factors that affect reaction rates is essential in planning a synthesis The light sticks, digital voltmeters and LDRs used in this experiment pose no hazard A glowstick consists of an inner, thin walled glass vial and an outer plastic tube The
Previous PDF | Next PDF |
[PDF] Chemoluminescence
Factors Applications: luminol, glow sticks Bioluminescence References The first written acknowledgement of chemiluminescent reactions was made by Aristotle who noted weak Factors affecting chemiluminescence emission
[PDF] Measure how the light output from a commercial light stick at room
factors that affect reaction rates is essential in planning a synthesis The light sticks, digital voltmeters and LDRs used in this experiment pose no hazard A glowstick consists of an inner, thin walled glass vial and an outer plastic tube The
[PDF] Kinetics – observing the effect of temperature on the rate of - Dr Hal
The brightness of the glowstick should increase as it gets hotter since the molecules are colliding more frequently Discussion: The brightness of the glowsticks is directly proportional to the temperature; reactions get faster as they get hotter and slower as they get colder
[PDF] Temperature and Glow Sticks - Cool Cosmos
The hot water has faster moving particles than the cold and room temperature water These fast-‐ moving particles collide with the glow stick, transferring energy This causes the liquid particles in the glow stick to move quicker, increasing the rate of the chemical reaction
[PDF] TOPIC 3: CHEMICAL KINETICS - Manitoba Education
Brown, W P “Factors Affecting the Speed-Rates of Chemical Reactions ” Doc Brown's Glow Sticks shows how temperature affects reaction rate One Glow
[PDF] Investigating reaction rates - The University of Western Australia
To Explore factors that affect the rate of a chemical reaction, through Light sticks that use chemiluminescent reactions to glow in the dark are affected by
[PDF] MITOCW ocw-5-111-f08-lec34_300k - MIT OpenCourseWare
with are factors affecting the rates of reaction People said any of you used glow sticks before, maybe trick or treating or some other point So basically,
[PDF] E:\Science 10\Chemistry\6 Reactions\62 PS - Surrey Schools
Factors Affecting Reaction Rates 6 2 PS Reaction Rates wpd Page 1 1 dissolving an alka seltzer tablet (a) advantage (b) disadvantage d glow stick (a)
[PDF] Rate-of-Reaction-Foundation - New Document 1
The results are shown in the table Temperature in °C Effect on glow stick Brightness of light Time it gave out light, in hours 5
[PDF] facts about paris for kids
[PDF] faculté médecine paris 7
[PDF] faire des ricochets dans l'eau
[PDF] faire des ricochets les enfoirés
[PDF] faire imprimer son rapport de stage
[PDF] faire la synthese d'une reunion
[PDF] faire une cour carrossable en gravier
[PDF] faire une cour en gravier
[PDF] faire une cour en gravier stabilisé
[PDF] fancy restaurants in paris france
[PDF] fanuc handling tool operation and programming manual pdf
[PDF] fanuc programming manual pdf
[PDF] fanuc r 30ib controller maintenance manual
1
Oxford University Chemistry Practical Course
1 st year physical chemistryX.3 Kinetics
Introduction
Kinetics, the study of the rates of chemical reactions, is one of the most important areas of chemistry. On paper, a reaction may look feasible, but if the rate at which it can be made to proceed is negligible, there will be no point in trying it, so an understanding of the factors that affect reaction rates is essential in planning a synthesis. In addition, if experiments can show how the rate of reaction varies with the concentration of reactants, this can provide an insight into the mechanism of the reaction. There are several ways to change the rate of a reaction, including adjusting the temperature, changing the reactant concentration, or adding a catalyst. An understanding of these factors will help you to select suitable conditions when trying a reaction for the first time.Objectives
This experiment covers some key ideas in kinetics. Light sticks will be used to investigate the intriguing production of "cold light". You will combine your data with those of other students to determine the activation energy for the reaction.The objectives of the experiment are to:
Measure how the light output from a commercial light stick at room temperature varies with time, using a light-sensitive resistor and a digital voltmeter. Make a suitable plot to determine whether the reaction responsible for the light emission follows 1 st order or 2 nd order kinetics and find the appropriate rate constant. Repeat the experiment at two further temperatures and find the value of the rate constants at those temperatures Repeat one of the measurements using a light stick of a different colour to check whether the presence of a dye alters the kinetics. Combine your results with those of other students and prepare a plot from which the activation energy for the reaction can be found.Safety
The light sticks, digital voltmeters and LDRs used in this experiment pose no hazard. However, if you have any concerns about safety, consult a demonstrator. 2Relevant topics
The following topics in the 1
st year kinetics course are relevant to this experiment: Rate equation, order of reaction, activation energy and its determination, integrated rate law.Theory
The rate of a reaction can be expressed in a rate law, which shows how the rate at which products are formed (or the rate at which reactants are consumed) depends upon the concentration of the reactants. For example, the rate law for the reaction2NO + 2H
2 N 2 + 2H 2 O has been found experimentally to be: 222 [][][]dHOkNO Hdt (1) In this equation the power to which the concentration of a reactant is raised is the order of reaction with respect to that reactant; thus we say that the reaction is "1 st order in hydrogen" and "2 nd order in nitric oxide". The overall order of the reaction is the sum of these coefficients, so this is a 3 rd order reaction. The orders need not, and often do not, equal the stoichiometric coefficients in the overall equation, so the rate equation cannot be determined directly from the stoichiometric equation. k is the rate constant for the reaction.