IB CHEMISTRY Unit 6: KINETICS STANDARD LEVEL: Number Objective Rates of Reaction Define the term rate of reaction. Describe suitable experimental procedures for measuring rates of reactions. Analyze data from rate experiments. Students should be familiar with graphs of changes in concentration‚ volume and mass against time. Collision Theory Describe the kinetic theory in terms of the movement of particles whose average energy is proportional to the temperature in Kelvins. Define the term activation
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Learning Goals: • Predict the kinetic and potential energy of objects. • Examine how kinetic and potential energy interact with each other. In the space provided‚ define the following words: Kinetic energy-is the energy of motion. An object that has motion - whether it is vertical or horizontal motion Potential energy-is the energy of an object or a system due to the position of the body or the arrangement of the particles of the system Open Internet Explorer. From the FMS
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¬¬¬¬¬¬04/28/2010 Monday & Wednesday 7:40-10:30 Experiment #2 – Kinetics of the Decomposition of Hydrogen Peroxide Introduction: Chemical reactions are dependent upon two factors: temperature and concentrations of substance. We can monitor the rate at which a chemical decomposes or the rate at which a chemical substance appears. In this experiment we will be measuring the rate of decomposition of hydrogen dioxide with the following reaction: 2 H202 (aq) 4 2 H20 (l) + 02 (g) We can trap the
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GROUP 2 Kinetics of De-esterification for Synthesis of Benzoic Acid BATCH REACTOR Shane Bulk Chris Crosley David McGuire Max Skula Yunjing Song Shriram Sundarraj Nelson Zhou 155:416 Process Laboratory II Professor Jerry Sheinbeim January 28 – February 28‚ 2014 ABSTRACT The observed reaction that took place in this experiment was the de-esterification of ethyl benzoate to form benzoic acid. This experiment was used to determine the rate constant k of the synthesis of benzoic
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Introduction The reaction rate of a chemical reaction is determined as the change in the concentration of a reactant or product over the change in time. [1] The rate of a reaction is determined by experiment. Many factors influence the rate of a reaction: the nature of the reaction‚ concentration‚ pressure‚ temperature‚ and surface area‚ presence of catalyst and intensity of light. [2] For a chemical reaction‚ the rate law or rate equation is a mathematical expressed equation that links the reaction
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Kinetic Theory Objectives • Describe how the kinetic-molecular theory is used to explain how gases behave at different temperatures. (Exploration 1) • Analyze data that shows how gas particle mass affects that gas’s behavior. (Exploration 2) • Describe the Maxwell-Boltzmann Distribution. (Explorations 1 and 2) Description of Activity The kinetic-molecular theory states that a collection of gas molecules’ average kinetic energy has a specific value at any given temperature
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Kinetic Molecular Theory Basic Concepts The gas laws developed by Boyle‚ Charles‚ and Gay-Lussac are based upon empirical observations and describe the behavior of a gas in macroscopic terms‚ that is‚ in terms of properties that a person can directly observe and experience. An alternative approach to understanding the behavior of a gas is to begin with the atomic theory‚ which states that all substances are composed of a large number of very small particles (molecules or atoms). In principle‚ the
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uniform disk of radius R = 0.25 m has a string wrapped around it‚ and a m = 3 kg weight is hanging on the string. The system of the weight and disk is released from rest. a) When the 3 kg weight is moving with a speed of 2.2 m/s‚ what is the kinetic energy of the entire system? KETOT = KEwheel+KEweight = (1/2)(I)(w2)+(1/2)(m*v2) =(0.5* v2)(m+1/2M) =0.5*(2.2^2)*(3+(.5*15)) J b) If the system started from rest‚ how far has the weight fallen?
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Chemistry 12: Reaction Kinetics Review 1. Looking at the expressions for reaction rate‚ write expressions with which you could express rates for the following reactions. (Hint: look at what happens to reactants and products.) Recall that solid or liquids can lose or gain mass‚ gases can lose or gain volume and aqueous solutions can increase or decrease in concentration. ("a" is done as an example.) a) Mg(s) + 2HCl(aq) H2(g) + MgCl2(aq) reaction rate = mass of Mg consumed unit time b) c) or
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HOW FAST ARE CHEMICAL REACTIONS? THEORY The study of reaction rates‚ how fast or how slow a reaction takes place‚ is known as chemical kinetics. The rate of chemical reactions varies greatly. Some reactions‚ such as the explosion of an atom bomb are uncontrollable. Reactions like the decay of radioactive carbon (14C) are so slow that it takes centuries to see any noticeable change. Between the two extremes are reactions that can be measured in the laboratory. There are several factors that
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