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: Comparison of first-order and zero-order reactions for the disappearance of reactant A with time. At which times during the reaction would you have trouble distinguishing a zero-order reaction from a first-order reaction?

Solution: Comparison of first-order and zero-order reactions for the disappearance of reactant A with time.At which times during the reaction would you have trouble distinguishing a zero-order reaction from a f

Problem


A graph has time on the x-axis and concentration of A on the y-axis. Both axes are unscaled. Two curves are plotted, one for a zero-order reaction and one for a first order reaction. Both begin high on the y-axis at the initial time at a concentration of A0. From there, the zero order reaction declines steeply and linearly with slope equal to negative k times t until it contacts the x-axis. The first order reaction declines with a concave shape and does not contact the x-axis.


Comparison of first-order and zero-order reactions for the disappearance of reactant A with time.


At which times during the reaction would you have trouble distinguishing a zero-order reaction from a first-order reaction?

Solution

We have to describe at what times we can have trouble distinguishing a zero-order reaction from a first-order reaction.


The order of a chemical reaction is defined as the sum of power of concentrations of the reactants in the rate equation.


Order of a chemical reaction is determined experimentally; it cannot be determined using stoichiometry from balanced chemical equation.


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