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Directions: Consider the given graphs below. Mix and match the graphs with the correct descriptions. Use the following options: X-zero order; Y- first order; Z- second order. Zero order First order Second order Concentration Concentration Concentration 1. Changing the concentration of the reactant will have no effect on its rate of reaction. 2. It depends on the concentration of one reactant. 3. The rate law is rate = k [A]. 4. The rate is expressed as rate = k. 5. May be expressed in any of the following equations: rate = k [A]? , rate = k [B]?, rate = k [A][B]. ane rate rate

Directions: Consider the given graphs below. Mix and match the graphs with the correct descriptions. Use the following options: X-zero order; Y- first order; Z- second order. Zero order First order Second order Concentration Concentration Concentration 1. Changing the concentration of the reactant will have no effect on its rate of reaction. 2. It depends on the concentration of one reactant. 3. The rate law is rate = k [A]. 4. The rate is expressed as rate = k. 5. May be expressed in any of the following equations: rate = k [A]? , rate = k [B]?, rate = k [A][B]. ane rate rate

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 12PS: The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table...
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Directions: Consider the given graphs below. Mix and match the graphs with the correct descriptions. Use the following options: X- zero order; Y- first order; Z- second order. Zero order First order Second order Concentration Concentration Concentration 1. Changing the concentration of the reactant will have no effect on its rate of reaction. 2. It depends on the concentration of one reactant. 3. The rate law is rate = k [A]. 4. The rate is expressed as rate = k. 5. May be expressed in any of the following equations: rate = k [A]? , rate = k [B]², rate = k [A][B]. rate rate
Transcribed Image Text:Directions: Consider the given graphs below. Mix and match the graphs with the correct descriptions. Use the following options: X- zero order; Y- first order; Z- second order. Zero order First order Second order Concentration Concentration Concentration 1. Changing the concentration of the reactant will have no effect on its rate of reaction. 2. It depends on the concentration of one reactant. 3. The rate law is rate = k [A]. 4. The rate is expressed as rate = k. 5. May be expressed in any of the following equations: rate = k [A]? , rate = k [B]², rate = k [A][B]. rate rate
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