Elements Of Physical Chemistry
Elements Of Physical Chemistry
7th Edition
ISBN: 9780198796701
Author: ATKINS, P. W. (peter William), De Paula, Julio
Publisher: Oxford University Press
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Chapter 6, Problem 6.6P

(a)

Interpretation Introduction

Interpretation:

The following data were collected for the given reaction at 780K, using these date the order of the reaction has to be determined.

Concept Introduction:

Rate of a reaction: It represents the speed at which a chemical reaction runs.  How much concentration of substrates (reactants) consumed and how much concentration of targets (products) formed in a unit of time is said to be rate of reaction.

Rate of reaction depends on time, temperature, pressure, concentration, and pH of the reaction.

Rate of the reaction is the change in the concentration of reactant or a product with time. It can be varied in accordance with temperature, pressure, concentration, presence of catalyst, surface area.

General rate reaction is,

  aA+bBcC+dD

  Rate=-1aΔ[A]Δt=-1bΔ[B]Δt=1cΔ[C]Δt=1dΔ[D]Δt

The negative sign indicates the reduction of concentration of reactant.

Integrated rate law for first order reaction:

Consider A as substance, that gives the product based on the equation,

    aAproducts

Where a= stoichiometric co-efficient of reactant A.

Consider the reaction has first-order rate law,

    Rate=-Δ[A]Δt=k[A]

The integrated rate law equation can be given as,

    ln[A]t[A]o=-kt

The above expression is called integrated rate law for first order reaction.

(a)

Expert Solution
Check Mark

Explanation of Solution

Given reaction is,

  2HI(g)H2(g)+I2(g)

Record the given data’s

  t/s01234[HI]/(moldm3)10.430.270.20.16

Let us consider the first order reaction

Rate constant is,

  ln[A]t=kt+ln[A]0ln[A]t[A]o=-ktk=1t[A]t[A]o

Given values are plugging above equation,

  k1=11[10.43]=0.43×103M1s1k2=12[10.27]=0.135×103M1s1k3=13[10.2]=0.06M1s1k4=14[10.16]=0.04M1s1

Hence, the all rate constant are nearly same, so this reaction confirmed to be first order reaction.

(b)

Interpretation Introduction

Interpretation:

Plot the given data in an appropriate fashion, the rate constant has to be determined.

Concept Introduction:

Rate of a reaction: It represents the speed at which a chemical reaction runs.  How much concentration of substrates (reactants) consumed and how much concentration of targets (products) formed in a unit of time is said to be rate of reaction.

Rate of reaction depends on time, temperature, pressure, concentration, and pH of the reaction.

Rate of the reaction is the change in the concentration of reactant or a product with time. It can be varied in accordance with temperature, pressure, concentration, presence of catalyst, surface area.

General rate reaction is,

  aA+bBcC+dD

  Rate=-1aΔ[A]Δt=-1bΔ[B]Δt=1cΔ[C]Δt=1dΔ[D]Δt

The negative sign indicates the reduction of concentration of reactant.

(b)

Expert Solution
Check Mark

Explanation of Solution

Given reaction is,

  2HI(g)H2(g)+I2(g)

Record the given data’s

  t/s01234[HI]/(moldm3)10.430.270.20.16

In order to determine the rate law, we need to determine the order of the reaction with respect to (HI).  This can be done graphically.

For a zeroth order reaction [HI] vs time should result in a straight line, for a first order reaction ln[HI] vs time will give a straight line while for a second order reaction 1/[HI] vs time will result in a straight line plot.

In the present case a plot 1/[HI] vs time gives a straight line as shown below (Figure -1), thus the given reaction is first order.

