- The document discusses methods for measuring the rate (speed) of a chemical reaction by monitoring changes in mass or volume of a reactant or product over time.
- Graphing these changes allows calculation of the reaction rate from the slope. Comparing rates with varying conditions like temperature indicates their effect.
- Specifically, the rate of a reaction between marble chips and hydrochloric acid producing carbon dioxide gas can be measured by the decreasing mass of the reaction vessel as gas is released.
Chemical kinetics is the study of the speed of chemical reactions and factors that affect the reaction rate. It provides information about reaction feasibility, timescales, and reaction mechanisms. The rate of a reaction can be examined by measuring changes in reactant or product concentrations over time. Reaction rates are determined experimentally and may follow zero-order, first-order, pseudo-first order, or second-order rate laws depending on the rate-determining step. Factors like temperature, concentration, physical state, and catalysts influence reaction rates.
1. Study of speed with which a chemical reaction occurs and the factors affecting that speed
2. Provides information about the feasibility of a chemical reaction
3. Provides information about the time it takes for a chemical reaction to occur
4. Provides information about the series of elementary steps which lead to the formation of product
The document discusses chemical kinetics and provides information about:
- The factors that affect the speed of a chemical reaction, including concentration, temperature, and catalysts.
- How to determine the rate law, rate constant, order, and mechanism of reactions from experimental data.
- The relationship between concentration and time for reactions of different orders (zero, first, and second order).
- How to calculate half-life, effect of temperature on reaction rate using the Arrhenius equation, and the role of homogeneous and heterogeneous catalysts.
Here are the effects on the rate of reaction of changing each condition:
- If the concentration of acid is increased, the rate of reaction will increase. This is because there will be more reactant particles per unit volume, resulting in more frequent collisions between reactants.
- If calcium carbonate powder is used instead of small pieces, the rate of reaction will increase. This is because powder has a larger surface area, allowing for more reactant particles at the interface where the reaction occurs.
- If the volume of acid is increased, the rate of reaction will initially increase but then level off. This is because there will be more reactant particles initially, but the reaction will use them up over time.
- If the
1) The document discusses kinetic chemistry, including reaction rates, rate constants, reaction orders, and factors that affect reaction rates such as concentration, temperature, surface area, and catalysts.
2) It provides examples of determining reaction orders based on changes in reaction rate with changes in concentration. Reaction orders can be fractional, zero, or higher than one.
3) The rate constant k depends on temperature according to the Arrhenius equation, and increases with higher temperature based on the activation energy of the reaction.
This document discusses kinetics and factors that affect reaction rates. It defines kinetics as how quickly reactions occur and the factors that influence reaction rates, such as temperature, concentration, and the presence of catalysts. Reaction rates are linked to reaction mechanisms - the step-by-step processes by which reactions take place. Increasing temperature leads to more collisions between reactant particles and faster reaction rates, as described by the Arrhenius equation. Catalysts lower the activation energy of reactions, speeding up reaction rates without being consumed.
For Session 2023-24, Artham provides notes for CLASS 12 Chemistry that are 100% updated to the latest curriculum. The notes cover key topics like Chemical Kinetics in concise yet easy to understand language with quick revision tips, mind maps, and to-the-point answers. Chemical Kinetics governs the rate of reactions and their mechanisms. The rate of a reaction is defined as the change in concentration of a reactant or product over time. Reaction rates depend on factors like temperature, concentration, and catalysts. Order of a reaction indicates how the rate depends on the concentrations of reactants.
This document provides an overview of chemical kinetics and reaction rates from the textbook "Chemistry: The Molecular Nature of Matter and Change". It discusses key topics such as:
- Factors that influence reaction rates like concentration, temperature, and surface area
- Expressing reaction rates in terms of changes in concentration over time
- Determining the rate law and reaction orders from experimental data
- Differentiating between zero, first, and second-order reactions based on their rate equations
- Calculating changes in reaction rates when concentrations are varied
The document uses diagrams, examples, and sample problems to illustrate concepts in chemical kinetics and determining reaction mechanisms and orders from rate data.
