EBK CHEMISTRY: PRINCIPLES AND REACTIONS
EBK CHEMISTRY: PRINCIPLES AND REACTIONS
8th Edition
ISBN: 8220100547966
Author: Hurley
Publisher: CENGAGE L
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Chapter 11, Problem 19QAP

The decomposition of nitrogen dioxide is a second-order reaction. At 550 K, a 0.250 M sample decomposes at the rate of 1.17 mol/L

min.

(a) Write the rate expression.

(b) What is the rate constant at 550 K?

(c) What is the rate of decomposition when [ NO 2 ] = 0.800 M ?

Expert Solution
Check Mark
Interpretation Introduction

(a)

Interpretation:

To write the expression of rate from the given statement of a chemical 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 19QAP

Expression of rate is:

rate=k[NO2]2

Explanation of Solution

Nitrogen dioxide decomposes into nitrogen and oxygen gas as:

2NO2(g)N2(g)+2O2(g)

Since the order of reaction with respect to NO2 is second. Thus, rate law equation will look like:

2NO2(g)N2(g)+2O2(g)rate=k[NO2]2

Expert Solution
Check Mark
Interpretation Introduction

(b)

Interpretation:

To determine the value of rate constant at 550 K.

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 19QAP

Rate constant for given reaction, k=18.72L/molmin1.

Explanation of Solution

Nitrogen dioxide decomposes into nitrogen and oxygen gas as:

2NO2(g)N2(g)+2O2(g)

Since the order of reaction with respect to NO2 is second. Thus, rate law equation will look like:

2NO2(g)N2(g)+2O2(g)rate=k[NO2]2........(1)

Here we have:

Rate = 1.17 mol/L.min

[NO2 ] = 0.250 M

Plugging value of rate of reaction in equation 1 to get the value of rate constant as:

rate=k[NO2]21.17mol/L.min=k(0.250)2k=18.72L/molmin1

Expert Solution
Check Mark
Interpretation Introduction

(c)

Interpretation:

To determine the value of rate of reaction when concentration of nitrogen dioxide is 0.800 M.

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 19QAP

Rate for given reaction when concentration of nitrogen dioxide is 0.800 M =11.981 M/min.

Explanation of Solution

Nitrogen dioxide decomposes into nitrogen and oxygen gas as:

2NO2(g)N2(g)+2O2(g)

Since the order of reaction with respect to NO2 is second. Thus, rate law equation will look like:

2NO2(g)N2(g)+2O2(g)rate=k[NO2]2........(1)

Here we have:

Rate constant= 18.72 L/mol.min

[NO2 ] = 0.800 M

Plugging value of rate of reaction in equation 1 to get the value of rate constant as:

