'Initial rate' diaporamas de présentation

KINETICS: RATES AND MECHANISMS OF CHEMICAL REACTIONS

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Chemical Kinetics

Chemical Kinetics. Expression of rates. Stoichiometric relationships of rates of different substances in a reaction. Determination of reaction orders, rate laws, and rate constant by method of initial rate. Determination of rate laws by graphical or integration method.

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Chapter 16

Chapter 16. Kinetics: Rates and Mechanisms of Chemical Reactions. Kinetics: Rates and Mechanisms of Chemical Reactions. 16.1 Factors That Influence Reaction Rates. 16.2 Expressing the Reaction Rate. 16.3 The Rate Law and Its Components.

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Chapter 16

Chapter 16. Kinetics: Rates and Mechanisms of Chemical Reactions. Kinetics: Rates and Mechanisms of Chemical Reactions. 16.1 Factors That Influence Reaction Rates. 16.2 Expressing the Reaction Rate. 16.3 The Rate Law and Its Components.

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Chapter 14

Chapter 14. Kinetics: Rates and Mechanisms of Chemical Reactions. Figure 16.1. Reaction rate: the central focus of chemical kinetics. The wide range of reaction rates. Figure 16.2. Factors That Influence Reaction Rate. Under a specific set of conditions, every reaction has its own

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Chapter 16

Chapter 16. Rate of reactions / Kinetics: Rates and Mechanisms of Chemical Reactions. Lecture 1. Lecture 2. Lecture 3. Lecture 4. Highlights: Rates and Mechanisms of Chemical Reactions. Expression of the Reaction Rate: average, instantaneous and initial reactions rates.

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Chpt 12 - Chemical Kinetics

Chpt 12 - Chemical Kinetics. Reaction Rates Rate Laws Reaction Mechanisms Collision Theory Catalysis HW set1: Chpt 12 - pg. 580-592, # 22, 23, 28 Due Dec. 13 HW set2: Chpt 12 # 39, 48, 53, 56, 58, 60 due Dec. 17 HW set3: Chpt 12 #62, 69, 72 due Dec. 19. Reaction Rate ? .

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Rate Laws

Rate Laws. Example: Determine the rate law for the following reaction given the data below. H 2 O 2 (aq) + 3 I - (aq) + 2H + (aq) I 3 - (aq) + H 2 O (l). [H 2 O 2 ] [I - ] [H + ] Initial Expt # (M) (M) (M) Rate (M /s) 1 0.010 0.010 0.00050 1.15 x 10 -6

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Rate Laws

Rate Laws. Example: Determine the rate law for the following reaction given the data below. H 2 O 2 (aq) + 3 I - (aq) + 2H + (aq) ? I 3 - (aq) + H 2 O (l). [H 2 O 2 ] [I - ] [H + ] Initial Expt # (M) (M) (M) Rate (M /s) 1 0.010 0.010 0.00050 1.15 x 10 -6

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Chapter 14

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Topic 16 Kinetics

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Chapter 17

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Sample Exercise 6.1 Calculating an Average Rate of Reaction

Solution. Analyze: We are given the concentration of A at 20 s (0.54 M) and at 40 s (0.30 M) and asked to calculate the average rate of reaction over this time interval.

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Drug discovery targeting Malaria

Drug discovery targeting Malaria. Target Identification and Validation Imperial College/ Sanger Centre. Crystallography Oxford University. Protein production and assay development Imperial academic and DDC. DDC Expertise (Project management). Screening Campaign

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Factors affecting enzyme concentration

Factors affecting enzyme concentration. Enzymes: true or false?. Spec Check explain the importance of cofactors and coenzymes in enzyme-controlled reactions; . What are cofactors?.

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Inductor

Inductor. Inductor. Inductor is a passive electric device that store energy in its Magnetic field when a current flows through it A coil of wire wound on a Ferromagnetic core Air core Inductor, iron core inductor Circuit representation is. L. i. v L. +. Inductive Circuit.

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EXERCISE Determining a Rate Law from Initial Rate Data

The initial rate of a reaction was measured for several different starting concentrations of A and B, and the results are as follows:. Answer. (a) the rate law for the reaction. Reaction is zero-order w.r.to B. Reaction is second-order w.r.to B.

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Chapter 18 Notes, part IV

Chapter 18 Notes, part IV. Rate Law Problems. Rate Laws. Earlier we discussed that the rate at which a reaction goes is dependent on the concentration of the reactants. Rate Laws. If the reaction is A a B, then the rate of reaction is dependent on the concentration of A. So: Rate=k[A] a.

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4.1 Ratios and Proportions

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