Chemical kinetics is the study of the speed of chemical reactions and factors that affect the reaction rate. It provides information about reaction feasibility, timescales, and reaction mechanisms. The rate of a reaction can be examined by measuring changes in reactant or product concentrations over time. Reaction rates are determined experimentally and may follow zero-order, first-order, pseudo-first order, or second-order rate laws depending on the rate-determining step. Factors like temperature, concentration, physical state, and catalysts influence reaction rates.
1. Study of speed with which a chemical reaction occurs and the factors affecting that speed
2. Provides information about the feasibility of a chemical reaction
3. Provides information about the time it takes for a chemical reaction to occur
4. Provides information about the series of elementary steps which lead to the formation of product
The document discusses chemical kinetics and provides information about:
- The factors that affect the speed of a chemical reaction, including concentration, temperature, and catalysts.
- How to determine the rate law, rate constant, order, and mechanism of reactions from experimental data.
- The relationship between concentration and time for reactions of different orders (zero, first, and second order).
- How to calculate half-life, effect of temperature on reaction rate using the Arrhenius equation, and the role of homogeneous and heterogeneous catalysts.
Here are the effects on the rate of reaction of changing each condition:
- If the concentration of acid is increased, the rate of reaction will increase. This is because there will be more reactant particles per unit volume, resulting in more frequent collisions between reactants.
- If calcium carbonate powder is used instead of small pieces, the rate of reaction will increase. This is because powder has a larger surface area, allowing for more reactant particles at the interface where the reaction occurs.
- If the volume of acid is increased, the rate of reaction will initially increase but then level off. This is because there will be more reactant particles initially, but the reaction will use them up over time.
- If the
1) The document discusses kinetic chemistry, including reaction rates, rate constants, reaction orders, and factors that affect reaction rates such as concentration, temperature, surface area, and catalysts.
2) It provides examples of determining reaction orders based on changes in reaction rate with changes in concentration. Reaction orders can be fractional, zero, or higher than one.
3) The rate constant k depends on temperature according to the Arrhenius equation, and increases with higher temperature based on the activation energy of the reaction.
This document discusses kinetics and factors that affect reaction rates. It defines kinetics as how quickly reactions occur and the factors that influence reaction rates, such as temperature, concentration, and the presence of catalysts. Reaction rates are linked to reaction mechanisms - the step-by-step processes by which reactions take place. Increasing temperature leads to more collisions between reactant particles and faster reaction rates, as described by the Arrhenius equation. Catalysts lower the activation energy of reactions, speeding up reaction rates without being consumed.
For Session 2023-24, Artham provides notes for CLASS 12 Chemistry that are 100% updated to the latest curriculum. The notes cover key topics like Chemical Kinetics in concise yet easy to understand language with quick revision tips, mind maps, and to-the-point answers. Chemical Kinetics governs the rate of reactions and their mechanisms. The rate of a reaction is defined as the change in concentration of a reactant or product over time. Reaction rates depend on factors like temperature, concentration, and catalysts. Order of a reaction indicates how the rate depends on the concentrations of reactants.
This document provides an overview of chemical kinetics and reaction rates from the textbook "Chemistry: The Molecular Nature of Matter and Change". It discusses key topics such as:
- Factors that influence reaction rates like concentration, temperature, and surface area
- Expressing reaction rates in terms of changes in concentration over time
- Determining the rate law and reaction orders from experimental data
- Differentiating between zero, first, and second-order reactions based on their rate equations
- Calculating changes in reaction rates when concentrations are varied
The document uses diagrams, examples, and sample problems to illustrate concepts in chemical kinetics and determining reaction mechanisms and orders from rate data.
kinetics of stability Molecular pharmaceuticsMittalGandhi
This document discusses kinetics of stability and reaction order. It defines key terms like rate, order of reaction, and molecularity. The main types of reaction order discussed are zero order, first order, pseudo first order, and second order. Graphs and equations to determine the rate constant and half-life are provided for each order. Methods for determining the experimental order of a reaction are outlined. Factors that can influence the reaction rate are also summarized. Tables listing the key equations for zero, first, and second order kinetics are included.