rate=k[NO2]2rate=(18.72)×(0.800)2rate=11.981mol/L.min

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Chapter 11 Solutions

EBK CHEMISTRY: PRINCIPLES AND REACTIONS

Ch. 11 - A reaction has two reactants X and Y. What is the...Ch. 11 - A reaction has two reactants Q and P. What is the...Ch. 11 - What will the units of the rate constants in...Ch. 11 - What will the units of the rate constants in...Ch. 11 - Consider the reaction ZproductsThe data below give...Ch. 11 - Consider the reaction YproductsThe graph below...Ch. 11 - Complete the following table for the reaction...Ch. 11 - Complete the following table for the reaction...Ch. 11 - The decomposition of nitrogen dioxide is a...Ch. 11 - The decomposition of ammonia on tungsten at 1100C...Ch. 11 - The reaction ICl(g)+12 H2(g)12 I2(g)+HCl(g)is...Ch. 11 - The hypothetical reaction X(g)+12Y(g)productsis...Ch. 11 - For a reaction involving the decomposition of Z at...Ch. 11 - For a reaction involving the decomposition of Y,...Ch. 11 - When boron trifluoride reacts with ammonia, the...Ch. 11 - When nitrogen dioxide reacts with carbon monoxide,...Ch. 11 - Hydrogen bromide is a highly reactive and...Ch. 11 - Diethylhydrazine reacts with iodine according to...Ch. 11 - The equation for the reaction between iodide and...Ch. 11 - Prob. 30QAPCh. 11 - In a solution at a constant H+ concentration,...Ch. 11 - Consider the reaction Â...Ch. 11 - Nitrosyl bromide decomposes to nitrogen oxide and...Ch. 11 - Prob. 34QAPCh. 11 - Azomethane decomposes into nitrogen and ethane at...Ch. 11 - The decomposition of sulfuryl chloride, SO2Cl2, to...Ch. 11 - The first-order rate constant for the...Ch. 11 - Consider the first-order decomposition of phosgene...Ch. 11 - The decomposition of azomethane, (CH3)2N2, to...Ch. 11 - The first-order rate constant for the...Ch. 11 - In the first-order decomposition of acetone at...Ch. 11 - The decomposition of sulfuryl chlorideSO2Cl2fur...Ch. 11 - Dinitrogen pentoxide gas decomposes to form...Ch. 11 - Sucrose (C12H22O11) hydrolyzes into glucose and...Ch. 11 - Iodine-131 is used to treat tumors in the thyroid....Ch. 11 - Cesium-131 is the latest tool of nuclear medicine....Ch. 11 - Prob. 47QAPCh. 11 - A sample of sodium-24 chloride contains 0.050 mg...Ch. 11 - The decomposition of A at 850C is a zero-order...Ch. 11 - The decomposition of R at 33C is a zero-order...Ch. 11 - For the zero-order decomposition of HI on a gold...Ch. 11 - For the zero-order decomposition of ammonia on...Ch. 11 - Ammonium cyanate, NH4NCO, in water rearranges to...Ch. 11 - Butadiene, C4H6, dimerizes according to the...Ch. 11 - The rate constant for the second-order reaction...Ch. 11 - The decomposition of nitrosyl chloride...Ch. 11 - An increase in temperature from 23C to 36C...Ch. 11 - If the activation energy of a reaction is 9.13 kJ,...Ch. 11 - The following data are obtained for the gas-phase...Ch. 11 - The following data are obtained for the...Ch. 11 - Consider the following hypothetical reaction:...Ch. 11 - For the reaction: Q+RY+ZH=128kJ Draw a...Ch. 11 - The uncoiling of deoxyribonucleic acid (DNA) is a...Ch. 11 - The precipitation of egg albumin in water at 100C...Ch. 11 - Prob. 65QAPCh. 11 - Prob. 66QAPCh. 11 - For the reaction 2N2O(g)2N2(g)+O2(g) the rate...Ch. 11 - For the decomposition of a peroxide, the...Ch. 11 - Consider a 5.000 M solution of the hypothetical...Ch. 11 - The decomposition of N2O5 to NO2 and NO3 is a...Ch. 11 - For a certain reaction, Ea is 135 kJ and H=45 kJ....Ch. 11 - Consider a reaction in which E a=129 kJ and H=29...Ch. 11 - A catalyst lowers the activation energy of a...Ch. 11 - A reaction has an activation energy of 363 kJ at...Ch. 11 - Write the rate expression for each of the...Ch. 11 - Write the rate expression for each of the...Ch. 11 - For the reaction between hydrogen and iodine,...Ch. 11 - For the reaction 2H2(g)+2NO(g)N2(g)+2H2O(g) the...Ch. 11 - At low temperatures, the rate law for the reaction...Ch. 11 - Two mechanisms are proposed for the reaction...Ch. 11 - The hypothetical reaction QR+Xproductswas...Ch. 11 - When a base is added to an aqueous solution of...Ch. 11 - The decomposition of sulfuryl chloride, SO2Cl2, to...Ch. 11 - How much faster would a reaction proceed at 46C...Ch. 11 - Prob. 85QAPCh. 11 - Prob. 86QAPCh. 11 - A drug decomposes in the blood by a first-order...Ch. 11 - Prob. 88QAPCh. 11 - Prob. 89QAPCh. 11 - Prob. 90QAPCh. 11 - Consider the decomposition of A represented by...Ch. 11 - Consider the decomposition reaction 2X2Y+ZThe...Ch. 11 - Consider the following activation energy diagram....Ch. 11 - Three first-order reactions have the following...Ch. 11 - Consider the first-order decomposition reaction...Ch. 11 - Consider the following energy diagram (not to...Ch. 11 - Prob. 97QAPCh. 11 - Prob. 98QAPCh. 11 - The gas-phase reaction between hydrogen and iodine...Ch. 11 - Consider the coagulation of a protein at 100C. The...Ch. 11 - Prob. 101QAPCh. 11 - Prob. 102QAPCh. 11 - Prob. 103QAPCh. 11 - In a first-order reaction, suppose that a quantity...Ch. 11 - Consider the hypothetical first-order reaction...
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Kinetics: Initial Rates and Integrated Rate Laws; Author: Professor Dave Explains;https://www.youtube.com/watch?v=wYqQCojggyM;License: Standard YouTube License, CC-BY