Chemistry: The Molecular Science
5th Edition
ISBN: 9781285199047
Author: John W. Moore, Conrad L. Stanitski
Publisher: Cengage Learning
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Textbook Question
Chapter 11, Problem 22QRT
Nitrosyl bromide, NOBr, is formed from NO and Br2.
Experiment shows that the reaction is first-order in Br2 and second-order in NO.
- (a) Write the rate law for the reaction.
- (b) If the concentration of Br2 is tripled, determine how the reaction rate changes.
- (c) Determine what happens to the reaction rate when the concentration of NO is doubled.
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Chapter 11 Solutions
Chemistry: The Molecular Science
Ch. 11.1 - For the reaction of crystal violet with NaOH(aq),...Ch. 11.1 - (a) From data in Table 11.1, calculate the rate of...Ch. 11.1 - For the reaction 4NO2(g)+O2(g)2N2O5(g) (a) express...Ch. 11.1 - Instantaneous rates for the reaction of hydroxide...Ch. 11.1 - Prob. 11.3CECh. 11.2 - Prob. 11.4ECh. 11.2 - Prob. 11.3PSPCh. 11.2 - Prob. 11.5ECh. 11.3 - Prob. 11.4PSPCh. 11.3 - Prob. 11.5PSP
Ch. 11.3 - Prob. 11.6PSPCh. 11.3 - Prob. 11.7PSPCh. 11.4 - Prob. 11.6ECh. 11.4 - Prob. 11.7CECh. 11.4 - Prob. 11.8PSPCh. 11.4 - Prob. 11.8CECh. 11.5 - Prob. 11.9PSPCh. 11.5 - The frequency factor A is 6.31 108 L mol1 s1 and...Ch. 11.6 - Prob. 11.10CECh. 11.7 - Prob. 11.11ECh. 11.7 - The Raschig reaction produces the industrially...Ch. 11.7 - Prob. 11.12ECh. 11.8 - The oxidation of thallium(I) ion by cerium(IV) ion...Ch. 11.9 - Prob. 11.11PSPCh. 11.9 - Prob. 11.14CECh. 11 - An excellent way to make highly pure nickel metal...Ch. 11 - Prob. 1QRTCh. 11 - Prob. 2QRTCh. 11 - Prob. 3QRTCh. 11 - Prob. 4QRTCh. 11 - Prob. 5QRTCh. 11 - Prob. 6QRTCh. 11 - Prob. 7QRTCh. 11 - Prob. 8QRTCh. 11 - Prob. 9QRTCh. 11 - Prob. 10QRTCh. 11 - Prob. 11QRTCh. 11 - Cyclobutane can decompose to form ethylene:
The...Ch. 11 - Prob. 13QRTCh. 11 - Prob. 14QRTCh. 11 - For the reaction 2NO2(g)2NO(g)+O2(g) make...Ch. 11 - Prob. 16QRTCh. 11 - Prob. 17QRTCh. 11 - Ammonia is produced by the reaction between...Ch. 11 - Prob. 19QRTCh. 11 - Prob. 20QRTCh. 11 - The reaction of CO(g) + NO2(g) is second-order in...Ch. 11 - Nitrosyl bromide, NOBr, is formed from NO and Br2....Ch. 11 - Prob. 23QRTCh. 11 - Prob. 24QRTCh. 11 - Prob. 25QRTCh. 11 - For the reaction
these data were obtained at 1100...Ch. 11 - Prob. 27QRTCh. 11 - Prob. 28QRTCh. 11 - Prob. 29QRTCh. 11 - Prob. 30QRTCh. 11 - Prob. 31QRTCh. 11 - Prob. 32QRTCh. 11 - For the reaction of phenyl acetate with water the...Ch. 11 - When phenacyl bromide and pyridine are both...Ch. 11 - The compound p-methoxybenzonitrile N-oxide, which...Ch. 11 - Prob. 36QRTCh. 11 - Radioactive gold-198 is used in the diagnosis of...Ch. 11 - Prob. 38QRTCh. 11 - Prob. 39QRTCh. 11 - Prob. 40QRTCh. 11 - Prob. 41QRTCh. 11 - Prob. 42QRTCh. 11 - Prob. 43QRTCh. 11 - Prob. 44QRTCh. 11 - Prob. 45QRTCh. 11 - Prob. 46QRTCh. 11 - Prob. 47QRTCh. 11 - Prob. 48QRTCh. 11 - Prob. 49QRTCh. 11 - Prob. 50QRTCh. 11 - Prob. 51QRTCh. 11 - Prob. 52QRTCh. 