The rate law is thus r=k[HI]2

Elements Of Physical Chemistry, Chapter 6, Problem 6.6P

Figure 1

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Chapter 6 Solutions

Elements Of Physical Chemistry

Ch. 6 - Prob. 6C.4STCh. 6 - Prob. 6D.1STCh. 6 - Prob. 6D.2STCh. 6 - Prob. 6D.3STCh. 6 - Prob. 6E.1STCh. 6 - Prob. 6E.2STCh. 6 - Prob. 6F.1STCh. 6 - Prob. 6F.2STCh. 6 - Prob. 6G.1STCh. 6 - Prob. 6G.2STCh. 6 - Prob. 6G.3STCh. 6 - Prob. 6H.1STCh. 6 - Prob. 6I.1STCh. 6 - Prob. 6I.2STCh. 6 - Prob. 6A.1ECh. 6 - Prob. 6A.2ECh. 6 - Prob. 6A.3ECh. 6 - Prob. 6B.1ECh. 6 - Prob. 6B.2ECh. 6 - Prob. 6B.3ECh. 6 - Prob. 6B.4ECh. 6 - Prob. 6B.5ECh. 6 - Prob. 6C.1ECh. 6 - Prob. 6C.2ECh. 6 - Prob. 6C.3ECh. 6 - Prob. 6C.4ECh. 6 - Prob. 6C.5ECh. 6 - Prob. 6C.6ECh. 6 - Prob. 6C.7ECh. 6 - Prob. 6C.8ECh. 6 - Prob. 6C.9ECh. 6 - Prob. 6C.10ECh. 6 - Prob. 6C.11ECh. 6 - Prob. 6C.12ECh. 6 - Prob. 6D.1ECh. 6 - Prob. 6D.2ECh. 6 - Prob. 6D.3ECh. 6 - Prob. 6D.4ECh. 6 - Prob. 6D.5ECh. 6 - Prob. 6D.6ECh. 6 - Prob. 6D.7ECh. 6 - Prob. 6D.8ECh. 6 - Prob. 6D.9ECh. 6 - Prob. 6D.10ECh. 6 - Prob. 6D.11ECh. 6 - Prob. 6E.1ECh. 6 - Prob. 6E.2ECh. 6 - Prob. 6E.3ECh. 6 - Prob. 6F.1ECh. 6 - Prob. 6F.2ECh. 6 - Prob. 6F.3ECh. 6 - Prob. 6G.1ECh. 6 - Prob. 6G.2ECh. 6 - Prob. 6G.3ECh. 6 - Prob. 6G.5ECh. 6 - Prob. 6H.1ECh. 6 - Prob. 6H.2ECh. 6 - Prob. 6H.3ECh. 6 - Prob. 6H.4ECh. 6 - Prob. 6I.1ECh. 6 - Prob. 6I.2ECh. 6 - Prob. 6I.3ECh. 6 - Prob. 6.1DQCh. 6 - Prob. 6.2DQCh. 6 - Prob. 6.3DQCh. 6 - Prob. 6.4DQCh. 6 - Prob. 6.5DQCh. 6 - Prob. 6.6DQCh. 6 - Prob. 6.7DQCh. 6 - Prob. 6.8DQCh. 6 - Prob. 6.9DQCh. 6 - Prob. 6.10DQCh. 6 - Prob. 6.11DQCh. 6 - Prob. 6.12DQCh. 6 - Prob. 6.13DQCh. 6 - Prob. 6.14DQCh. 6 - Prob. 6.1PCh. 6 - Prob. 6.2PCh. 6 - Prob. 6.3PCh. 6 - Prob. 6.4PCh. 6 - Prob. 6.5PCh. 6 - Prob. 6.6PCh. 6 - Prob. 6.9PCh. 6 - Prob. 6.10PCh. 6 - Prob. 6.11PCh. 6 - Prob. 6.12PCh. 6 - Prob. 6.13PCh. 6 - Prob. 6.15PCh. 6 - Prob. 6.16PCh. 6 - Prob. 6.17PCh. 6 - Prob. 6.19PCh. 6 - Prob. 6.20PCh. 6 - Prob. 6.21PCh. 6 - Prob. 6.22PCh. 6 - Prob. 6.24PCh. 6 - Prob. 6.25PCh. 6 - Prob. 6.26PCh. 6 - Prob. 6.27PCh. 6 - Prob. 6.28PCh. 6 - Prob. 6.29PCh. 6 - Prob. 6.30P
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