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: The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.44×10−4 s-1 at a certain temperature. If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the

Solution: The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.44×10−4 s-1 at a certain temperature. If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the

Problem

The decomposition of SO2Cl2 is first order in SO2Cl2 and has a rate constant of 1.44×10−4 s-1 at a certain temperature. If the initial concentration of SO2Cl2 is 1.00 M, how long will it take for the concentration to decrease to 0.78 M ?

Solution

The Integrated Rate Laws relates the variable of time to the Rate Law equation.

For a First Order reaction, the integrated rate law is:

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