1. Laju reaksi adalah laju pengurangan konsentrasi pereaksi atau penambahan konsentrasi produk per satuan waktu. Laju reaksi dipengaruhi oleh konsentrasi, luas permukaan, suhu, tekanan, dan katalisator.
2. Untuk reaksi 2X → Y + Z, data menunjukkan reaksi berorde 0 karena konsentrasi X berkurang secara linier terhadap waktu. Konsentrasi X pada menit ke-30 adalah 2,
The document describes an experiment to determine the rate law of a chemical reaction between potassium permanganate (KMnO4) and oxalic acid. It involves measuring the rate of disappearance of the purple KMnO4 color as the concentration of reactants is varied. The method of initial rates is used to determine the rate law exponents and rate constant. The rate law is then determined at different temperatures to see how temperature affects the reaction rate. Safety precautions are outlined for the chemicals used.
The document discusses various topics related to chemical kinetics including:
- Definitions of rate of reaction, instantaneous rate, and average rate.
- Integrated rate equations for zero-order and first-order reactions and how to determine the half-life of a first-order reaction from its rate constant.
- The Arrhenius equation and how it relates the temperature dependence of reaction rates to activation energy. Increasing temperature increases the fraction of molecules with energy exceeding the activation energy.
- How catalysts increase reaction rates by providing an alternative reaction pathway requiring lower activation energy.
This document discusses reaction kinetics including:
1) Rate equations relate the rate of reaction to reactant concentrations and can be determined experimentally. The orders of reaction indicate how changing concentrations affect rate.
2) Reaction mechanisms involve multiple steps, with the rate determined by the slowest step. Molecularity refers to the number of species involved in a step.
3) Catalysts increase reaction rates by providing alternative reaction pathways. Heterogeneous catalysts involve different phases while homogeneous catalysts are the same phase as reactants. Common examples are discussed.
This document discusses chemical kinetics and rate of reactions. It defines chemical kinetics as the study of reaction rates and their mechanisms. It then discusses factors that influence reaction rates such as concentration, temperature, pressure, catalysts and more. It defines rate of reaction and discusses how to determine rates. It introduces reaction orders such as zero order, first order and second order reactions. Examples of each type of reaction order are provided along with the appropriate rate equations. Pseudo-first order reactions are also discussed.
The document summarizes an experiment investigating the effect of concentration and temperature on the rate of a Harcourt-Essen reaction. By varying the concentration of iodide ions between runs, the reaction was found to be second order overall and first order with respect to both peroxide ions and iodide ions. Increasing the temperature between runs caused the rate coefficient to increase, demonstrating that the reaction rate increases with temperature in accordance with the Arrhenius equation.
The document discusses reaction rates and kinetics. It defines the rate law and explains how the order of a reaction relates to how concentration affects reaction rate. Zero-order, first-order, and second-order reactions are described. Integrated rate laws show how concentration changes over time for different reaction orders. Reaction mechanisms, elementary steps, rate-determining steps, and reaction coordinates are also summarized.
This document discusses chemical kinetics, which is the study of reaction rates and how reaction rates change under varying conditions. Chemical kinetics is an empirical and experimental area of study that allows investigation of reaction mechanisms. Kinetic studies involve measuring reaction rates at different reactant concentrations and time intervals to determine the rate law equation and rate constant for a reaction. The rate law relates the reaction rate to the concentrations of reactants in the reaction and can provide information about the reaction mechanism and steps.
Chemical kinetics is the study of reaction rates and mechanisms. It involves determining:
- Reaction orders and rate laws from initial rates or graphical methods.
- Rate constants and activation energies.
