Ch.13 - Chemical KineticsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Given the following diagrams at t = 0 and t = 30, what is the half-life of the reaction if it follows first-order kinetics?

Solution: Given the following diagrams at t = 0 and t = 30, what is the half-life of the reaction if it follows first-order kinetics?

Problem

Time equals 0 minutes: 16 O, 0 N. Time equals 30 minutes: 4 O and 12 N.

Given the following diagrams at t = 0 and t = 30, what is the half-life of the reaction if it follows first-order kinetics?

Solution

We are asked to find the half-life of the reaction from the diagram if it follows first-order kinetics.


The integrated rate law for a first-order reaction is as follows:


ln [N]t = -kt + ln [N]0


where:

[N]t = concentration of reactants at time t

k = decay constant

t = time

[N]0 = initial concentration


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