What are the missing entries in the table?Run [C,H,Br,b (M)[I-], (M)Initial rate of formation of C,H, (M-s )10.2150.001050.215y0.00052430.2150.2150.712X =Incorrect0.356y =Incorrect0.000179= ZIncorrect Consider the reaction described by the equationС,Н, Вг, (аq) + 3Г (аq)С,Н, (9) + 2 Br (aq) + I; (aq)The rate law israte = k [C,H,Br,][I¯]-2where k =0.00567 M-1.s-1.What are the missing entries in the table?Run| [C, H, Br, h (M) | (М)Initial rate of formation of C,H, (M-s )10.2150.0010520.215y0.00052430.2150.2150.712X =Incorrect0.356y =

The speed of the chemical reaction is measured in terms of rate Here we are required to complete…

Consider the reaction described by the equation C,H,Br, (aq) + 3I(aq) → C,H,(g) + 2 Br¯(aq) + I5 (aq) The rate law is rate = k [C,H,Br,]I] %3D where k = 0.00567 M-1. s-1. What are the missing entries in the table? Run [C,H,Br, (M) | [I-lo (M) Initial rate of formation of C,H, (M-s ¯') 1 0.215 0.00105 0.215 y 0.000524 0.215 0.215 0.712 x = Incorrect 0.356 y =

Consider the reaction described by the equation C,H,Br, (aq) + 3I(aq) → C,H,(g) + 2 Br¯(aq) + I5 (aq) The rate law is rate = k [C,H,Br,]I] %3D where k = 0.00567 M-1. s-1. What are the missing entries in the table? Run [C,H,Br, (M) | [I-lo (M) Initial rate of formation of C,H, (M-s ¯') 1 0.215 0.00105 0.215 y 0.000524 0.215 0.215 0.712 x = Incorrect 0.356 y =

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 30QAP

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Azomethane decomposes into nitrogen and ethane at high temperatures according to the following equation: (CH3)2N2(g)N2(g)+C2H6(g)The rate of the reaction is followed by monitoring the disappearance of the purple color due to iodine. The following data are obtained at a certain temperature. (a) By plotting the data, show that the reaction is first-order. (b) From the graph, determine k. (c) Using k, find the time (in hours) that it takes to decrease the concentration to 0.100 M. (d) Calculate the rate of the reaction when [ (CH3)2N2 ]=0.415M.
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, fur the reaction was measured at several different temperatures and the data are shown here: Temperature (K) k (M -1 5-1) 555 6.23107 575 2.42106 645 1.44104 700 2.01103 What is the value of the activation energy (in kJ/mol) for this reaction?
Consider the following energy diagram (not to scale) for the reaction. 2CH3(g)C2H6(g) (a) What is the activation energy of the forward reaction? (b) At what point would 2CH3 (g) appear? (c) What is H for the reaction? (d) What is the activation energy of the reverse reaction? (e) At what point would C2H6 certainly be found? (f) What is any species at point C called?
Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
The reaction H2SeO3(aq) + 6I-(aq) + 4H+(aq) Se(s) + 2I-3(aq) + 3H2O(l) was studied at 0C, and the following data were obtained: [H2SeO3]0 (mol/L) [H+]0 (mol/L) [I]0(mol/L) Initial Rate (mol/L s) 1.0 104 2.0 102 2.0 102 1.66 107 2.0 104 2.0 102 2.0 10-2 3.33 107 3.0 104 2.0 102 2.0 102 4.99 107 1.0 104 4.0 102 2.0 102 6.66 107 1.0 104 1.0 102 2.0 102 0.42 107 1.0 104 2.0 102 4.0 102 13.2 107 1.0 104 1.0 102 4.0 102 3.36 107 These relationships hold only if there is a very small amount of I3 present. What is the rate law and the value of the rate constant? (Assumethatrate=[H2SeO3]t)
The following rate constants were obtained in an experiment in which the decomposition of gaseous N2O; was studied as a function of temperature. The products were NO, and NO,. Temperature (K) 3.5 x 10_i 298 2.2 x 10"4 308 6.8 X IO-4 318 3.1 x 10 1 328 Determine Etfor this reaction in kj/mol.
For a first order gas phase reaction A products, k = 7.2 104s1 at 660. K and k = 1.7 102s1 at 720. K. If the initial pressure of A is 536 torr at 295C, how long will it take for the pressure of A to decrease to 268 torr?
11.35 For the reaction 2 NO(g) + 2 H?(g) — N,(g) + 2 H,O(g) at 1100°C, the following data have been obtained: [NOJ [HJ Rate = A(N2]/At (mol L~1) (mol L_1) (mol L-1 s_1) 5.0 X 10’1 0.32 0.012 1.0 X 10~’ 0.32 0.048 1.0 X 10"2 0.64 0.096 Derive a rate law for the reaction and determine the value of the rate constant.
The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?