The rate law for the reaction 2 NO (g) + Cl2 (g) ⇄ 2 NOCl (g) is given by the rate=k[NO][Cl2]. A mechanism involving these steps has been proposed for the reactionNO (g) + Cl2 (g) ⇄ NOCl2 (g)NOCl2 (g)+ NO (g) ⇄ 2 NOCl (g)(2a) If this mechanism is correct, what does it imply about the relative rates of these two steps (e.g. How do the rates of reaction compare? Which is slow?)(2b) What is the reaction intermediate in this mechanism?

Consider these three reactions as the elementary steps in the mechanism for a chemical reaction.(i) Cl2 (g) + Pt (s) à 2Cl (g) + Pt (s) Ea = 1550 kJ ∆H = – 950 kJ(ii) Cl (g)+ CO (g) + Pt (s) à ClCO (g) + Pt (s) Ea = 2240 kJ ∆H = 575 kJ(iii) Cl (g) + ClCO (g) à Cl2CO (g) Ea = 2350 kJ ∆H = – 825 kJ e. Which reaction intermediate would be considered a catalyst (if any) and why?f. If you were to add 2700kJ of activation energy to the reaction, would you be able to make thereaction reverse itself (i.e. have the products become reactants)? Justify your answer.g. If you were to added a positive catalyst to step (iii) what would the end result be? Justify yourprediction.h. Your friend is looking at your graph and states that she believes that step (ii) is the ratedetermining step. Do you agree with her? Justify your reasoning.

In a steady-state approximation, it is assumed that     the concentrations of the reactants remain constant and small throughout the reaction.     the concentration of the product remains constant and large throughout the reaction.     The concentration of the product remains unchanged and small throughout the reaction.     the concentration of the reaction intermediates remains constant and small throughout the reaction.   there is no more information that is needed for this question.

The rate constant of a chemical reaction increased from 0.100 s−1 to 3.20 s−1 upon raising the temperature from 25.0 ∘C to 55.0 ∘C . Calculate the value of (1T2−1T1) where T1 is the initial temperature and T2 is the final temperature. Express your answer numerically.

A + B yields C + D D + 2A yields E + F F + A yields G + B What is the molecularity of the second step? Write the overall reaction equation: What molecule(s) is (are) the intermediates? What molecule(s) is (are) the catalysis?

The rate of a reaction increases by 4 times when temperature of the reaction is raised from 340K to 360K. Calculate the energy of activation of the reaction. [Given: R = 8.314 JK¹ mol¹].