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Consider a chemical reaction: 2 A(aq) + B(aq) → 2 C(aq) + 2 D(s) the initial rate was measured at three different reactant concentrations. What is the rate law for the reaction? Trial Initial [A] 1 2 3 (mol/L) 0.100 0.100 0.200 rate = K[A]²[B]2 O rate = K[A][B]² O rate = k[A][B]3 rate = k[A]2[B] Initial [B] (mol/L) 0.100 0.300 0.100 Initial Rate (mol/(L-min)) 1.30 x 10-7 1.17 x 10-6 2.60 x 10-7

Consider a chemical reaction: 2 A(aq) + B(aq) → 2 C(aq) + 2 D(s) the initial rate was measured at three different reactant concentrations. What is the rate law for the reaction? Trial Initial [A] 1 2 3 (mol/L) 0.100 0.100 0.200 rate = K[A]²[B]2 O rate = K[A][B]² O rate = k[A][B]3 rate = k[A]2[B] Initial [B] (mol/L) 0.100 0.300 0.100 Initial Rate (mol/(L-min)) 1.30 x 10-7 1.17 x 10-6 2.60 x 10-7

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Consider a chemical reaction: 2 A(aq) + B(aq) → 2 C(aq) + 2 D(s) the initial rate was measured at three different reactant concentrations. What is the rate law for the reaction? Trial Initial [A] 1 2 3 (mol/L) 0.100 0.100 0.200 rate = K[A]²[B]² O rate = k[A][B]² O rate= K[A][B]³ rate = K[A]²[B] Initial [B] (mol/L) 0.100 0.300 0.100 Initial Rate (mol/(L-min)) 1.30 x 10-7 1.17 x 10-6 2.60 x 10-7
Transcribed Image Text:Consider a chemical reaction: 2 A(aq) + B(aq) → 2 C(aq) + 2 D(s) the initial rate was measured at three different reactant concentrations. What is the rate law for the reaction? Trial Initial [A] 1 2 3 (mol/L) 0.100 0.100 0.200 rate = K[A]²[B]² O rate = k[A][B]² O rate= K[A][B]³ rate = K[A]²[B] Initial [B] (mol/L) 0.100 0.300 0.100 Initial Rate (mol/(L-min)) 1.30 x 10-7 1.17 x 10-6 2.60 x 10-7
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