![For the reaction (aA produts) at order n= 1,5 with regards to A, integrate the rate law obtain the relationship of [A] functi](http://img.homeworklib.com/questions/55fd72f0-3690-11eb-a682-13735d895dfb.png?x-oss-process=image/resize,w_560)
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![a A - products order = 1.5 according to the rate law, - d[A] K [A] dt 1.5 -d [A] Caglos k dt nt X (Sunda nt t d[A [A]S =kldt](http://img.homeworklib.com/questions/56c9bae0-3690-11eb-8dcd-7138fd3ead56.png?x-oss-process=image/resize,w_560)
![t112 for half life til (A) = [Ao i expression for the will be -1/2 ktort [ Ao 112 WE [Ao] -112 = Ktiz f (Ao 2. 2[20]²(3-1) K](http://img.homeworklib.com/questions/5852fa00-3690-11eb-9d5c-9f8363b93d44.png?x-oss-process=image/resize,w_560)
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For the reaction (aA produts) at order n= 1,5 with regards to A, integrate the rate...
Suppose that the rate law for an irreversible reaction is Derive the integrated rate expression for...
Suppose that the rate law for an irreversible reaction is
Derive the integrated rate expression for CA as a
function of time. What would you plot along the y-axis vs. time in
order to obtain a linear relationship?
The reaction, aA products, is a first order reaction with a rate constant of 1.248...
The reaction, aA products, is a first order reaction with a rate constant of 1.248 x 10-4 s-1 . a. How long (in seconds) does it take for the initial amount of A to decrease by 30%? b. What fraction of reactant remains after 30 minutes? c. What is the half-life for the reaction? d. How long does it take for the initial amount of reactant to decrease by 87.5%?
4. The reaction A - B is n-th order (where n +0,1; in other words n...
4. The reaction A - B is n-th order (where n +0,1; in other words n = 1/2, 3/2, 2, 3, ...) and goes to completion. Derive the expression for the half-life of the reaction as a function of k, n and the initial concentration [A]
Worksheet: Kinetics and Rate Order 1. The rate of the reaction NO, + CO → NO...
Worksheet: Kinetics and Rate Order 1. The rate of the reaction NO, + CO → NO + CO2 depends only on the concentration of nitrogen dioxide below 225 °C. At a temperature below 225 °C, the following data were collected Time (s) 0 1200 3000 4500 9000 18000 [NO2] (M) 0.500 0.444 0.381 0.340 0.250 0.174 a. Determine the order of the reaction by using the integrated rate law. b. What is the rate constant for this reaction? c. Determine...
A certain reaction has the following general form: aA rightarrow bB. temperature and [A]_o = 2.00...
A certain reaction has the following general form: aA rightarrow bB. temperature and [A]_o = 2.00 times10^-2 M, concentration versus time data were collected for this reaction, and a plot of ln [A] versus time resulted in a straight line with a slope value of -2.97 times 10^-2 min^-1 Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction. Calculate the half-life for this reaction. How much time is required for the...
1. Derive the second order rate law for the reaction 2 A →P, and an expression...
1. Derive the second order rate law for the reaction 2 A →P, and an expression for its half life, t 1/2, in terms of the initial concentration of A. State your assumptions and show each step. [See Atkins 10th ed, 20B2; Atkins 11th ed, 17B2]
4) Consider the schematic reaction A →P a) If the reaction is one-half order with respect...
4) Consider the schematic reaction A →P a) If the reaction is one-half order with respect to [A], what is the integrated rate law expression for this reaction? b) What plot would you construct to determine the rate constant k for the reaction? c) What would be the half-life for this reaction? Will it depend on initial concentration of the reactant'?
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is...
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is reported in units of sl. What is the overall order of the reaction? 2) The rate law for a reaction was reported as rate=k[A] [B][C] with molar concentrations in moles per cubic decimetre and time in seconds. What are the units of k? 3) The rate constant for the pseudo first-order acid- catalysed hydrolysis of glucose is 4.07' 10-s. Calculate the half-life for the...
