The following initial rate data are for the reaction of ICI with hydrogen: 2 ICI + H2→I2 + 2 HCI Experiment [IC]], M [H2],, M Initial Rate, M s1 1 0.356 0.165 1.80x10-2 2 0.712 0.165 3.61x10-2 3 0.356 0.330 7.21x10-2 4 0.712 0.330 0.144 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]* , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M-251.

The following initial rate data are for the reaction of ICI with hydrogen: 2 ICI + H2→I2 + 2 HCI Experiment [IC]], M [H2],, M Initial Rate, M s1 1 0.356 0.165 1.80x10-2 2 0.712 0.165 3.61x10-2 3 0.356 0.330 7.21x10-2 4 0.712 0.330 0.144 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]* , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is M-251.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.50PAE

See similar textbooks

Similar questions

Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 C and their first-order decomposition studied. Determine the average rate constants for each experiment using the following data: Initial [C3H5N3O9] (M) 4.88 3.52 2.29 1.81 5.33 4.05 2.95 1.72 t (s) 300 300 300 300 180 180 180 180 %Decomposed 52.0 52.9 53.2 53.9 34.6 35.9 36.0 35.4
The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common laboratory experiment used in general chemistry courses to teach the method of initial rates. The reaction is followed spectrophotometrically by the disappearance of the color of iodine in the solution. The following data (J. P. Birk and D. L Walters, Journal of Chemical Education, Vol. 69, p. 585, 1992) were collected at 23 C for this reaction. Determine the rate law for this reaction.
11.48 The following data were collected for the decomposition of NT),-: Time, f (min) [N2Os] (mol L-1) 0 0.200 5 0.171 10 0.146 15 0.125 20 0.106 25 0.0909 30 0.0777 35 0.0664 40 0.0570 Use appropriate graphs to determine the rate constant for this reaction. Find the half-life of the reaction.
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?
The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
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.
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?
Label the elementary processes for the reaction between H2 and O2 see section 20.7 as initiation, propagation, branching, or termination reactions.
What is the difference between average rate, initial rate, and instantaneous rate?
Two mechanisms are proposed for the reaction 2NO(g)+O2(g)2NO2(g)Mechanism 1: NO+O2NO3(fast) NO3+NO2NO2(slow) Mechanism 2: NO+ON2O2(fast) N2O2+O22NO2(slow) Show that each of these mechanisms is consistent with the observed rate law: rate=k[ NO2 ]2[ O2 ].
Experiments have shown that the average frequency of chirping by a snowy tree cricket (Oecanthus fultoni) depends on temperature as shown in the table. Chirping Rate (per min) Temperature (C) 178 25.0 126 20.3 100. 17.3 What is the apparent activation energy of the process that controls the chirping? What is the rate of chirping expected at a temperature of 7.5C?
In a first-order reaction, suppose that a quantity X of a reactant is added at regular intervals of time, t. At first the amount of reactant in the system builds up; eventually, however, it levels off at a saturation value given by the expression a saturation value saturationvalue= x110a where a=0.30tt1/2 This analysis applies to prescription drugs, of which you take a certain amount each day. Suppose that you take 0.100 g of a drug three times a day and that the half-life for elimination is 2.0 days. Using this equation, calculate the mass of the drug in the body at saturation. Suppose further that side effects show up when 0.500 g of the drug accumulates in the body. As a pharmacist, what is the maximum dosage you could assign to a patient for an 8-h period without causing side effects?