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: At 28 oC, raw milk sours in 4 h but takes 50 h to sour in a refrigerator at 5 oC.Estimate the activation energy in kJ/mol for the reaction that leads to the souring of milk.

Solution: At 28 oC, raw milk sours in 4 h but takes 50 h to sour in a refrigerator at 5 oC.Estimate the activation energy in kJ/mol for the reaction that leads to the souring of milk.

Problem

At 28 oC, raw milk sours in 4 h but takes 50 h to sour in a refrigerator at 5 oC.

Estimate the activation energy in kJ/mol for the reaction that leads to the souring of milk.

Solution

We are asked to calculate for the activation energy of a chemical reaction given with two temperatures and two reaction times. 

The equation that connects two given temperatures and two reaction times with the activation energy is the two-point form of the Arrhenius equation:

 ln k2k1= -EaR1T2-1T1

where: k1 is the rate of first reaction

            k2 is the rate of second reaction

            Ea is the activation energy

           R is the gas constant

          T1 is the temperature for the first reaction

          T2 is the temperature of the second reaction


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