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A gas phase reaction between nitrogen dioxide and fluorine is proposed to occur by the following mechanism: step 1 slow: NO2 + F2 → NO2F + F step 2 fast: F + NO2 → NO2F (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]™[B]^... , where '1' is understood (so don't write it) for m, n etc.) Rate =

A gas phase reaction between nitrogen dioxide and fluorine is proposed to occur by the following mechanism: step 1 slow: NO2 + F2 → NO2F + F step 2 fast: F + NO2 → NO2F (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]™[B]^... , where '1' is understood (so don't write it) for m, n etc.) Rate =

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.30PAE: The rate of the decomposition of hydrogen peroxide, H2O2, depends on the concentration of iodide ion...
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A gas phase reaction between nitrogen dioxide and fluorine is proposed to occur by the following mechanism: step 1 slow: NO2 + F2 → NO2F + F step 2 fast: F + NO2 → NO2F (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]m[B]^... , where '1' is understood (so don't write it) for m, n etc.) Rate =
Transcribed Image Text:A gas phase reaction between nitrogen dioxide and fluorine is proposed to occur by the following mechanism: step 1 slow: NO2 + F2 → NO2F + F step 2 fast: F + NO2 → NO2F (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave it blank. + + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: (4) Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A]m[B]^... , where '1' is understood (so don't write it) for m, n etc.) Rate =
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Step 1 rate law

Rate law is defined as rate of reaction is directly proportional to reactants concentration to the power of its  stochiometric coefficient.

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