- Elementary reaction steps and overall mechanisms.
The rate of a reaction depends on factors like temperature, concentration, and the presence of catalysts. Reaction rates are quantified by rate laws, which relate the rate to concentrations of reactants raised to their order of reaction. Graphical methods can be used to determine reaction orders from concentration-time data.
1. The velocity of a chemical reaction describes how quickly reactants are consumed and products are formed. It is expressed as the change in concentration of reactants or products with respect to time.
2. Factors that affect the rate of reaction include: the nature of reactants, temperature, concentration of reactants, and presence of catalysts. Specifically, increasing the temperature or concentration of reactants increases the reaction rate, while catalysts lower the activation energy and speed up the reaction.
3. For example, the rate of reaction can be expressed in terms of the rate of change of each reactant and product based on their stoichiometric coefficients. The example reaction rate is calculated based on the given rate of one reactant.
This document provides background information on reaction rates and mechanisms. It discusses how factors like reactant concentrations, temperature, catalysts, and surface area can influence reaction rates. It also defines concepts like the rate law, rate constant, reaction order, energy of activation, and Arrhenius equation. Methods for determining reaction order are described, including by varying reactant concentrations and analyzing integrated rate expressions for zero, first, and second order reactions. The effects of temperature on reaction rates are also addressed through the Arrhenius equation.
This unit includes: rate of a chemical reaction, graphs,, unit of rate, average rate& instantaneous rate,. factors influuncing rate of a reaction, Rate expression & rate constant, Order & molecularity of a reaction,, initiall rate method & integrated rate law equations, numerical problems,, Half life period, Pseudo first order reaction, Temperature of rate of reaction, Activation energy, collision frequency & effective collision, Collision theory, Arrhenius equation,, effect of catalyst on rate of reaction, numerical problems
The document discusses kinetics and the rate law for the decolorization of crystal violet. It describes using a spectroscopic colorimeter to monitor the concentration of crystal violet over time as it reacts with sodium hydroxide. The goals are to determine the overall rate law and rate constant k for the decolorization reaction. Experiments are conducted at different concentrations and the orders are determined by analyzing linear regression graphs of integrated rate laws versus time and concentration. The 1st order graph provided the best correlation, indicating the reaction is first order with respect to crystal violet concentration.
Chemical kinetics deals with the rates of chemical reactions and the factors that affect reaction rates. The rate of a reaction depends on variables like concentration, temperature, and presence of a catalyst. A reaction's rate law expresses how its rate depends on the concentrations of reactants. Integrated rate laws relate concentration over time for different reaction orders. Pseudo-first-order reactions occur when one reactant is in excess. The Arrhenius equation describes how temperature affects a reaction's rate constant.
The document discusses reaction rates and kinetics. It defines factors that affect reaction rates such as concentration of reactants, physical state, temperature, and catalysts. It also describes methods for determining reaction rates by measuring changes in concentration over time. Rate laws relate the rate of reaction to concentrations of reactants through rate constants and reaction orders. Integrated rate laws can be used to determine concentrations of reactants over time for reactions of different orders.
The document describes a laboratory experiment to determine the reaction order and rate constant of the reaction between sodium hydroxide (NaOH) and ethyl acetate (CH3COOC2H5). The group prepared 0.1 M solutions of each reactant and mixed them in a batch reactor at room temperature while measuring conductivity over time. Calculations using the conductivity readings showed the reaction was second order. The rate constant was determined to be 1.291651 × 10-3 at 21°C based on the nonlinear ln(CA/CAo) vs time graph.
This document discusses chemical kinetics and factors that affect reaction rates:
1) Reaction rates can be defined as the decrease in reactants or increase in products per unit time. Rates depend on concentrations and temperature.
2) Factors that increase reaction rates include higher concentrations, increased surface area, and higher temperatures. Higher temperatures provide more collisions with energy above the activation energy.
3) A catalyst provides an alternative reaction pathway with lower activation energy, increasing the number of effective collisions and thereby increasing the reaction rate.
