Chemistry: The Molecular Nature of Matter and Change - Standalone book
Chemistry: The Molecular Nature of Matter and Change - Standalone book
7th Edition
ISBN: 9780073511177
Author: Martin Silberberg Dr., Patricia Amateis Professor
Publisher: McGraw-Hill Education
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Chapter 16, Problem 16.114P

(a)

Interpretation Introduction

Interpretation:

Average rate for each trial has to be determined.

Concept introduction:

Relative rates and stoichiometry: During a chemical reaction, amounts of reactant decrease with time and amounts of products increases.

Reaction Rate = - 1coefficientΔ[reactants]Δt = +1coefficient Δ[products]Δt

(a)

Expert Solution
Check Mark

Explanation of Solution

The reaction given is:

Givenreaction: I2(aq)+2S2O32-(aq)2I-(aq)+S4O62-(aq)

The average rate of the chemical reaction:

Reaction Rate = - 1coefficientΔ[reactants]Δt = +1coefficient Δ[products]ΔtReaction Rate = - Δ[I2]Δt = -12 Δ[S2O32-]Δt

Molarity of [S2O32-]is,

=[(10.0mL)(0.0050M)]50.0mL=(0.0010M)S2O32-.

Reaction Rate = - Δ[I2]Δt = -12 Δ[S2O32-]Δt=[12(0.0010M)]time=[0.00050M]time=rate

Hence, the average rates:

For experiment (1): Rate1 = (0.00050M)29.0sec=1.7×10-5M.s-1.

For experiment (2): Rate2 = (0.00050M)14.5sec=3.45×10-5M.s-1.

For experiment (3): Rate3 = (0.00050M)14.5sec=3.45×10-5M.s-1.

Therefore, the average rate for each trial was calculated as shown above.

(b)

Interpretation Introduction

Interpretation:

Reaction order with respect to each reactant has to be found.

Concept introduction:

Rate law or rate equation: The relationship between the reactant concentrations and reaction rate is expressed by an equation.

aA + bBxXRate of reaction = k [A]m[B]nTotalorderof reaction = (m + n).

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

Rate constant, k: It is a proportionality constant that relates rate and concentration at a given temperature.

(b)

Expert Solution
Check Mark

Explanation of Solution

Molarity of [I-]=[(10.0mL)(0.20M)]50.0mL=(0.040M)I-(Experiment1)

Molarity of [I-]=[(20.0mL)(0.20M)]50.0mL=(0.080M)I-(Experiment2and3)

Molarity of [S2O82-]=[(20.0mL)(0.10M)]50.0mL=(0.040M)I-(Experiment1and2)

Molarity of [S2O82-]=[(10.0mL)(0.10M)]50.0mL=(0.020M)I-(Experiment3)

Rate law equation: Rate = k [I-]m[S2O82-]n

Let’s find the order of reactant [I-] by comparing first and second experiments as follows,

Findorderofthereaction:_ Comparingfirsttwoexperiments1and2,rate1=[I-]1m[S2O82-]1n, rate1 = 1.7 ×10-5mol/L.srate2 = k[I-]2m[S2O82-]2n, rate2 = 3.4×105 mol/L.srate2rate1=k[I-]2m[S2O82-]2n[I-]1m[S2O82-]1n3.4×105 mol/L.s1.7 ×10-5mol/L.s=(0.0800)m(0.040)n(0.0400)m(0.040)n 2 = (2)mm = 1 

The order with respect to [I-] is FIRST order.

Let’s find the order of reactant [S2O82-] by comparing second and third experiments as follows,

Findorderofthereaction:_ Comparingfirsttwoexperiments2 and3,rate3=[I-]3m[S2O82-]3n, rate3 = 3.4 ×10-5mol/L.srate2 = k[I-]2m[S2O82-]2n, rate2 = 3.4×105 mol/L.srate3rate 2=k[I-]3m[S2O82-]3nk[I-]2m[S2O82-]2n3.4×105 mol/L.s3.4 ×10-5mol/L.s=(0.040)m(0.0200)n(0.040)m(0.0400)n 1 = (0.5)mln(1)=nln(0.5)n = 0 

The order with respect to [S2O82-] is ZERO order.

In order to figure out the reaction equation the order of the reactants needed, which is calculated by comparing any two experiments where the concentration of two reactants are constant and another varies, and in vice-versa. Hence, Rate equation is

Reaction rate = k [I]1[S2O82-]0.

The respective order of reactant [I] is FIRST ORDER.

The respective order of reactant [S2O82-] is ZERO ORDER.

Hence, the reaction rate becomes,

Reaction rate = k [I-]1[S2O82-]0.

(c)

Interpretation Introduction

Interpretation:

Rate constant of the reaction has to be calculated.

Concept introduction:

Rate law or rate equation: The relationship between the reactant concentrations and reaction rate is expressed by an equation.

aA + bBxXRate of reaction = k [A]m[B]nTotalorderof reaction = (m + n).

Reaction Rate = k [A]m[B]n[C]p,where 'm, n and p' are orders of the reactants.

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

Rate constant, k: It is a proportionality constant that relates rate and concentration at a given temperature.

(c)

Expert Solution
Check Mark

Explanation of Solution

Considering the experiment (1),

rate1 = 1.7 ×10-5mol/L.s ; [I-]=0.0400mol/L;[S2O82-]=0.040mol/L.

Given rate law: Reaction rate = k [I]1[S2O82-]0

Calculating the rate constant of reaction as follows,

Reaction rate = k [I]1[S2O82-]0(1.7 ×10-5mol/L.s)=k( 0.0400mol/L)1k=1.7 ×10-5mol/L.s( 0.0400mol/L)1=42.5 ×10-5L/mol.s.

Therefore, the rate constant of reaction at given concentration is 42.5 ×10-5L/mol.s.

(d)

Interpretation Introduction

Interpretation:

Rate law of the overall reaction has to be calculated.

Concept introduction:

Rate law or rate equation: The relationship between the reactant concentrations and reaction rate is expressed by an equation.

aA + bBxXRate of reaction = k [A]m[B]nTotalorderof reaction = (m + n).

Reaction Rate = k [A]m[B]n[C]p,where 'm, n and p' are orders of the reactants.

Order of a reaction: The order of a reaction with respect to a particular reactant is the exponent of its concentration term in the rate law expression, and the overall reaction order is the sum of the exponents on all concentration terms.

Rate constant, k: It is a proportionality constant that relates rate and concentration at a given temperature.

(d)

Expert Solution
Check Mark

Explanation of Solution

The overall reaction law is obtained by substituting the rate constant value as follows,

Reaction rate = k [I-]1[S2O82-]0.

The rate constant of reaction at given concentration is 42.5 ×10-5L/mol.s.

Reaction rate = (42.5 ×10-5L/mol.s.) [I-]1.

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Chapter 16 Solutions

Chemistry: The Molecular Nature of Matter and Change - Standalone book

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