The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. The integrated rate law for a first-order reaction is: [A] = [A]oe-kt Now say we are particularly interested in the time it would take for the concentration to become one- half of its initial value. Then we could substitute [Alo for [A] and rearrange the equation to: t1/2 = 0.693 k This equation calculates the time required for the reactant concentration to drop to half its initial value. In other words, it calculates the half-life. Half-life equation for first-order reactions: t1/2 = 0.693 k where t₁/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s-¹). Part A To calculate the half-life, plug the value for k into the half-life equation and solve. What is the half-life of a first-order reaction with a rate constant of 1.40x104 s-¹? Express your answer with the appropriate units. Value Submit A Units Review | Constants | Periodic Table Request Answer 21 ?
The integrated rate law allows chemists to predict the reactant concentration after a certain amount of time, or the time it would take for a certain concentration to be reached. The integrated rate law for a first-order reaction is: [A] = [A]oe-kt Now say we are particularly interested in the time it would take for the concentration to become one- half of its initial value. Then we could substitute [Alo for [A] and rearrange the equation to: t1/2 = 0.693 k This equation calculates the time required for the reactant concentration to drop to half its initial value. In other words, it calculates the half-life. Half-life equation for first-order reactions: t1/2 = 0.693 k where t₁/2 is the half-life in seconds (s), and k is the rate constant in inverse seconds (s-¹). Part A To calculate the half-life, plug the value for k into the half-life equation and solve. What is the half-life of a first-order reaction with a rate constant of 1.40x104 s-¹? Express your answer with the appropriate units. Value Submit A Units Review | Constants | Periodic Table Request Answer 21 ?
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter13: Chemical Kinetics
Section: Chapter Questions
Problem 13.23QE: Nitrogen monoxide reacts with chlorine to form nitrosyl chloride. NO(g)+12Cl2(g)NOCl(g) The figure...
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