Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Chapter 11, Problem 25QAP

When boron trifluoride reacts with ammonia, the following reaction occurs:

BF 3 ( g ) + NH 3 ( g ) BF 3 NH 3 ( g ) The following data are obtained at a particular temperature:

Chapter 11, Problem 25QAP, When boron trifluoride reacts with ammonia, the following reaction occurs: BF3(g)+NH3(g)BF3NH3(g)The

(a) What is the order of the reaction with respect to BF3, NH3, and overall?

(b) Write the rate expression for the reaction.

(c) Calculate k for the reaction.

(d) When [ BF 3 ] = 0.533 M and NH 3 = 0.300 M , what is the rate of the reaction at the temperature of the experiment?

Expert Solution
Check Mark
Interpretation Introduction

(a)

Interpretation:

To determine the order of reaction with respect to BF3, NH3 and overall for the following reaction:

BF3(g)+NH3(g)BF3NH3(g)

Concept introduction:

Rate of a chemical reaction: It tells us about the speed at which the reactants are converted into products.

Mathematically, rate of reaction is directly proportional to the product of concentration of each reactant raised to the power equal to their respective stoichiometric coefficients.

Let’s say we have a reaction:

aA+bBcC+dDthen,rateα[A]a[B]brate=Kf[A]a[B]bwhereKf= rateconstanta and b are order of reaction with respect to A and B 

Answer to Problem 25QAP

Order of given reaction

With respect to BF3 =1

With respect to NF3 =1

Overall = 2.

Explanation of Solution

Given information:

Here the chemical reaction is:

BF3(g)+NH3(g)BF3NH3(g)

Chemistry: Principles and Reactions, Chapter 11, Problem 25QAP

Let’s assume the reaction to be ‘t’ order with respect to BF3 and ‘y’ order with respect to NH3.

Then, rate law for experiment 1 in above reaction will be:

rate=k[BF3]t[NH3]y0.0341=k[0.100]t[0.100]y......(1)

And, rate law for experiment 4 in above reaction will be;

rate=k[BF3]t[NH3]y0.102=k[0.300]t[0.100]y......(2)

Divide (1) by (2) to get value of ‘t’.

0.03410.102=(0.1000.300)t0.334=(13)ttakniglogbothside,weget:log(0.334)=log(13)tAsweknow:log(a)t=t×log(a)-0.476=t×log(13)-0.476=t×[log(1)-log(3)]-0.476=t×[0-0.476]0.476=t×0.476t=1

Now writing rate law for experiment 2 in above reaction will be;

rate=k[BF3]t[NH3]y0.159=k[0.200]t[0.233]y......(3)

And, rate law for experiment 4 in above reaction will be;

rate=k[BF3]t[NH3]y0.0512=k[0.200]t[0.0750]y......(4)

Divide (3) by (4) to get value of ‘y’.

3.10=(0.2330.0750)y3.10=(3.10)yy=1

Thus, order with respect to NH3 is 1.

And the order of reaction will be:

                              t + y = 1+1 =2

Thus, overall order of reaction is 2.

Expert Solution
Check Mark
Interpretation Introduction

(b)

Interpretation:

To write the rate expression for the given reaction.

Concept introduction:

Rate of a chemical reaction: It tells us about the speed at which the reactants are converted into products.

Mathematically, rate of reaction is directly proportional to the product of concentration of each reactant raised to the power equal to their respective stoichiometric coefficients.

Let’s say we have a reaction:

aA+bBcC+dDthen,rateα[A]a[B]brate=Kf[A]a[B]bwhereKf= rateconstanta and b are order of reaction with respect to A and B 

Answer to Problem 25QAP

Rate law expression for the given reaction will be;

rate=k[BF3][NH3]

Explanation of Solution

Here the chemical reaction is:

BF3(g)+NH3(g)BF3NH3(g)

Order of reaction with respect to BF3 = 1

Order of reaction with respect to NH3 = 1

Let the rate constant be ‘k’.

Then, rate law expression for above reaction will be;

rate=k[BF3][NH3]

Expert Solution
Check Mark
Interpretation Introduction

(c)

Interpretation:

To determine the rate constant for the given reaction.

Concept introduction:

Rate of a chemical reaction: It tells us about the speed at which the reactants are converted into products.

Mathematically, rate of reaction is directly proportional to the product of concentration of each reactant raised to the power equal to their respective stoichiometric coefficients.

Let’s say we have a reaction:

aA+bBcC+dDthen,rateα[A]a[B]brate=Kf[A]a[B]bwhereKf= rateconstanta and b are order of reaction with respect to A and B 

Answer to Problem 25QAP

Rate constant for given reaction is 3.41L/mol.s

Explanation of Solution

Here the chemical reaction is:

BF3(g)+NH3(g)BF3NH3(g)

Rate law expression for above reaction:

rate=k[BF3][NH3]

Plugging values in rate law expression for experiment 1 as:

0.0341=k[0.100][0.100]

k=0.03410.100×0.100k=3.41L/mol.s

Hence, the rate constant is 3.41L/mol.s

Expert Solution
Check Mark
Interpretation Introduction

(d)

Interpretation:

To determine the rate of reaction at given concentration of reactants.

Concept introduction:

Rate of a chemical reaction: It tells us about the speed at which the reactants are converted into products.

Mathematically, rate of reaction is directly proportional to the product of concentration of each reactant raised to the power equal to their respective stoichiometric coefficients.

Let’s say we have a reaction:

aA+bBcC+dDthen,rateα[A]a[B]brate=Kf[A]a[B]bwhereKf= rateconstanta and b are order of reaction with respect to A and B 

Answer to Problem 25QAP

Rate of reaction for given reaction at given conditions is 0.5453mol/L.s

Explanation of Solution

Here the chemical reaction is:

BF3(g)+NH3(g)BF3NH3(g)

Rate law expression for above reaction:

rate=k[BF3][NH3]

Here we have:

[BF3 ]= 0.533 M

[NH3 ] = 0.300 M

Rate constant = 3.41 L/mol.s

Plugging values in rate law as:

rate=3.41[0.533][0.300]rate=0.5453mol/L.s

Hence, the rate of reaction is 0.5453mol/L.s

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Chapter 11 Solutions

Chemistry: Principles and Reactions

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