) + CI (g) > Сle (g) (fast equilibrium) (fast) Is this an acceptable mechanism based on the rate law you determined in part a? answer should be Yes/No to "is this an acceptable mechanism") Initial Rate [CI,] [CHCI3] 0.00253 | 0.2 0.3 A) Yes 0.00759 0.2 0.9 B) No 0.00506 0.8 0.3

The formation of ammonia is one of the most important processes in the chemical industry: N₂(g) +3 H₂ (g) → 2 NH₃ (g) Express the rate in terms of changes in [N₂], [H₂], and [NH₃].

Nitrogen(II) oxide, NO, reacts with hydrogen, H2, according to the following equation: 2 NO + 2 H2 - N2 + 2 H20 What would the rate law be if the reaction mechanism occurs in the following steps: Step 1:2 NO + H2 - N2 + H,O2 Step 2: H,02 + H2-2 H20 O rate = k[H2O2]H2] O rate = k[H2O2]|N2] O rate = k[NO]°[H2] O rate = k[H2O]*