This document discusses chemical kinetics and reaction rates. It begins with an introduction to chemical kinetics and defines reaction rate. It then discusses factors that affect reaction rates such as nature of reactants, concentration, temperature, and catalysts. It describes different types of reaction rates and how they are measured. The document also covers rate laws, determining rate orders experimentally, and integrated and differential rate equations for zero, first, and second order reactions. It concludes with an overview of rate theories including the Arrhenius equation.
kinetics of stability Molecular pharmaceuticsMittalGandhi
This document discusses kinetics of stability and reaction order. It defines key terms like rate, order of reaction, and molecularity. The main types of reaction order discussed are zero order, first order, pseudo first order, and second order. Graphs and equations to determine the rate constant and half-life are provided for each order. Methods for determining the experimental order of a reaction are outlined. Factors that can influence the reaction rate are also summarized. Tables listing the key equations for zero, first, and second order kinetics are included.
1. Laju reaksi adalah laju pengurangan konsentrasi pereaksi atau penambahan konsentrasi produk per satuan waktu. Laju reaksi dipengaruhi oleh konsentrasi, luas permukaan, suhu, tekanan, dan katalisator.
2. Untuk reaksi 2X → Y + Z, data menunjukkan reaksi berorde 0 karena konsentrasi X berkurang secara linier terhadap waktu. Konsentrasi X pada menit ke-30 adalah 2,
The document describes an experiment to determine the rate law of a chemical reaction between potassium permanganate (KMnO4) and oxalic acid. It involves measuring the rate of disappearance of the purple KMnO4 color as the concentration of reactants is varied. The method of initial rates is used to determine the rate law exponents and rate constant. The rate law is then determined at different temperatures to see how temperature affects the reaction rate. Safety precautions are outlined for the chemicals used.
The document discusses various topics related to chemical kinetics including:
- Definitions of rate of reaction, instantaneous rate, and average rate.
- Integrated rate equations for zero-order and first-order reactions and how to determine the half-life of a first-order reaction from its rate constant.
- The Arrhenius equation and how it relates the temperature dependence of reaction rates to activation energy. Increasing temperature increases the fraction of molecules with energy exceeding the activation energy.
- How catalysts increase reaction rates by providing an alternative reaction pathway requiring lower activation energy.
This document discusses reaction kinetics including:
1) Rate equations relate the rate of reaction to reactant concentrations and can be determined experimentally. The orders of reaction indicate how changing concentrations affect rate.
2) Reaction mechanisms involve multiple steps, with the rate determined by the slowest step. Molecularity refers to the number of species involved in a step.
3) Catalysts increase reaction rates by providing alternative reaction pathways. Heterogeneous catalysts involve different phases while homogeneous catalysts are the same phase as reactants. Common examples are discussed.
This document discusses chemical kinetics and rate of reactions. It defines chemical kinetics as the study of reaction rates and their mechanisms. It then discusses factors that influence reaction rates such as concentration, temperature, pressure, catalysts and more. It defines rate of reaction and discusses how to determine rates. It introduces reaction orders such as zero order, first order and second order reactions. Examples of each type of reaction order are provided along with the appropriate rate equations. Pseudo-first order reactions are also discussed.
The document summarizes an experiment investigating the effect of concentration and temperature on the rate of a Harcourt-Essen reaction. By varying the concentration of iodide ions between runs, the reaction was found to be second order overall and first order with respect to both peroxide ions and iodide ions. Increasing the temperature between runs caused the rate coefficient to increase, demonstrating that the reaction rate increases with temperature in accordance with the Arrhenius equation.
The document discusses reaction rates and kinetics. It defines the rate law and explains how the order of a reaction relates to how concentration affects reaction rate. Zero-order, first-order, and second-order reactions are described. Integrated rate laws show how concentration changes over time for different reaction orders. Reaction mechanisms, elementary steps, rate-determining steps, and reaction coordinates are also summarized.
