(d) Identify the catalyst in the reaction.O H₂OorH₂O2O HOI(e) Identify a reactant in the reaction.O H₂O2OrO HOIH₂O(f) Identify a product in the reaction.H₂O2O H₂OO HOIOr The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism:(a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process.O Rate = k [I] [HO]O Rate = k [1] [H₂0₂]O Rate = k [H₂0₂]²O Rate = k [HOI] [H₂0₂]O Rate = k [H₂0₂] [H₂02]O Rate = k [H₂0₂]² [H₂0₂](b) Choose the correct chemical equation for the overall process.O 2 HzOz(aq) --> 2 HzO(l) + Oz(g)O HOI(aq) + OH(aq) --> H₂O(l) + 01 (aq)O H₂O₂(aq) + 1°(aq) --> HOI(aq) + OH (aq)(c) Identify an intermediate in the reaction.OrO H₂O2O HOIO H₂OH₂O₂(aq) + (aq) --> HOI(aq) + OH(aq) (slow)HOI(aq) + OH(aq) --> H₂O(l) + OI (aq)OI (aq) + H₂O₂(aq) --> HOOI(aq) + OH (aq)HOOI(aq) + OH(aq) --> H₂O(l) + O₂(g) + (aq)

Kindly repost d, e, f questions seperately.

The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism: (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. O Ratek [I] [HOT] O Rate = k [1] [H₂0₂] O Rate = k [H₂0₂1² O Rate = k [HOI] [H₂0₂] O Rate = k [H₂0₂] [H₂0₂] O Rate = k [H₂0₂]² [H₂0₂] (b) Choose the correct chemical equation for the overall process. O2 H2Oz(aq) -- 2 H2O(l) + O2(s) HOI(aq) + OH(aq) --> H₂O(l) + 01 (aq) O H₂O₂(aq) + 1'(aq) --> HOI(aq) + OH(aq) (c) Identify an intermediate in the reaction. Or O H₂02 O HOI O H2O H₂O₂(aq) + (aq) --> HOI(aq) + OH(aq) (slow) HOI(aq) + OH(aq) --> H₂O(1) + 01¹(aq) or (aq) + H₂O₂(aq) --> HOOI(aq) + OH (aq) HOOI(aq) + OH(aq) --> H₂O(l) + O₂(g) + (aq)

The iodide-catalyzed decomposition of hydrogen peroxide is thought to proceed by a four-step mechanism: (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. O Ratek [I] [HOT] O Rate = k [1] [H₂0₂] O Rate = k [H₂0₂1² O Rate = k [HOI] [H₂0₂] O Rate = k [H₂0₂] [H₂0₂] O Rate = k [H₂0₂]² [H₂0₂] (b) Choose the correct chemical equation for the overall process. O2 H2Oz(aq) -- 2 H2O(l) + O2(s) HOI(aq) + OH(aq) --> H₂O(l) + 01 (aq) O H₂O₂(aq) + 1'(aq) --> HOI(aq) + OH(aq) (c) Identify an intermediate in the reaction. Or O H₂02 O HOI O H2O H₂O₂(aq) + (aq) --> HOI(aq) + OH(aq) (slow) HOI(aq) + OH(aq) --> H₂O(1) + 01¹(aq) or (aq) + H₂O₂(aq) --> HOOI(aq) + OH (aq) HOOI(aq) + OH(aq) --> H₂O(l) + O₂(g) + (aq)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

