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 XY is second order in XY and has a rate constant of 7.02×10−3 M-1 s-1 at a certain temperature. If the initial concentration of  XY is 0.050 M, what is the concentration of XY aft

Solution: The decomposition of XY is second order in XY and has a rate constant of 7.02×10−3 M-1 s-1 at a certain temperature. If the initial concentration of  XY is 0.050 M, what is the concentration of XY aft

Problem

The decomposition of XY is second order in XY and has a rate constant of 7.02×10−3 M-1 s-1 at a certain temperature. If the initial concentration of  XY is 0.050 M, what is the concentration of XY after 55.0 s?

Solution

We’re being asked to determine the concentration of XY after 55.0 s given an initial concentration of 0.050 M.


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


1[A]t=kt+1[A]0


where:

[A]t = concentration at time t

k = rate constant

t = time

[A]0 = initial concentration


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