This document discusses chemical kinetics, which is the study of reaction rates and how reaction rates change under varying conditions. Chemical kinetics is an empirical and experimental area of study that allows investigation of reaction mechanisms. Kinetic studies involve measuring reaction rates at different reactant concentrations and time intervals to determine the rate law equation and rate constant for a reaction. The rate law relates the reaction rate to the concentrations of reactants in the reaction and can provide information about the reaction mechanism and steps.
Chemical kinetics is the study of reaction rates and mechanisms. It involves determining:
- Reaction orders and rate laws from initial rates or graphical methods.
- Rate constants and activation energies.
- Elementary reaction steps and overall mechanisms.
The rate of a reaction depends on factors like temperature, concentration, and the presence of catalysts. Reaction rates are quantified by rate laws, which relate the rate to concentrations of reactants raised to their order of reaction. Graphical methods can be used to determine reaction orders from concentration-time data.
1. The velocity of a chemical reaction describes how quickly reactants are consumed and products are formed. It is expressed as the change in concentration of reactants or products with respect to time.
2. Factors that affect the rate of reaction include: the nature of reactants, temperature, concentration of reactants, and presence of catalysts. Specifically, increasing the temperature or concentration of reactants increases the reaction rate, while catalysts lower the activation energy and speed up the reaction.
3. For example, the rate of reaction can be expressed in terms of the rate of change of each reactant and product based on their stoichiometric coefficients. The example reaction rate is calculated based on the given rate of one reactant.
This document provides background information on reaction rates and mechanisms. It discusses how factors like reactant concentrations, temperature, catalysts, and surface area can influence reaction rates. It also defines concepts like the rate law, rate constant, reaction order, energy of activation, and Arrhenius equation. Methods for determining reaction order are described, including by varying reactant concentrations and analyzing integrated rate expressions for zero, first, and second order reactions. The effects of temperature on reaction rates are also addressed through the Arrhenius equation.
This unit includes: rate of a chemical reaction, graphs,, unit of rate, average rate& instantaneous rate,. factors influuncing rate of a reaction, Rate expression & rate constant, Order & molecularity of a reaction,, initiall rate method & integrated rate law equations, numerical problems,, Half life period, Pseudo first order reaction, Temperature of rate of reaction, Activation energy, collision frequency & effective collision, Collision theory, Arrhenius equation,, effect of catalyst on rate of reaction, numerical problems
The document discusses kinetics and the rate law for the decolorization of crystal violet. It describes using a spectroscopic colorimeter to monitor the concentration of crystal violet over time as it reacts with sodium hydroxide. The goals are to determine the overall rate law and rate constant k for the decolorization reaction. Experiments are conducted at different concentrations and the orders are determined by analyzing linear regression graphs of integrated rate laws versus time and concentration. The 1st order graph provided the best correlation, indicating the reaction is first order with respect to crystal violet concentration.
Chemical kinetics deals with the rates of chemical reactions and the factors that affect reaction rates. The rate of a reaction depends on variables like concentration, temperature, and presence of a catalyst. A reaction's rate law expresses how its rate depends on the concentrations of reactants. Integrated rate laws relate concentration over time for different reaction orders. Pseudo-first-order reactions occur when one reactant is in excess. The Arrhenius equation describes how temperature affects a reaction's rate constant.
The document discusses reaction rates and kinetics. It defines factors that affect reaction rates such as concentration of reactants, physical state, temperature, and catalysts. It also describes methods for determining reaction rates by measuring changes in concentration over time. Rate laws relate the rate of reaction to concentrations of reactants through rate constants and reaction orders. Integrated rate laws can be used to determine concentrations of reactants over time for reactions of different orders.
