The reaction between no2 and co to produce no and co2 is thought to occur in two steps: step 1: no2 + no2 no + no3 step 2: no3 + co no2 + co2 the experimental rate law is rate = k[no2]2. (a) write the equation for the overall reaction. do not include phase abbreviations. (b) identify the intermediate(s). no3 no2 co no co2

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27-03-2018
Chemistry

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The reaction between no2 and co to produce no and co2 is thought to occur in two steps: step 1: no2 + no2 no + no3 step 2: no3 + co no2 + co2 the experimental rate law is rate = k[no2]2. (a) write the equation for the overall reaction. do not include phase abbreviations. (b) identify the intermediate(s). no3 no2 co no co2

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mixter17 mixter17 · Answer 1 · 2018-04-05T17:02:49+02:00

Hello!

Part a) The equation for the overall reaction can be found by adding up the reactions for each individual step, substrating chemical compounds that are in opposite sites of the arrow, in the following way:

NO₂ + NO₂ → NO + NO₃

NO₃ + CO → NO₂ + CO₂
-------------------------------------
NO₂ + CO → NO + CO₂

Part b) The intermediates of a reaction are chemical compounds that are formed in the initial steps of a reaction and continues to react in the next step(s) of the reaction to produce the final products of the reaction. In this case, the reagent that is produced in the first reaction and consumed in the second is NO₃, so this is the reaction intermediate.

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tutorareej tutorareej · Answer 2 · 2021-10-19T13:48:24+02:00

The reaction between [tex]\rm NO_2\;and\;CO[/tex] to produce NO and [tex]\rm CO_2[/tex] occurs in the given two steps.

(a) The overall equation for the reaction can be given by reactants that are not the part of intermediate.

[tex]\rm NO_2\;+\;NO_2\;\rightarrow\;NO\;+NO_3[/tex]

[tex]\rm NO_3\;+\;CO\;\rightarrow\;NO_2\;+\;CO_2[/tex]

The overall reaction not include [tex]\rm NO_3[/tex] because it act as an intermediate and is utilized in the next step.

[tex]\rm NO_2\;+\;CO\;\rightarrow\;NO\;+\;CO_2[/tex]

(b) The intermediate species are consumed in the reaction after they are formed. In the reaction [tex]\rm NO_3[/tex] is formed in the first step and is consumed in the second step. So, the intermediate is [tex]\rm NO_3[/tex].

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