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 gas phase decomposition of sulfuryl chloride at 600 ºK SO2Cl2(g) → SO2 (g) + Cl2(g) is first order in SO2Cl2. During one experiment it was found that when the initial concentration of SO 2Cl2 was

Solution: The gas phase decomposition of sulfuryl chloride at 600 ºK SO2Cl2(g) → SO2 (g) + Cl2(g) is first order in SO2Cl2. During one experiment it was found that when the initial concentration of SO 2Cl2 was

Problem

The gas phase decomposition of sulfuryl chloride at 600 ºK 

SO2Cl2(g) → SO2 (g) + Cl2(g) 

is first order in SO2Cl2

During one experiment it was found that when the initial concentration of SO 2Cl2 was 4.42x10-3 M, the concentration of SO2Cl2 dropped to 1.02x10-3 M after 391 min had passed. 

Based on this experiment, the rate constant for the reaction is _____ min-1.



Solution

We’re given the following first order reaction:

SO2Cl2  SO2 + Cl2


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



where [A]t = concentration at time t, k = rate constant, t = time, [A]0 = initial concentration. We’re being asked to determine the rate constant for the reaction.


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