The document describes a laboratory experiment to determine the reaction order and rate constant of the reaction between sodium hydroxide (NaOH) and ethyl acetate (CH3COOC2H5). The group prepared 0.1 M solutions of each reactant and mixed them in a batch reactor at room temperature while measuring conductivity over time. Calculations using the conductivity readings showed the reaction was second order. The rate constant was determined to be 1.291651 × 10-3 at 21°C based on the nonlinear ln(CA/CAo) vs time graph.
This document discusses chemical kinetics and factors that affect reaction rates:
1) Reaction rates can be defined as the decrease in reactants or increase in products per unit time. Rates depend on concentrations and temperature.
2) Factors that increase reaction rates include higher concentrations, increased surface area, and higher temperatures. Higher temperatures provide more collisions with energy above the activation energy.
3) A catalyst provides an alternative reaction pathway with lower activation energy, increasing the number of effective collisions and thereby increasing the reaction rate.
This document discusses chemical kinetics and reaction rates. It begins with an introduction to chemical kinetics and defines reaction rate. It then discusses factors that affect reaction rates such as nature of reactants, concentration, temperature, and catalysts. It describes different types of reaction rates and how they are measured. The document also covers rate laws, determining rate orders experimentally, and integrated and differential rate equations for zero, first, and second order reactions. It concludes with an overview of rate theories including the Arrhenius equation.
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Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.pptHenry Hollis
The History of NZ 1870-1900.
Making of a Nation.
From the NZ Wars to Liberals,
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Social Laboratory, New Zealand,
Confiscations, Kotahitanga, Kingitanga, Parliament, Suffrage, Repudiation, Economic Change, Agriculture, Gold Mining, Timber, Flax, Sheep, Dairying,
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Chapter wise All Notes of First year Basic Civil Engineering.pptxDenish Jangid
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
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2. M5 Rate of Rxn: Speed of Rxn II
Slide 2 of 23
Learning Objectives
Concepts:
– speed (rate) of reaction, concentration, catalyst, surface area,
temperature, activation energy
Skills:
– Describe a practical method for investigating the speed of a reaction
involving gas evolution by collecting mass data over time and graphing
the result.
– Analyze and interpret data obtained from experiments on speed of
reaction
– Devise experiments to test the effect of any four of the factors on speed
of reaction
– Be able to determine rate of reaction from a mass-time graph
3. M5 Rate of Rxn: Speed of Rxn II
Slide 3 of 23
Preamble
You have learned that concentration of a reactant particles, temperature,
surface area of the reactants, and catalyst affect the speed of
reaction.
But how can we actually follow the progress of a chemical reaction to
confirm this?
Whereas speed of a vehicle is change of distance per unit time, speed of
a chemical reaction is a measure of change of a measurable quantity
per unit time.
Speed of reaction is a measure of how fast a reactant is being used up or
how fast a product is being produced.
We must therefore be able to follow the progress of a reaction by looking
at a quantity that changes over time.
4. M5 Rate of Rxn: Speed of Rxn II
Slide 4 of 23
Following the Progress of a Chemical
Reaction
As you know, we have two choices:
1. Record the change in quantity of a reactant as the reaction progresses.
– Again, the quantity measured could be mass or volume or concentration of the
reactant.
– (We will not be looking at any example of this kind because you are not likely to
encounter it this in your MYP chemistry course.)
1.Record the change in quantity of a product as the reaction progresses.
– The quantity measured could be volume or mass or concentration of the product
– We will be looking at methods involving collection and recording of volume of gas
produced first and then mass of reaction vessel.)
The method chosen depends on the chemical reaction being studied.
– Reactions that produce a gas for example can be followed by measuring the
change in volume of gas evolved or mass of the reaction vessel.
– To be sure, there are other ways of following the progress of a reaction.
5. M5 Rate of Rxn: Speed of Rxn II
Slide 5 of 23
2. Progress of a Chemical Reaction: Mass
Change of Reaction mixture
The reaction between marble chips and hydrochloric acid once again:
CaCO3 (s) + 2HCl (aq) CaCl2 (aq) + H2O (l) + CO2 (g)
Since one of the products is a gas (CO2) if allowed, it will escape from a
reaction container causing the mass to decreases over time.
