Nitrosyl chloride is produced from the reaction of nitrogen(II)oxide and chlorine. 2 NO(g) + Cl2(g) ---> 2 NOCI(g) The following initial rates at a given temperature were obtained for the concentrations given below: Experiment 1 2 3 What is the Rate Law? Rate (mol/L.hr) 2.21 8.83 17.5 NO (mol/L) 0.25 0.50 0.50 Cl₂_(mol/L) 0.25 0.25 0.50

Nitrosyl chloride is produced from the reaction of nitrogen(II)oxide and chlorine. 2 NO(g) + Cl2(g) ---> 2 NOCI(g) The following initial rates at a given temperature were obtained for the concentrations given below: Experiment 1 2 3 What is the Rate Law? Rate (mol/L.hr) 2.21 8.83 17.5 NO (mol/L) 0.25 0.50 0.50 Cl₂_(mol/L) 0.25 0.25 0.50

Chemistry

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Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 31E: The decomposition of nitrosyl chloride was studied: 2NOCl(g) 2NO(g) + Cl2(g) The following data...

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A study of the rate of dimerization of C4H6 gave the data shown in the table: 2C4H6C8H12 (a) Determine the average rate of dimerization between 0 s and 1600 s, and between 1600 s and 3200 s. (b) Estimate the instantaneous rate of dimerization at 3200 s from a graph of time versus [C4H6]. What are the units of this rate? (c) Determine the average rate of formation of C8H12 at 1600 s and the instantaneous rate of formation at 3200 s from the rates found in parts (a) and (b).
Nitryl fluoride is an explosive compound that can be made by oxidizing nitrogen dioxide with fluorine: 2 NO2(g) + F2(g) → 2 NO2F(g) Several kinetics experiments, all done at the same temperature and involving formation of nitryl fluoride, are summarized in this table: Write the rate law for the reaction. Determine what the order of the reaction is with respect to each reactant and each product. Calculate the rate constant k and express it in appropriate units.
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Nitrogen monoxide reacts with oxygen to give nitrogen dioxide. 2NO(g)+O2(g)2NO2(g) The rate law is [NO]/t = k[NO]2[O2], where the rate constant is 1.16 103 L2/(mol2 s) at 339oC. A vessel contains NO and O2 at 339oC. The initial partial pressures of NO and O2 arc 155 mmHg and 345 mmHg, respectively. What is the rate of decrease of partial pressure of NO (in mmHg per second)? (Hint: From the ideal gas law, obtain an expression for the molar concentration of a particular gas in terms of its partial pressure.)
For each of the rate laws below, what is the order of the reaction with respect to the hypothetical substances X, Y, and Z? What is the overall order? (a) Rate = k [X][Y][Zl, (b) Rate = k [X]-[Y]1/2[Z], (c) Rate = k [X]L5[Y]-1, (d) Rate = k [X]/[Y]2
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
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?
Nitrogen monoxide reacts with hydrogen as follows: 2NO(g)+H2(g)N2O(g)+H2O(g) The rate law is [H2]/t = k[NO]2[H2], where k is 1.10 107 L2/(mol2 s) at 826C. A vessel contains NO and H2 at 826C. The partial pressures of NO and H2 are 144 mmHg and 315 mmHg, respectively. What is the rate of decrease of partial pressure of NO? See Problem 13.151.
A The compound 1,3-butadiene (C4H6) forms 1,5-cyclooctadiene, C8H12 at higher temperatures. C4H6(g) C8H12(g) Use the following data to determine the order of the reaction and the rate constant, k. (Note that the total pressure is the pressure of the unreacted C4H6 at any time plus the pressure of the C8H12.)
Chlorine dioxide, ClO2, is a reddish-yellow gas that is soluble in water. In basic solution it gives ClO3 and ClO2 ions. 2ClO2(aq)+2OH(aq)ClO3(aq)+ClO2(aq)+H2O To obtain the rate law for this reaction, the following experiments were run and, for each, the initial rate of reaction of ClO2 was determined. Obtain the rate law 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 decomposition of nitrosyl chloride was studied: 2NOCl(g) 2NO(g) + Cl2(g) The following data were obtained where Rate=[NOCl]t [NOCl]0(molecules/cm3) Initial Rate (molecules/cm3 s) 3.0 1016 5.98 104 2.0 1016 2.66 104 1.0 1016 6.64 103 4.0 1016 1.06 105 a. What is the rate law? b. Calculate the value of the rate constant. c. Calculate the value of the rate constant when concentrations are given in moles per liter.

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