Chemistryplease i need the answer of any two of themthanks. The following initial rate data are for the gas phase reaction of hydrogen with iodine:H₂+1₂ → 2 HIExperiment [H₂0, M [12]o, M Initial Rate, M-s-¹0.01720.01374.24 x 10-220.01720.02758.51 x 10-220.03440.01378.48 x 10-220.03440.02751.70 x 10-21234Complete the rate law for this reaction in the box below.Use the formk[A] [B]", where '1' is understood form orn and concentrations taken to the zero power do not appear. Don't enter 1 form or11.Rate=k=M-1 The following initial rate data are for the oxidation of nitrogen monoxide by oxygen at 25 °C:2NO+O₂ → 2NO₂Experiment [NO]o, M[02]o, MInitial Rate, M-s-¹S0.002020.003260.0001190.004040.003260.0004770.002020.006520.0002380.00404 0.00652 0.000953Complete the rate law for this reaction in the box below.Use the formk[A] [B]", where '1' is understood for134m orn and concentrations taken to the zero power do not appear. Don't enter 1 form orn.Rate =k=M-2.8-¹

Answered: Image /qna-images/answer/170bda9f-e9c7-4b5e-938c-74e68fe206f5.jpg

The following initial rate data are for the gas phase reaction of hydrogen with iodine: H₂+1₂ → 2 HI Experiment 1 2 3 4 [H₂0, M [12]o, M Initial Rate, M-s 0.0172 0.0137 4.24 x 10 0.0172 0.0275 8.51 x 10-22 0.0344 0.0137 8.48 x 10-22 0.0344 0.0275 1.70 x 10-2 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for Rate= -22 m or n and concentrations taken to the zero power do not appear. Don't enter 1 for mor 11. k= M-1-1

The following initial rate data are for the gas phase reaction of hydrogen with iodine: H₂+1₂ → 2 HI Experiment 1 2 3 4 [H₂0, M [12]o, M Initial Rate, M-s 0.0172 0.0137 4.24 x 10 0.0172 0.0275 8.51 x 10-22 0.0344 0.0137 8.48 x 10-22 0.0344 0.0275 1.70 x 10-2 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for Rate= -22 m or n and concentrations taken to the zero power do not appear. Don't enter 1 for mor 11. k= M-1-1

Chemistry for Engineering Students

3rd Edition

ISBN:9781285199023

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.52PAE

See similar textbooks

Similar questions

The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
Sulfuryl chloride (SO2Cl2) decomposes to sulfur dioxide (SO2) and chlorine (Cl2) by reaction in the gas phase. The following pressure data were obtained when a sample containing 5.00 102 mol sulfuryl chloride was heated to 600. K in a 5.00 101-L container. Time (hours): 0.00 1.00 2.00 4.00 8.00 16.00 PSO2Cl2(atm): 4.93 4.26 3.52 2.53 1.30 0.34 Defining the rate as [SO2Cl2]t, a. determine the value of the rate constant for the decomposition of sulfuryl chloride at 600. K. b. what is the half-life of the reaction? c. what fraction of the sulfuryl chloride remains after 20.0 h?
11.32 The following experimental data were obtained for the reaction 2A + 3 B—C + 2D [A](mol L 1) [B](mol L ’) Rate = A(C]/Af (mol L-1 s-1) 0.127 0.15 0.033 0.127 0.30 0.132 0.255 0.15 0.066 Determine the reaction order for each reactant and the value of the rate constant.
Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following initial rates of reaction have been observed for certain reactant concentrations: [NO] (moI/L1) [CI2] (mol/L) Rate (moI/L/h) 0.50 0.50 1.14 1.00 0.50 4.56 1.00 1.00 9.12 What is the rate equation that describes the rate’s dependence on the concentrations of NO and CI2? What is the rate constant? What are the orders with respect to each reactant?
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.
Consider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5
A study of the rate of the reaction represented as 2AB gave the following data: Time (s) 0.0 5.0 10.0 15.0 20.0 25.0 35.0 [A](M) 1.00 0.775 0.625 0.465 0.350 0.205 0.230 (a) Determine the average rate of disappearance of A between 0.0 s and 10.0 s, and between 10.0 s and 20.0 s. (b) Estimate the instantaneous rate of disappearance of A at 15.0 s from a graph of time versus [A]. What are theunits of this rate? (c) Use the rates found in parts (a) and (b) to determine the average rate of formation of B between 0.00 s and 10.0 s, and the instantaneous rate of formation of B at 15.0 s.
In Exercise 11.39, if the initial concentration of N2Oj is 0.100 .\1. how long will it take for the concentration to drop to 0.0100 times its original value? The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction: 2N2O5—»4NO2 + O2 The rate constant at a given temperature is found to be 5.25 X 10-4 s-’. If the initial concentration of N2O5 is 0.200 M, what is its concentration after exactly 10 minutes have passed?
6. Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5°C. Time (s) [Phenyl acetate] (mol/L) 0 0.55 15.0 0.42 30.0 0.31 45.0 0.23 60.0 0.17 75.0 0.12 90.0 0.085 Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. Calculate the rate of change of the phenyl acetate concentration during the period 15.0 seconds to 30.0 seconds and also during the period 75.0 seconds to 90.0 seconds. Why is one value smaller than the other? What is the rate of change of the phenyl acetate concentration during the time period 60.0 seconds to 75.0 seconds? What is the instantaneous rate at 15.0 seconds?
Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5 C. (a) Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. (b) Calculate the rate of change of the phenyl acetate concentration during the period 15.0 seconds to 30.0 seconds and also during the period 75.0 seconds to 90.0 seconds. Why is one value smaller than the other?
At 40C, H2O2 (aq) will decompose according to the following reaction: 2H2O2(aq)2H2O(l)+O2(g) The following data were collected for the concentration of H2O2 at various times. Times(s) [H2O2](mol/L) 0 1.000 2.16 104 0.500 4.32 104 0.250 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.16 104 s. Use this rate to calculate the average rate of production of O2(g) over the same time period. b. What are these rates for the time period 2.16 104 s to 4.32 104 s?
Ammonia decomposes when heated according to the equation NH3(g) NH2(g) + H(g) The data in the table for this reaction were collected at a high temperature. Plot In [NH3] versus time and 1/[NH3] versus time. What is the order of this reaction with respect to NH3? Find the rate constant for the reaction from the slope.