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: A series of experiments were performed to determine the rate constant for the reaction 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g)at different temperatures. A plot of ln k against 1/T was a straight line with a slope of −1.5275x104 and intercept of 23.6. What is the frequency factor?a) 196.2b) 23.6c) 1.5275x104d) 5.63x10−11e) 1.78x1010

Solution: A series of experiments were performed to determine the rate constant for the reaction 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g)at different temperatures. A plot of ln k against 1/T was a straight line wit

Problem

A series of experiments were performed to determine the rate constant for the reaction 

2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g)

at different temperatures. A plot of ln k against 1/T was a straight line with a slope of −1.5275x104 and intercept of 23.6. What is the frequency factor?

a) 196.2

b) 23.6

c) 1.5275x104

d) 5.63x10−11

e) 1.78x1010

Solution

We’re being asked to determine the frequency factor (A) of a reaction given that the plot of ln k vs. 1/T has a slope of −1.5275 × 104 and an intercept of 23.6.


We’re given the plot of ln k (y) vs. 1/T (x)


This means we need to use the two-point form of the Arrhenius Equation:


ln k=-EaR 1T + ln A


where: 

k = rate constant

Ea = activation energy (in J/mol)

R = gas constant (8.314 J/mol • K)

T = temperature (in K)

A = Arrhenius constant or frequency factor


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