11 - For the reaction of iodine atoms with hydrogen...Ch. 11 - Prob. 54QRTCh. 11 - The activation energy Ea is 139.7 kJ mol1 for the...Ch. 11 - Prob. 56QRTCh. 11 - Prob. 57QRTCh. 11 - Prob. 58QRTCh. 11 - Prob. 59QRTCh. 11 - Prob. 60QRTCh. 11 - Prob. 61QRTCh. 11 - Prob. 62QRTCh. 11 - Prob. 63QRTCh. 11 - Which of the reactions in Question 62 would (a)...Ch. 11 - Prob. 65QRTCh. 11 - Prob. 66QRTCh. 11 - Prob. 67QRTCh. 11 - Prob. 68QRTCh. 11 - Prob. 69QRTCh. 11 - Prob. 70QRTCh. 11 - Prob. 71QRTCh. 11 - For the reaction the rate law is Rate=k[(CH3)3CBr]...Ch. 11 - Prob. 73QRTCh. 11 - Prob. 74QRTCh. 11 - Prob. 75QRTCh. 11 - For this reaction mechanism,
write the chemical...Ch. 11 - Prob. 77QRTCh. 11 - Prob. 78QRTCh. 11 - Prob. 79QRTCh. 11 - When enzymes are present at very low...Ch. 11 - Prob. 81QRTCh. 11 - The reaction is catalyzed by the enzyme succinate...Ch. 11 - Prob. 83QRTCh. 11 - Many biochemical reactions are catalyzed by acids....Ch. 11 - Prob. 85QRTCh. 11 - Prob. 86QRTCh. 11 - Prob. 87QRTCh. 11 - Prob. 88QRTCh. 11 - Prob. 89QRTCh. 11 - Prob. 90QRTCh. 11 - Prob. 91QRTCh. 11 - Prob. 92QRTCh. 11 - Prob. 93QRTCh. 11 - Prob. 94QRTCh. 11 - Nitryl fluoride is an explosive compound that can...Ch. 11 - Prob. 96QRTCh. 11 - Prob. 97QRTCh. 11 - For a reaction involving the decomposition of a...Ch. 11 - Prob. 99QRTCh. 11 - Prob. 100QRTCh. 11 - Prob. 101QRTCh. 11 - This graph shows the change in concentration as a...Ch. 11 - Prob. 103QRTCh. 11 - Prob. 104QRTCh. 11 - Prob. 105QRTCh. 11 - Prob. 106QRTCh. 11 - Prob. 107QRTCh. 11 - Prob. 108QRTCh. 11 - Prob. 109QRTCh. 11 - Prob. 110QRTCh. 11 - Prob. 111QRTCh. 11 - Prob. 112QRTCh. 11 - Prob. 113QRTCh. 11 - Prob. 114QRTCh. 11 - Prob. 115QRTCh. 11 - Prob. 116QRTCh. 11 - Prob. 118QRTCh. 11 - Prob. 119QRTCh. 11 - In a time-resolved picosecond spectroscopy...Ch. 11 - If you know some calculus, derive the integrated...Ch. 11 - If you know some calculus, derive the integrated...Ch. 11 - (Section 11-5) A rule of thumb is that for a...Ch. 11 - Prob. 11.BCPCh. 11 - Prob. 11.CCPCh. 11 - Prob. 11.DCP
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- At 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an initial concentration of 1.9 102 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant and the rate constant for this reaction, at 573 K, is 1.1 L/mol s.arrow_forwardOne experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?arrow_forwardNitrosyl bromide, NOBr, is formed from NO and Br2: 2 NO(g) + Br2(g) 2 NOBr(g) Experiments show that this reaction is second-order in NO and first-order in Br2. (a) Write the rate equation for the reaction. (b) How does the initial reaction rate change if the concentration of Br2 is changed from 0.0022 mol/L to 0.0066 mol/L? (c) What is the change in the initial rate if the concentration of NO is changed from 0.0024 mol/L to 0.0012 mol/L?arrow_forward