ChemActivity T10 Gibbs Energy as a Function of Temperature and Pressure 121 Model 2: Chemical Potential....
ChemActivity T10 Gibbs Energy as a Function of Temperature and Pressure 121 Model 2: Chemical Potential. For a pure phase, the chemical potential is given by where G is the molar Gibbs energy and n is the number of moles. Critical Thinking Questions 5. For a constant temperature process, what is the relationship between do, volume, and pressure? 6. A particularly useful relationship is that between G and volume and pressure for various systems at constant temperature. a) For condensed...
1. A reaction is second order in[A] and second-order in [B]: Rate,=K[A]^2[B]^2. what are the units...
1. A reaction is second order in[A] and second-order in [B]: Rate,=K[A]^2[B]^2. what are the units of k for this reaction? If the concentration of air decreases by a factor of 2 and the concentration of b increases by a factor of 5 what happens to the rate? 2. for the forward reaction 2NO+Cl2=>2NOCl. determine the rate(m/s)for experiment #4 given [NO]°(M)=0.40M and [Cl2]°z(M)=0?20M. Rate? 3.The following data were collected over time for the forward reaction 2NO2=>2NO+O2 ( 1/[NO2]=100 at 0...
Suppose that the rate law for an irreversible reaction is
Derive the integrated rate expression for CA as a
function of time. What would you plot along the y-axis vs. time in
order to obtain a linear relationship?
4. The reaction A - B is n-th order (where n +0,1; in other words n = 1/2, 3/2, 2, 3, ...) and goes to completion. Derive the expression for the half-life of the reaction as a function of k, n and the initial concentration [A]
Worksheet: Kinetics and Rate Order 1. The rate of the reaction NO, + CO → NO + CO2 depends only on the concentration of nitrogen dioxide below 225 °C. At a temperature below 225 °C, the following data were collected Time (s) 0 1200 3000 4500 9000 18000 [NO2] (M) 0.500 0.444 0.381 0.340 0.250 0.174 a. Determine the order of the reaction by using the integrated rate law. b. What is the rate constant for this reaction? c. Determine...
A certain reaction has the following general form: aA rightarrow bB. temperature and [A]_o = 2.00 times10^-2 M, concentration versus time data were collected for this reaction, and a plot of ln [A] versus time resulted in a straight line with a slope value of -2.97 times 10^-2 min^-1 Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction. Calculate the half-life for this reaction. How much time is required for the...
1. Derive the second order rate law for the reaction 2 A →P, and an expression for its half life, t 1/2, in terms of the initial concentration of A. State your assumptions and show each step. [See Atkins 10th ed, 20B2; Atkins 11th ed, 17B2]
4) Consider the schematic reaction A →P a) If the reaction is one-half order with respect to [A], what is the integrated rate law expression for this reaction? b) What plot would you construct to determine the rate constant k for the reaction? c) What would be the half-life for this reaction? Will it depend on initial concentration of the reactant'?
1) The rate constant for the reaction 2 N,Os(9) = 4 NO (9) + O2(9) is reported in units of sl. What is the overall order of the reaction? 2) The rate law for a reaction was reported as rate=k[A] [B][C] with molar concentrations in moles per cubic decimetre and time in seconds. What are the units of k? 3) The rate constant for the pseudo first-order acid- catalysed hydrolysis of glucose is 4.07' 10-s. Calculate the half-life for the...
ChemActivity T10 Gibbs Energy as a Function of Temperature and Pressure 121 Model 2: Chemical Potential. For a pure phase, the chemical potential is given by where G is the molar Gibbs energy and n is the number of moles. Critical Thinking Questions 5. For a constant temperature process, what is the relationship between do, volume, and pressure? 6. A particularly useful relationship is that between G and volume and pressure for various systems at constant temperature. a) For condensed...
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