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8. The enthalpy of formation of 02(g) is: Select one: a. negative b. impossible to tell...
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step...
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step N2048) -> NO(g) + NO3(g) Slow NO3(g) NO) + O2(g) Fast The target rate law is rate = k (NO2)2 The target reaction is 2NO2(e) 2NON + O2) A. Write the rate law expected for this mechanism: B. What is the rate-determining step? C. What is the overall balanced equation for this mechanism? D. If there is/are a reactive intermediate(s), which is/are they? E....
[17 Marks Q 2(b) The rate equation for the reaction 2NO + O2 -» 2NO2 was...
[17 Marks Q 2(b) The rate equation for the reaction 2NO + O2 -» 2NO2 was determined experimentally to be Rate kINO] [02]. Two mechanisms have been proposed for this reaction: Mechanism A Mechanism B 2NO N202 NO O2 NO3 NO3 + NO → 2NO2 N202 O22NO2 (i) Determine the rate equation for the formation of NO2 by both mechanisms. (i) Under what conditions will both of these mechanisms fit the experimental data? (i) Suggest one reason why either mechanism...
After your selection in a if more than one mechanism is still plausible propose possible experiment...
After your selection in a if more than one mechanism is still
plausible propose possible experiment that could help determine
which of the remaining mechanisms might be further validated
The macro rate law for conversion of nitrogen monoxide from auto exhausts into the brown smog pollutant nitrogen dioxide, 2 NO (g) + O2 (g) → 2 NO2 (g) is: rate-k[NOF [02] Six mechanisms proposed. When艹appears, means elementary step is an equilibrium reaction: Mech A NO (g) + NO (g) N2O2...
Gaseous ozone undergoes decomposition according to the stochiometric equation: 203(g) →302 (g) Two alternative mechanisms have...
Gaseous ozone undergoes decomposition according to the stochiometric equation: 203(g) →302 (g) Two alternative mechanisms have been proposed to account for this reaction. Mechanism 2 03 302 bimolecular, rate constant k Mechanism II 03 02 + fast equilibrium, equilibrium constant K1 0+ 03 — 202 slow, rate constant k2 A. Derive rate laws for the formation of O2 for each mechanism. B. Thermodynamic measurements give standard enthalpies of formation for each of the following species at 298 K: species AH°...
Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) Given the following reactions and enthalpies of formation: N2(g)...
Calculate the enthalpy of the reaction 2NO(g)+O2(g)→2NO2(g) Given the following reactions and enthalpies of formation: N2(g) + 2O2(g)→ 2NO2(g), ΔH∘ = 66.4kJ N2(g)+ O2(g)→ 2 NO(g), ΔH∘=180.4 kJ Please explain the steps as well!
The standard enthalpy of formation of NO(g) is +90.3 kJ·mol-1 and that of NO2(g) is +33.2...
The standard enthalpy of formation of NO(g) is +90.3 kJ·mol-1 and that of NO2(g) is +33.2 kJ·mol-1. Calculate the reaction enthalpy for 2NO(g) + O2(g) ® 2NO2(g) A. -47.8 kJ B. -57.1 kJ C. +123.5 kJ D. -23.9 kJ E. -114.2 kJ Please explain why/steps.
Consider the reaction: 2 BsHs (I)12 02 (g) (a) Use the standard enthalpies of formation found...
Consider the reaction: 2 BsHs (I)12 02 (g) (a) Use the standard enthalpies of formation found in Appendix B of the textbook to calculate the enthalpy change of the reaction. The standard enthalpy of formation of BsH, (I) is 73.2 kl/mol. 5 B2Os (s) +9 H2O (I) (b) Predict the sign of the entropy change and provide the two reasons likely to have made the biggest impact on the entropy change (and upon which you based your prediction). (c) Based...
