Consider the hypothetical reaction A + B + 2C → 2D + 3E where the rate law is Rate = -(Δ[A])/(Δt) = k [A] [B]2 An experiment is carried out where [A]0 = 1.0 x 10-2 M, [B]0 = 3.0 M, and [C]0 = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. b. Calculate the half-life for this experiment. c. Calculate the concentration of A after 13.0 seconds. d. Calculate the concentration of C after 13.0 seconds.
Consider the hypothetical reaction A + B + 2C → 2D + 3E where the rate law is Rate = -(Δ[A])/(Δt) = k [A] [B]2 An experiment is carried out where [A]0 = 1.0 x 10-2 M, [B]0 = 3.0 M, and [C]0 = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10-3 M. a. Calculate the value of k for this reaction. b. Calculate the half-life for this experiment. c. Calculate the concentration of A after 13.0 seconds. d. Calculate the concentration of C after 13.0 seconds.
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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Consider the hypothetical reaction
A + B + 2C → 2D + 3E
where the rate law is
Rate = -(Δ[A])/(Δt) = k [A] [B]2
An experiment is carried out where [A]0 = 1.0 x 10-2 M, [B]0 = 3.0 M, and [C]0 = 2.0 M. The reaction is started, and after 8.0 seconds, the concentration of A is 3.8 x 10-3 M.
a. Calculate the value of k for this reaction.
b. Calculate the half-life for this experiment.
c. Calculate the concentration of A after 13.0 seconds.
d. Calculate the concentration of C after 13.0 seconds.
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