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11 Nov 2019
The reaction 2 NOCl (g) rightarrow 2 NO (g) + Cl_2 (g) has an Ea of l.00 times 10^2 kJ/mol and a rote constant of 0 286 L mol^-1s^-1 at 500. K. What is the rate constant at 490. K? Understanding the high-temperature formation and breakdown of the nitrogen oxides is essential for controlling the pollutants generated by car engines. The second-order reaction for the breakdown of nitric oxide, NO, to its elements has rate constants of 0.0796 L mol^-1 s^-1 at 737 degree C and 0.0815 L mol^-1 s^-1 at 947 degree C. What is the activation energy of this reaction? For the reaction A_2(g) + B_2(g) rightarrow 2 AB (g), Ea_(fwd) = 125 kJ/mol and Ea_(rev) = 85 kJ/mol. Assuming the reaction occurs in one step... a. Draw the reaction energy diagram. Label: the axes, reactants, products, Ea_(fwd), Ea_(rev), delta Hrxn, transition state b. Calculate delta Hrxn. Is the reaction endo-or exothermic? c. Sketch the structure of a possible transition state for the reaction between A_2 and B_2. The decomposition of hydrogen peroxide into water and oxygen gas occurs very slowly on its own. But the rate of decomposition is catalyzed by iodide. The reaction mechanism for the iodide-catalyzed decomposition of hydrogen peroxide is: H_2O_2 + gamma rightarrow H_2O + IO^- IO^- + H_2O_2 rightarrow H_O + O_2 + gamma a. What are the intermediates in the mechanism above? What do intermediates have in common with each other? b. As far as being produced and being consumed go, how does a catalyst compare to an intermediate? c. Are intermediates part of the overall chemical reaction? Are catalysts? d. Concerning the iodide-catalyzed decomposition of hydrogen peroxide, k_1
The reaction 2 NOCl (g) rightarrow 2 NO (g) + Cl_2 (g) has an Ea of l.00 times 10^2 kJ/mol and a rote constant of 0 286 L mol^-1s^-1 at 500. K. What is the rate constant at 490. K? Understanding the high-temperature formation and breakdown of the nitrogen oxides is essential for controlling the pollutants generated by car engines. The second-order reaction for the breakdown of nitric oxide, NO, to its elements has rate constants of 0.0796 L mol^-1 s^-1 at 737 degree C and 0.0815 L mol^-1 s^-1 at 947 degree C. What is the activation energy of this reaction? For the reaction A_2(g) + B_2(g) rightarrow 2 AB (g), Ea_(fwd) = 125 kJ/mol and Ea_(rev) = 85 kJ/mol. Assuming the reaction occurs in one step... a. Draw the reaction energy diagram. Label: the axes, reactants, products, Ea_(fwd), Ea_(rev), delta Hrxn, transition state b. Calculate delta Hrxn. Is the reaction endo-or exothermic? c. Sketch the structure of a possible transition state for the reaction between A_2 and B_2. The decomposition of hydrogen peroxide into water and oxygen gas occurs very slowly on its own. But the rate of decomposition is catalyzed by iodide. The reaction mechanism for the iodide-catalyzed decomposition of hydrogen peroxide is: H_2O_2 + gamma rightarrow H_2O + IO^- IO^- + H_2O_2 rightarrow H_O + O_2 + gamma a. What are the intermediates in the mechanism above? What do intermediates have in common with each other? b. As far as being produced and being consumed go, how does a catalyst compare to an intermediate? c. Are intermediates part of the overall chemical reaction? Are catalysts? d. Concerning the iodide-catalyzed decomposition of hydrogen peroxide, k_1
Nestor RutherfordLv2
8 Feb 2019