#13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Br2  
#13 Interpreting Mechanisms 1. Consider the following mechanism: Step 1 Br2 2Br fast Step 2 Br + H2 H2Br fast Step 3 H2Br + Br 2HBr slow a. What is the overall equation? b. Identify the intermediate(s) if any. c. What is the molecularity and the rate law for each step including any reversible steps? d. What is the predicted rate law expression for this reaction. Be sure to only list reactants from the overall equation and...
The reaction of NO with O2 to give NO2 is an important process in the formation...
The reaction of NO with O2 to give NO2 is an important process in the formation of smog in any large city: 2NO+ O2 + 2NO2 Experiments show that this reaction is third order overall. The following mechanism has been proposed: NO + NON202 N202 + O2 NO2 + NO2 (a) If the second step is rate-determining, what is the rate law? e rate law? [NO] Rate = k2 [02] (6) Is this rate law consistent with the overall third-order...
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 ...
2. Consider this two step mechanism for a reaction… Step 1 NO2 + O3 --> NO3 + O2 slow; rate determining step Step 2 NO3 + NO2 --> N2O5 fast a. What is the overall reaction? b. Identify the intermediates in the mechanism. c. Write the rate law expression for each step of the mechanism including any reversible reactions. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates...
A proposed mechanism for a reaction is as follows: NO2(g) + NO2(g) + N204(8) Fast/Equilibrium Step N2048) -> NO(g) + NO3(g) Slow NO3(g) NO) + O2(g) Fast The target rate law is rate = k (NO2)2 The target reaction is 2NO2(e) 2NON + O2) A. Write the rate law expected for this mechanism: B. What is the rate-determining step? C. What is the overall balanced equation for this mechanism? D. If there is/are a reactive intermediate(s), which is/are they? E....
[17 Marks Q 2(b) The rate equation for the reaction 2NO + O2 -» 2NO2 was determined experimentally to be Rate kINO] [02]. Two mechanisms have been proposed for this reaction: Mechanism A Mechanism B 2NO N202 NO O2 NO3 NO3 + NO → 2NO2 N202 O22NO2 (i) Determine the rate equation for the formation of NO2 by both mechanisms. (i) Under what conditions will both of these mechanisms fit the experimental data? (i) Suggest one reason why either mechanism...
After your selection in a if more than one mechanism is still
plausible propose possible experiment that could help determine
which of the remaining mechanisms might be further validated
The macro rate law for conversion of nitrogen monoxide from auto exhausts into the brown smog pollutant nitrogen dioxide, 2 NO (g) + O2 (g) → 2 NO2 (g) is: rate-k[NOF [02] Six mechanisms proposed. When艹appears, means elementary step is an equilibrium reaction: Mech A NO (g) + NO (g) N2O2...
Gaseous ozone undergoes decomposition according to the stochiometric equation: 203(g) →302 (g) Two alternative mechanisms have been proposed to account for this reaction. Mechanism 2 03 302 bimolecular, rate constant k Mechanism II 03 02 + fast equilibrium, equilibrium constant K1 0+ 03 — 202 slow, rate constant k2 A. Derive rate laws for the formation of O2 for each mechanism. B. Thermodynamic measurements give standard enthalpies of formation for each of the following species at 298 K: species AH°...
Consider the reaction: 2 BsHs (I)12 02 (g) (a) Use the standard enthalpies of formation found in Appendix B of the textbook to calculate the enthalpy change of the reaction. The standard enthalpy of formation of BsH, (I) is 73.2 kl/mol. 5 B2Os (s) +9 H2O (I) (b) Predict the sign of the entropy change and provide the two reasons likely to have made the biggest impact on the entropy change (and upon which you based your prediction). (c) Based...
The reaction of NO with O2 to give NO2 is an important process in the formation of smog in any large city: 2NO+ O2 + 2NO2 Experiments show that this reaction is third order overall. The following mechanism has been proposed: NO + NON202 N202 + O2 NO2 + NO2 (a) If the second step is rate-determining, what is the rate law? e rate law? [NO] Rate = k2 [02] (6) Is this rate law consistent with the overall third-order...
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