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- The reaction of CO(g) + NO2(g) is second-order in NO2 and zeroth-order in CO at temperatures less than 500 K. (a) Write the rate law for the reaction. (b) Determine how the reaction rate changes if the NO2 concentration is halved. (c) Determine how the reaction rate changes if the concentration of CO is doubled.arrow_forwardDinitrogen pentoxide, N2O5, decomposes when heated in carbon tetrachloride solvent.N2O5 →2NO2 + 1/2 O2(g) If the rate constant for the decomposition of N2O5 is 6.2 x10-4/min, what is the half-life? (The rate law is first order in N2O5.)(a) How long would it take for the concentration of N2O5 to decrease to 25% of its initial value? (b) To 12.5% of its initial value?arrow_forwardThe following kinetic data are collected for the initial rates of a reaction 2 X + Z→ products: Experiment [X ]o(M) [Z]o(M) Rate (M/s) 0.25 0.25 4.0 x 10! 0.50 0.50 3.2 x 102 0.50 0.75 7.2 x 102 (a) What is the rate law for this reaction? (b) What is the value of the rate constant with proper units? (c) What is the reaction rate when the initial concentration of X is 0.75 M and that of Z is 1.25 M? 2. 3.arrow_forward
- The reaction 2 NO₂(g) + O₂(g) → N₂O5(g) + O₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? Rate = k [NO₂(g)] [03(g)] O Rate = k [NO₂(g)]² [03(g)] O Rate = k [NO₂(g)] [03(g)]² O Rate = k [NO₂(g)]² [03(g)]² O Rate = k [NO₂(g)] [03(g)]³ O Rate = k [NO₂(g)]* [03(g)] (b) What is the value of the rate constant? 137268 Experiment M/S AWNPE 1 2 3 4 [NO₂(g)] (M) 0.718 0.718 1.44 1.44 [03(g)] (M) 0.718 1.44 0.718 1.44 Rate (M/s) (c) What is the reaction rate when the concentration of NO₂(g) is 1.26 M and that of O3(g) is 2.10 M if the temperature is the same as that used to obtain the data shown above? 26600 53400 53400 1.07e+05arrow_forwardThe reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Rate = k [0₂(g)] [NO(g)] O Rate = k [0₂(g)]² [NO(g)] O Rate = k [0₂(g)] [NO(g)]² O Rate = k [O₂(g)]² [NO(g)]²2 O Rate = k [O₂(g)] [NO(g)]³ O Rate = k [0₂(g)]4 [NO(g)] (b) What is the value of the rate constant? Experiment M/s 1 2 3 4 [0₂(g)] (M) 0.0231 0.0231 0.0462 0.0462 [NO(g)] (M) 0.0231 0.0462 0.0231 0.0462 Rate (M/s) 0.112 0.448 0.224 0.896 (c) What is the reaction rate when the concentration of O₂(g) is 0.0437 M and that of NO(g) is 0.0567 M if the temperature is the same as that used to obtain the data shown above?arrow_forwardExperiments show that each of the following redox reac-tions is second order overall:Reaction 1: NO₂(g)+CO(g) →NO(g)+CO₂(g) Reaction 2: NO(g)+O₃(g) →NO₂(g)+O₂(g) (a) When [NO₂] in reaction 1 is doubled, the rate quadruples.Write the rate law for this reaction.(b) When [NO] in reaction 2 is doubled, the rate doubles. Writethe rate law for this reaction.(c) In each reaction, the initial concentrations of the reactantsare equal. For each reaction, what is the ratio of the initial rateto the rate when the reaction is 50% complete?(d) In reaction 1, the initial [NO₂] is twice the initial [CO].What is the ratio of the initial rate to the rate at 50% completion?(e) In reaction 2, the initial [NO] is twice the initial [O₃]. Whatis the ratio of the initial rate to the rate at 50% completion?arrow_forward
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