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:
Consider the data presented below.
 Time  (s04080120160
Moles of A0.1000.0670.0450.0300.020
Determine whether the reaction is first order or second order.

Solution: Consider the data presented below. Time  (s) 04080120160Moles of A0.1000.0670.0450.0300.020Determine whether the reaction is first order or second order.

Problem
Consider the data presented below.


 Time  (s04080120160
Moles of A0.1000.0670.0450.0300.020


Determine whether the reaction is first order or second order.

Solution

We’re being asked to determine a reaction is first order or second order based on the data given.


Recall the first order and second order integrated rate law and their graph:

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

ln[A]t=-kt+ln[A]0

where: 

[A]t = concentration at time t
k = rate constant
t = time
[A]0 = initial concentration


The plot of ln [A] vs. t is linear which shows first-order reaction:

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