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: Reaction A and reaction B have identical frequency factors. However, reaction B has a higher activation energy than reaction A.Which reaction has a greater rate constant at room temperature?

Solution: Reaction A and reaction B have identical frequency factors. However, reaction B has a higher activation energy than reaction A.Which reaction has a greater rate constant at room temperature?

Problem

Reaction A and reaction B have identical frequency factors. However, reaction B has a higher activation energy than reaction A.

Which reaction has a greater rate constant at room temperature?

Solution

The temperature dependence of a chemical reaction is represented by the Arrhenius equation:


<math xmlns="http://www.w3.org/1998/Math/MathML"><menclose mathcolor="#0000FF" notation="box"><mi>k</mi><mo>&#xA0;</mo><mo>=</mo><mo>&#xA0;</mo><mi>A</mi><mo>&#xB7;</mo><msup><mi>e</mi><mrow><mo>-</mo><mfrac><msub><mi>E</mi><mi>a</mi></msub><mrow><mi>R</mi><mi>T</mi></mrow></mfrac></mrow></msup></menclose><mspace linebreak="newline"></mspace><mi>w</mi><mi>h</mi><mi>e</mi><mi>r</mi><mi>e</mi><mo>,</mo><mspace linebreak="newline"></mspace><mi mathvariant="normal">k</mi><mo>&#xA0;</mo><mo>=</mo><mo>&#xA0;</mo><mi>rate</mi><mo>&#xA0;</mo><mi>constant</mi><mspace linebreak="newline"></mspace><mi mathvariant="normal">A</mi><mo>&#xA0;</mo><mo>=</mo><mo>&#xA0;</mo><mi>frequency</mi><mo>&#xA0;</mo><mi>factor</mi><mspace linebreak="newline"></mspace><msub><mi mathvariant="normal">E</mi><mi mathvariant="normal">a</mi></msub><mo>&#xA0;</mo><mo>=</mo><mo>&#xA0;</mo><mi>activation</mi><mo>&#xA0;</mo><mi>energy</mi><mspace linebreak="newline"></mspace><mi mathvariant="normal">R</mi><mo>&#xA0;</mo><mo>=</mo><mo>&#xA0;</mo><mi>gas</mi><mo>&#xA0;</mo><mi>constant</mi><mspace linebreak="newline"></mspace><mi mathvariant="normal">T</mi><mo>&#xA0;</mo><mo>=</mo><mo>&#xA0;</mo><mi>temperature</mi></math>


We have to determine whether reaction A or reaction B has a greater rate constant at room temperature while we are given that the activation energy for reaction B is higher.


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