Kinetics pt2

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Nov 24, 2024

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Chm152 Spring 2023 1 T-ORDER REACTIONS: INTEGRATED RATE LAW First-order reactions are reactions in which the rate of the reaction depends directly on the concentration of one reactant. ND-ORDER REACTIONS: INTEGRATED RATE LAW Second-order reactions come in two types one in which the reaction rate depends on the concentration of a single reactant raised to the second power another in which the reaction rate depends on the concentrations of two reactants
Chm152 Spring 2023 2 ND-ORDER REACTIONS: INTEGRATED RATE LAW
Chm152 Spring 2023 3 t (s) [A] (M) 0 0.750 5.00 0.728 10.0 0.708 20.0 0.670 30.0 0.636 40.0 0.605 50.0 0.577 Data for the second-order reaction A→ products were collected and are listed in the table that follows: 1.Determine the value of the rate constant.
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Chm152 Spring 2023 4 t (s) [A] (M) 0 0.750 5.00 0.728 10.0 0.708 20.0 0.670 30.0 0.636 40.0 0.605 50.0 0.577 Data for the second-order reaction A→ products were collected and are listed in the table that follows: 1.Determine the value of the rate constant.
Chm152 Spring 2023 5 t (s) [A] (M) 0 0.750 5.00 0.728 10.0 0.708 20.0 0.670 30.0 0.636 40.0 0.605 50.0 0.577 Data for the second-order reaction A→ products were collected and are listed in the table that follows: 1.Determine the value of the rate constant. 1/0.728 M= k · 5s + 1/0.750 M k = 0.00800 M -1 s -1
Chm152 Spring 2023 6 t (s) [A] (M) 0 0.750 5.00 0.728 10.0 0.708 20.0 0.670 30.0 0.636 40.0 0.605 50.0 0.577 Data for the second-order reaction A→ products were collected and are listed in the table that follows: 2. Determine the concentration of the reactant at 90 s after the reaction has begun.
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Chm152 Spring 2023 7 t (s) [A] (M) 0 0.750 5.00 0.728 10.0 0.708 20.0 0.670 30.0 0.636 40.0 0.605 50.0 0.577 Data for the second-order reaction A→ products were collected and are listed in the table that follows: 2. Determine the concentration of the reactant at 90 s after the reaction has begun.
Chm152 Spring 2023 8 t (s) [A] (M) 0 0.750 5.00 0.728 10.0 0.708 20.0 0.670 30.0 0.636 40.0 0.605 50.0 0.577 Data for the second-order reaction A→ products were collected and are listed in the table that follows: 2. Determine the concentration of the reactant at 90 s after the reaction has begun. k = 0.00800 M -1 s -1
Chm152 Spring 2023 9 t (s) [A] (M) 0 0.750 5.00 0.728 10.0 0.708 20.0 0.670 30.0 0.636 40.0 0.605 50.0 0.577 Data for the second-order reaction A→ products were collected and are listed in the table that follows: 2. Determine the concentration of the reactant at 90 s after the reaction has begun. k = 0.00800 M -1 s -1
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Chm152 Spring 2023 10
Chm152 Spring 2023 11
Chm152 Spring 2023 12
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Chm152 Spring 2023 13 SECOND-ORDER REACTIONS: HALF-LIFE
Chm152 Spring 2023 14 The compound AB decomposes via a second-order process with a rate constant equal to 5.13×10−4 M −1 s −1 at 35°C. 1.Calculate the half-life of the reaction with an initial concentration of [AB]=0.230M . 2.This same reaction has a half-life of 45.0 minutes when carried out at 55°C with an initial concentration of 0.230 M. What is the rate constant at 55°C? 3.Compare the rate constants at the two temperatures.
Chm152 Spring 2023 15 The compound AB decomposes via a second-order process with a rate constant equal to 5.13×10−4 M −1 s −1 at 35°C. 1.Calculate the half-life of the reaction with an initial concentration of [AB]=0.230M . 2.This same reaction has a half-life of 45.0 minutes when carried out at 55°C with an initial concentration of 0.230 M. What is the rate constant at 55°C? 3.Compare the rate constants at the two temperatures.
