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Consider the hypothetical reaction 2D+3E A+B+2C where the rate law is Rate -- k[A][B]¹ An experiment is carried out where (Al-1.0 x 103 M [B] -7.0 M, and [C] -2.0 M. The reaction is started, and after 6.0 seconds, the concentration of A is 3.8 x 103 M a. Calculate the value of k for this reaction. A[A] At k- L² mol-1 b. Calculate the half life for this experiment Half-life- c. Calculate the concentration of A after 15.0 seconds. Concentration d. Calculate the concentration of C after 15 seconds. Concentration-

Consider the hypothetical reaction 2D+3E A+B+2C where the rate law is Rate -- k[A][B]¹ An experiment is carried out where (Al-1.0 x 103 M [B] -7.0 M, and [C] -2.0 M. The reaction is started, and after 6.0 seconds, the concentration of A is 3.8 x 103 M a. Calculate the value of k for this reaction. A[A] At k- L² mol-1 b. Calculate the half life for this experiment Half-life- c. Calculate the concentration of A after 15.0 seconds. Concentration d. Calculate the concentration of C after 15 seconds. Concentration-

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.96PAE: The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g)...
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Consider the hypothetical reaction A+B+2C 2D+3E where the rate law is Rate- =k[A][B]¹ An experiment is carried out where [A], -1.0 x 102 M. [B] -7.0 M, and [C] -2.0 M. The reaction is started, and after 6.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. A[A] At k- L² mol-1 b. Calculate the half-life for this experiment. Half-life- c. Calculate the concentration of A after 15.0 seconds. Concentration M d. Calculate the concentration of C after 15 seconds. Concentration - M
Transcribed Image Text:Consider the hypothetical reaction A+B+2C 2D+3E where the rate law is Rate- =k[A][B]¹ An experiment is carried out where [A], -1.0 x 102 M. [B] -7.0 M, and [C] -2.0 M. The reaction is started, and after 6.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. A[A] At k- L² mol-1 b. Calculate the half-life for this experiment. Half-life- c. Calculate the concentration of A after 15.0 seconds. Concentration M d. Calculate the concentration of C after 15 seconds. Concentration - M
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