The activation energy Ea for a particular reaction is50.0 kJ/mol. How much faster is the reaction at 317K than at 310.0 K? (R = 8.314 J/mol • K)

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Answered: The activation energy Ea for a…

Chemistry

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ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 79E: Old-fashioned smelling salts consist of ammonium carbonate, (NH4)2CO3. The reaction for the...

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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.
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 a. Draw the potential energy diagram for the reaction. Label the data points for clarity.The potential energy of the reactants is 600 kJ. b. What is the overall chemical equation? c. What is the overall change in enthalpy for the above chemical reaction? d. What is the overall amount of activation energy for the above chemical reaction? 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 the reaction 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…
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.

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The activation energy Ea for a particular reaction is 50.0 kJ/mol. How much faster is the reaction at 317 K than at 310.0 K? (R = 8.314 J/mol • K)