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Chm152 Spring 2023 16 The compound AB decomposes via a second-order process with a rate constant equal to 5.13×10−4 M −1 s −1 at 35°C. 1.Calculate the half-life of the reaction with an initial concentration of [AB]=0.230M . 2.This same reaction has a half-life of 45.0 minutes when carried out at 55°C with an initial concentration of 0.230 M. What is the rate constant at 55°C? 3.Compare the rate constants at the two temperatures.
Chm152 Spring 2023 17 The compound AB decomposes via a second-order process with a rate constant equal to 5.13×10−4 M −1 s −1 at 35°C. 1.Calculate the half-life of the reaction with an initial concentration of [AB]=0.230M . 2.This same reaction has a half-life of 45.0 minutes when carried out at 55°C with an initial concentration of 0.230 M. What is the rate constant at 55°C? 3.Compare the rate constants at the two temperatures.
Chm152 Spring 2023 18 The compound AB decomposes via a second-order process with a rate constant equal to 5.13×10−4 M −1 s −1 at 35°C. 1.Calculate the half-life of the reaction with an initial concentration of [AB]=0.230M . t 1/2 = 8475 s = 8.48 x 10 3 s 2.This same reaction has a half-life of 45.0 minutes when carried out at 55°C with an initial concentration of 0.230 M. What is the rate constant at 55°C? 3.Compare the rate constants at the two temperatures.
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Chm152 Spring 2023 19 The compound AB decomposes via a second-order process with a rate constant equal to 5.13×10−4 M −1 s −1 at 35°C. 1.Calculate the half-life of the reaction with an initial concentration of [AB]=0.230M . t 1/2 = 8475 s = 8.48 x 10 3 s 2.This same reaction has a half-life of 45.0 minutes when carried out at 55°C with an initial concentration of 0.230 M. What is the rate constant at 55°C? k = 0.0966 M -1 min -1 s 3.Compare the rate constants at the two
Chm152 Spring 2023 20 The compound AB decomposes via a second-order process with a rate constant equal to 5.13×10−4 M −1 s −1 at 35°C. 1.Calculate the half-life of the reaction with an initial concentration of [AB]=0.230M . t 1/2 = 8475 s = 8.48 x 10 3 s 2.This same reaction has a half-life of 45.0 minutes when carried out at 55°C with an initial concentration of 0.230 M. What is the rate constant at 55°C? k = 0.0966 M -1 min -1 s 3.Compare the rate constants at the two
Chm152 Spring 2023 21 ERO-ORDER REACTIONS: INTEGRATED RATE LAW Rate = k �[A] 0 = k �
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Chm152 Spring 2023 22 The half-life of a zero-order reaction depends on both the rate constant and the initial concentration of the reactant, [A] 0 . But unlike the second- order half-life, the zero-order half-life is directly proportional to the initial reactant concentration.
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Chm152 Spring 2023 23
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Chm152 Spring 2023 24 ACTIVATION ENERGY
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Chm152 Spring 2023 25 For the reaction shown here, determine if the reaction is endothermic or exothermic the values of the activation energy and the enthalpy.
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Chm152 Spring 2023 26
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Chm152 Spring 2023 27 There are many factors that contribute to the size of the activation energy, including the nature of the reactants and the types of bonds being rearranged during the reaction.
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Chm152 Spring 2023 28 COLLISION THEORY: ARRHENIUS EQUATION k represents the rate constant A is known as the frequency factor Indicates the number of correctly oriented reactions per unit time. Ea �a is the activation energy R the gas law constant in the form 8.3145 J/mol·K, T is the absolute temperature (in kelvins)
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Chm152 Spring 2023 29 USING THE ARRHENIUS EQUATION
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Chm152 Spring 2023 30 Use the experimental rate constant data shown in the table to calculate the activation energy for the following reaction:
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Chm152 Spring 2023 31 Use the experimental rate constant data shown in the table to calculate the activation energy for the following reaction:
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Chm152 Spring 2023 32
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