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FOR PRACTICE 15.2 Consider the equation: CHCI3(8) + Cl2(8) CCI4(8) + HCI(g) The initial rate of reaction is measured at several different concentrations of the reactants with the tabulated results shown here. [CHCI3] (M) [Cl2] (M) Initial Rate (M/s) 0.010 0.010 0.0035 0.020 0.010 0.0069 0.020 0.020 0.0098 0.040 0.040 0.027 From the data, determine: (a) the rate law for the reaction (b) the rate constant (k) for the reaction

FOR PRACTICE 15.2 Consider the equation: CHCI3(8) + Cl2(8) CCI4(8) + HCI(g) The initial rate of reaction is measured at several different concentrations of the reactants with the tabulated results shown here. [CHCI3] (M) [Cl2] (M) Initial Rate (M/s) 0.010 0.010 0.0035 0.020 0.010 0.0069 0.020 0.020 0.0098 0.040 0.040 0.027 From the data, determine: (a) the rate law for the reaction (b) the rate constant (k) for 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 25E: Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following...
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FOR PRACTICE 15.2 Consider the equation: CHCI3(g) + Cl2(8) CCI4(8) + HCI(8) The initial rate of reaction is measured at several different concentrations of the reactants with the tabulated results shown here. [CHCI3] (M) [Cl2] (M) Initial Rate (M/s) 0.010 0.010 0.0035 0.020 0.010 0.0069 0.020 0.020 0.0098 0.040 0.040 0.027 From the data, determine: (a) the rate law for the reaction (b) the rate constant (k) for the reaction
Transcribed Image Text:FOR PRACTICE 15.2 Consider the equation: CHCI3(g) + Cl2(8) CCI4(8) + HCI(8) The initial rate of reaction is measured at several different concentrations of the reactants with the tabulated results shown here. [CHCI3] (M) [Cl2] (M) Initial Rate (M/s) 0.010 0.010 0.0035 0.020 0.010 0.0069 0.020 0.020 0.0098 0.040 0.040 0.027 From the data, determine: (a) the rate law for the reaction (b) the rate constant (k) for the reaction
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