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: Dinitrogen pentoxide (N2 O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45 oC of 1.0x10 - 5 hr- 1.Calculate the partial pressur

Solution: Dinitrogen pentoxide (N2 O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45 oC of 1.0x10 - 5 hr- 1.Calculate the partial pressur

Problem

Dinitrogen pentoxide (N2 O5) decomposes in chloroform as a solvent to yield NO2 and O2. The decomposition is first order with a rate constant at 45 oC of 1.0x10 - 5 hr- 1.

Calculate the partial pressure of O2 produced from 1.51 L of 0.601 M N2 O5 solution at 45 oC over a period of 20.1 h if the gas is collected in a 11.6-L container. (Assume that the products do not dissolve in chloroform.)

Solution

We are being asked to determine the partial pressure of O2 given the following first-order reaction:

N2 O5(g) NO2(g) + O2(g) ; k = 1.0x10 - 5 hr- 1


For this problem, we will do the following steps:


Step 1: Calculate [A] at time t using the first-order integrated rate law

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


lnAt = -kt + lnA0


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


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