Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
Chapter 11, Problem 66QAP
Interpretation Introduction
(a)
Interpretation:
The chirping rates should be determined at the temperature
Concept introduction:
The decomposition reaction can be determined when one compound is broken into two or more products.
Interpretation Introduction
(b)
Interpretation:
The activation energy of the given reaction should be determined.
Concept introduction:
Activation energy is defined as the amount of energy required in the reaction to activate the atoms of molecules to undergo reaction and form a new product.
Interpretation Introduction
(c)
Interpretation:
The percentage increase in rate for rise of
Concept introduction:
The rate of reaction represents the speed of the
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
The water in a pressure cooker boils at a temperature
greater than 100°C because it is under pressure. At this
higher temperature, the chemical reactions associated with
the cooking of food take place at a greater rate.
(a) Some food cooks fully in 5 min in a pressure cooker
at 112°C and in 10 minutes in an open pot at 100°C.
Calculate the average activation energy for the reac-
tions associated with the cooking of this food.
(b) How long will the same food take to cook in an open
pot of boiling water in Denver, where the average
atmospheric pressure is 0.818 atm and the boiling
point of water is 94.4°C?
(a) Define the following terms:(i) Collision frequency(ii) Rate constant (k)(b) The rate constant of a first order reaction increases from 4 X 10-2 to 24 X 10-2 when the temperature changes from 300 K to 350 K. Calculate the energy of activation (JEa). (log 2 = 0.301, log 3 = 0.4771, log 4 = 0.6021, log 6 = 0.7782)
The water in a pressure cooker boils at a temperature greater than 100°C because it is under pressure. At this higher temperature, the chemical reactions associated with the cooking of food take place at a greater rate.(a) Some food cooks fully in 5 min in a pressure cooker at 112°C and in 10 minutes in anopen pot at 100°C. Calculate the average activation energy for the reactions associatedwith the cooking of this food.(b) How long will the same food take to cook in an open pot of boiling water in Denver,where the average atmospheric pressure is 0.818 atm and the boiling point of water is94.4°C?
Chapter 11 Solutions
Chemistry: Principles and Reactions
Ch. 11 - Express the rate of the reaction...Ch. 11 - Express the rate of the reaction...Ch. 11 - Consider the following hypothetical reaction: X( g...Ch. 11 - Consider the following hypothetical reaction:...Ch. 11 - Consider the combustion of ethane:...Ch. 11 - For the reaction 5Br(aq)+BrO3(aq)+6...Ch. 11 - Nitrosyl chloride (NOCI) decomposes to nitrogen...Ch. 11 - Ammonia is produced by the reaction between...Ch. 11 - Experimental data are listed for the following...Ch. 11 - Experimental data are listed for the hypothetical...
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...
Knowledge Booster
Similar questions
- The precipitation of egg albumin in water at 100C has an activation energy of 52.0 kJ/mol. By what percent does the rate of precipitation decrease if the water is at 92C?arrow_forwardSuppose that the half-life of steroids taken by an athlete is 42 days. Assuming that the steroids biodegrade by a first-order process 5, how long would it take for 164 of the initial dose to remain in the athlete’s body?arrow_forwardList at least four experimentally determined parameters that you, an experimenter, can define when exploring the hydrolysis of ethyl benzoate by aqueous sodium hydroxide.arrow_forward
- Bacteria cause milk to go sour by generating lactic acid. Devise an experiment that could measure the activation energy for the production of lactic acid by bacteria in milk. Describe how your experiment will provide the information you need to determine this value. What assumptions must be made about this reaction?arrow_forward. explain the difference between elementary reactions and multistep reactions.arrow_forwardThe rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.arrow_forward
- Experiments during a recent summer on a number of fireflies (small beetles, Lampyridaes photinus) showed that the average interval between flashes of individual insects was 16.3 s at 21.0C and 13.0 sat 27.8C. a. What is the apparent activation energy of the reaction that controls the flashing? b. What would be the average interval between flashes of an individual firefly at 30.0C? c. Compare the observed intervals and the one you calculated in part b to the rule of thumb that the Celsius temperature is 54 minus twice the interval between flashes.arrow_forwardThe degradation of the antibiotic clindamycin stored at 343 K in aqueous solution at pH 4 is found to be first order with a rate constant of 2.49 x 10−7 s −1. Over the temperature range 320 K to 360 K theactivation energy was found to be 123.3 kJ mol−1. (a) Calculate the rate constant at 325 K.(b) The threshold for product safety is 1% degradation. At 295 K the time taken for 1% of the antibiotic to degrade is found to be close to 0.01/ k. Comment on the shelf-life of the drug.arrow_forwardCertain bacteria use the enzyme penicillinase to decom- pose penicillin and render it inactive. The Michaelis- Menten constants for this enzyme and substrate are Km = 5 × 10-5 mol L-ªand k, = 2 × 10³ s¯1. (a) What is the maximum rate of decomposition of peni- cillin if the enzyme concentration is 6 × 10-7 M? (b) At what substrate concentration will the rate of decomposition be half that calculated in part (a)?arrow_forward
- The reaction between ethyl iodide and hydroxide ion inethanol (C2H5OH) solution, C2H5(1alc) + OH- (1alc)----->C2H5OH(l) + I - (alc) , has an activation energy of86.8 kJ>mol and a frequency factor of 2.10 x 1011 M-1 s-1.(a) Predict the rate constant for the reaction at 35 °C. (b) Asolution of KOH in ethanol is made up by dissolving 0.335g KOH in ethanol to form 250.0 mL of solution. Similarly,1.453 g of C2H5I is dissolved in ethanol to form 250.0mL of solution. Equal volumes of the two solutions aremixed. Assuming the reaction is first order in each reactant,what is the initial rate at 35 °C? (c) Which reagent inthe reaction is limiting, assuming the reaction proceeds tocompletion? (d) Assuming the frequency factor and activationenergy do not change as a function of temperature,calculate the rate constant for the reaction at 50 °C.arrow_forwardA particular second-order reaction has a rate constant of 2.4 x 10–6 M–1 s–1 at 575 K and 6.0 x 10–5 M–1 s–1 at 630 K. (a) Calculate the activation energy of the reaction. (b) What is the value of the rate constant at 25°C?arrow_forward(a) Distinguish between reactions rate and reaction mechanism (b) The following data were obtained for the reaction I'aq + OCI aq→ IO" + CI'aq [OCI ] [1] mol/dm3 Initial Rate mol/dm3 mol/dm?/s 1.8 x 103 3.6 х 103 2.1 x 103 5.4 x 105 2.1 x 103 10.8 x 10$ I II I 1.8х 103 (i)What is the order of the reaction with respect to [I'] and [OCI] (ii) Calculate the rate constant using the results of experiment II (iii) What is the rate law or rate equation for this reaction? 6.3х 103 4.9 x 104arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781285199023Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781285199023
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning