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The reaction between chlorine monoxide and nitrogen dioxide CIO(g) + NO₂(g) + M(g) → CIONO2(g) + M(g) produces chlorine nitrate (CIONO₂). A third molecule (M) takes part in the reaction but is unchanged by it (it remains "M" as a reactant and as a product). The reaction is first order in [CIO] and [NO₂]. What is the rate law of the reaction? Rate = k[CIO][NO₂][M] O Rate = k[CIONO₂] O Rate = = K[CIONO₂][M] O Rate = k[CIO][NO₂][M]* - O Rate = k[CIONO₂][M]* O Rate = k[CIO][NO₂] Indicate the reaction order with respect to M. O Zero order with respect to M O Impossible to determine the order with respect to M O First order with respect to M Hint: Knowing that the reaction is first order in both NO2 and CIO means that the exponent for the concentrations in the rate law for both of these reactants is 1. Because no dependence on the rate was given in the problem for M, we can assume that changing [M] does not affect the rate of the reaction.

The reaction between chlorine monoxide and nitrogen dioxide CIO(g) + NO₂(g) + M(g) → CIONO2(g) + M(g) produces chlorine nitrate (CIONO₂). A third molecule (M) takes part in the reaction but is unchanged by it (it remains "M" as a reactant and as a product). The reaction is first order in [CIO] and [NO₂]. What is the rate law of the reaction? Rate = k[CIO][NO₂][M] O Rate = k[CIONO₂] O Rate = = K[CIONO₂][M] O Rate = k[CIO][NO₂][M]* - O Rate = k[CIONO₂][M]* O Rate = k[CIO][NO₂] Indicate the reaction order with respect to M. O Zero order with respect to M O Impossible to determine the order with respect to M O First order with respect to M Hint: Knowing that the reaction is first order in both NO2 and CIO means that the exponent for the concentrations in the rate law for both of these reactants is 1. Because no dependence on the rate was given in the problem for M, we can assume that changing [M] does not affect the rate of the reaction.

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 30E: The annual production of HNO3 in 2013 was 60 million metric tons Most of that was prepared by the...
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The reaction between chlorine monoxide and nitrogen dioxide CIO(g) + NO₂(g) + M(g) → CIONO2(g) + M(g) produces chlorine nitrate (CIONO2). A third molecule (M) takes part in the reaction but is unchanged by it (it remains "M" as a reactant and as a product). The reaction is first order in [CIO] and [NO₂]. What is the rate law of the reaction? O Rate = = k[CIO][NO₂] [M] =k[CIONO₂] O Rate = O Rate = k[CIONO₂] [M] O Rate = k[CIO][NO₂] [M] O Rate = k[CIONO₂][M] O Rate = k[CIO][NO₂] Indicate the reaction order with respect to M. O Zero order with respect to M O Impossible to determine the order with respect to M O First order with respect to M Hint: Knowing that the reaction is first order in both NO₂ and CIO means that the exponent for the concentrations in the rate law for both of these reactants is 1. Because no dependence on the rate was given in the problem for M, we can assume that changing [M] does not affect the rate of the reaction. Question Help: Read Submit Question
Transcribed Image Text:The reaction between chlorine monoxide and nitrogen dioxide CIO(g) + NO₂(g) + M(g) → CIONO2(g) + M(g) produces chlorine nitrate (CIONO2). A third molecule (M) takes part in the reaction but is unchanged by it (it remains "M" as a reactant and as a product). The reaction is first order in [CIO] and [NO₂]. What is the rate law of the reaction? O Rate = = k[CIO][NO₂] [M] =k[CIONO₂] O Rate = O Rate = k[CIONO₂] [M] O Rate = k[CIO][NO₂] [M] O Rate = k[CIONO₂][M] O Rate = k[CIO][NO₂] Indicate the reaction order with respect to M. O Zero order with respect to M O Impossible to determine the order with respect to M O First order with respect to M Hint: Knowing that the reaction is first order in both NO₂ and CIO means that the exponent for the concentrations in the rate law for both of these reactants is 1. Because no dependence on the rate was given in the problem for M, we can assume that changing [M] does not affect the rate of the reaction. Question Help: Read Submit Question
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