Instructions to follow • Solution is accepted in Handwritten format on a white A4 unruled sheet • Detailed and explained solution Avoid Al or plagiarism of any kind Q2 b. The selective oxidation of butan-2-one, B, produces diacetyl, D, over a vanadium phosphorus oxide catalyst by way of the following reaction: CH3COC2H5 (g) + O2(g) = CH3COCOCH3(g) + H2O(g) B Ꭰ Under certain experimental conditions the reaction appears to involve a Langmuir-Hinshelwood mechanism, with non-dissociatively adsorbed reactants: B(g) B(ad) O2(g) 02 (ad) B(ad) + O2(ad) → 'free'products (3.1) (3.2) (3.3) where 'free' products represents CH3COCOCH3(g) + H2O(g) which both desorb as quickly as they are formed. i. Identify which of the reactions (3.1 - 3.3) in the mechanism is the rate-limiting step if the reaction were to obey a Langmuir-Hinshelwood mechanism. (1 mark) ii. Write down the rate equation for this reaction and hence show that the theoretical rate equation is given by: dpB dpo₂ = ke T dt dt bBPB bo₂ Po₂ (1+bBB + bo₂Po₂)² where ko is the theoretical rate constant. You should explain why it is not necessary to include terms for the products in your equation. (7 marks) iii. At high partial pressure of butan-2-one, the experimental rate equation is given by: T = dpB dt dpokR dt PO₂ = PB (3.4) (3.5) where KR is the experimental rate constant. Show how this is consistent with the theoretical rate equation (Equation 3.4). [Hint: Remember to relate KR to ko in your answer.] (4 marks) iv. What other experimental condition would enable reduction of the theoretical rate equation to be consistent with this experimental rate equation (Equation 3.5) (one sentence)? (1 mark)