24.) At 700 °C, hydrogen gas reduces nitric oxide according to the equation 2H2(g) + 2NO(g)  2H2O(g) + N2(g) whichobeys the rate law, Rate = k [H2][NO]2. What is the value of the rate constant, in 1M2⋅h , if the initial rate of thereaction is 0.183 M/h when the initial [H2] = 0.220 M and the initial [NO] = 0.250 M.a. 3.33 b. 0.075 c. 0.003 d. 13.33 e. 15.15
Consider the following reaction: 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g)(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M?Rate = _______ M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00858 M while the concentration of O2(g) is 0.00758 M?Rate = _______ M/s
[4] Consider the following mechanism for the reaction of nitric oxide and hydrogen: kı 2NO(g)+ H2(g) → N;O(g) + H¿O(g) slow k2 N,0(g) + H2(g) → N2(g) + H2O(g) fast (a) Write an equation for the overall reaction. (b) Write the theoretical rate law for the above mechanism. (c) Is a catalyst involved in the above mechanism? If so, what is it? (d) Are there any reaction intermediates? If so, list them.
5*) a) The reaction A B has been experimentally determined to be second order. The initial rate is 0.0100 M/s at an initial concentration of [A] of 0.100 M. What is the initial rate at [A]o = 0.500 M? b) The reaction below was experimentally determined to be first order with respect to O2 and second order with respect to NO. O2(g) + 2 NO(g) → 2 NO2(g) The diagrams provided represent reaction mixtures in which the number of each type of molecule represents its relative initial concentration. Which mixture has the fastest initial rate? Explain. KEY: = 02 = NO (i) (ii) (iii)
The decomposition of NOBr is studied manometrically because the number of moles of gas changes; it cannot be studied colorimetrically because both NOBr and Br2 are reddish-brown. 2NOBr(g) →2NO(g) + Br2(g) Use the data below to make the following determinations: (a) the average rate of decomposition of NOBr over the entire experiment. (b) the average rate of decomposition of NOBr between 2.00 and 4.00 seconds. Time (s) [NOBr] (mol/L) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00 0.0033 The rates of decomposition of NOBr are (a) mol L−1 s−1 (b) mol L−1 s−1
(d) Decreasing the pressure of NO, from 0.50 atm to 0.250 atm. (b) Increasing the concentration of CO from 0.01 M to 0.03 M. 16. How will each of the following affect the rate of the reaction: CO(g)+ NO2(8) → CO2(8) + NO(6) se. -> rate law for the reaction is rate = K[NO2][CO] ? (a) Increasing the pressure of NO, from 0.1 atm to 0.3 atm (b) Increasing the concentration of CO from 0.02 M to 0.06 M. 17 Reaul
Identify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. Reaction Molecularity Rate expression (a) NO2 + NO2→2 NO + 02 rate = (b) BrONO- ЭBro + NOz rate = (c) 0+ 02 + M 03 + M rate = unimolecular bimolecular termolecular
The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C H,O2(aq)H,0() + ½ O2(g) is first order in H20, with a rate constant of 1.10x10-3 min!. If the initial concentration of H,O, is 6.48×10-2 M, the concentration of H,O, will be 1.17x10-2 M after min have passed.
The first order rate constant for the decomposition of N2Os to NO2 and O2 at 70 °C is 6.82 x 10-3 s. Suppose we start with 0.300 mol of N,O5(g) in a 0.5 dm container. 5. (a) How many moles of N2O5 will remain after 1.5 minutes? (b) How many minutes will it take for the concentration of N2O5 to decrease by 0.4 M? (c) What is the half-life of N2O5 at 70 °C? (d) How long will it take for [N2O5] to decrease to 20 % of its original value?
6. The rate constant for the reaction, 2 N₂O5 (g) → 4 NO2 (g) + O2 (g), doubles when the temperature is raised from 295.65 K to 300.62 K. (a) Determine the activation energy (in kJ/mol) for the reaction, assuming that the pre- exponential factor, A, in the Arrhenius equation is independent of temperature. (b) At what temperature would you predict this rate constant to increase by another factor of 10 relative to its value at 300.62 K?
The following data was obtained from the reaction: (a) Determine the rate law. (b) Calculate the rate constant. (c) Calculate the initial rate, if [NO2~] = 0.1 M and [NH4+] = 0.1 M
For the zero-order decomposition of HI on a gold surface HI (g) →Au1/2 H2 (g) + 1/2 I2(g) it takes 16.0 s for the pressure of HI to drop from 1.00 atm to 0.200 atm. (a) What is the rate constant for the reaction?(b) How long will it take for the pressure to drop from 0.150 atm to 0.0432 atm?(c) What is the half-life of HI at a pressure of 0.500 atm?