6. M5 Rate of Rxn: Speed of Rxn II
Slide 6 of 23
2. Progress of a Chemical Reaction: Mass Change
of Reaction mixture
A setup shown below can be used for this.
Here too, if the speed of
the reaction is to be
determined, then mass
would be recorded at a
regular interval and the
data collected could be
analyzed in one of two
ways.
7. M5 Rate of Rxn: Speed of Rxn II
Slide 7 of 23
Analysis: Mass Change of Reaction mixture
You can either plot a graph of mass of reaction vessel against time as
shown below
or…
mass
of
reaction
vessel
/cm
3
Time/sec.
8. M5 Rate of Rxn: Speed of Rxn II
Slide 8 of 23
Analysis: Mass Change of Product
…plot a graph of mass of CO2 evolved against time.
mass
of
carbon
dioxide
/cm
3
Time /sec.
Either way, the slope of the
curve shows the speed of
the reaction.
9. M5 Rate of Rxn: Speed of Rxn II
Slide 9 of 23
Analysis: Effect of Surface Area
Comparison of speed of reaction between two different surface areas of marble
chips could be carried out by graphing the results of the two experiments on
the same graph.
Time /sec.
two 3g chips
four 3g chips
mass
of
reaction
vessel
/g
Speed higher when 4
chips used
because:
• Curve is steeper,
and
• Curve levels off
earlier—reaction
ends earlier
(Here however, the
limiting reagent
would be the
acid.)
10. M5 Rate of Rxn: Speed of Rxn II
Slide 10 of 23
Other ways of Following progress of a
reaction
You can count the number of bubbles evolved at fixed interval of time
and then plot that.
Or you can count the number of bubbles evolved in a fixed time if speed
of reaction between two or more experiments are being compared.
Concentration of one of the reactants can be determined at regular
intervals and analyzed to obtained information about speed of the
reaction, but that requires a lot more sophisticated methods and
instruments.
The only thing to remember is that regardless of the method used, if a
factor is being studied, for example concentration, that is the only
variable that should be changed from one experiment to another
otherwise the investigation will not be a fair test.
11. M5 Rate of Rxn: Speed of Rxn II
Slide 11 of 23
Determining Speed from Mass-time Graph
Time /sec.
mass
of
reaction
vessel
/g
Rise
Run
(x2, y2)
(x1, y1)
2 1
2 1
Rise
Slope = =
Run
y y
x x
How do you keep the coordinates
straight?
The coordinates for where the
tangent touches the curve is
(x1, y1) and the other one (x2,
y2).
Speed of reaction = Slope at t=0
The negative sign is required
because rate has to be a
positive value.
12. M5 Rate of Rxn: Speed of Rxn II
Slide 12 of 23
Determining Speed from Mass-time Graph
2 1
2 1
Speed =
y y
x x
2 1
180.20 180.85
Speed =
60 0
= 1.08 10
gs
0
Time/sec.
60 120 180 140
mass
of
container
/g
180.6
180.4
180.8
180.2
(60, 180.20)
(0, 180.85)
NB: Students often make the
mistake of firstly drawing a
very small tangent, and
secondly, equating y2 to “0”
when it starts above “0” as is
the case on the left.
13. M5 Rate of Rxn: Speed of Rxn II
Slide 13 of 23
Summary
Progress of a reaction can be followed by recording mass or volume or
concentration change of a reactant or product over time
Plots of the quantity measured over time furnishes information about the
speed of the reaction.
If the effect of a factor on speed is being studied, then both the relative
slope of the plots and the time taken for the reaction to go to
completion indicate the relative speeds of the reaction.
Study of the effect of a factor on the rate of a reaction can also be
carried out by determining the time taken for a fixed change in the
quantity being measured, such as mass or volume.
– The inverse (reciprocal) of the time taken in this case gives the relative
speeds.
14. M5 Rate of Rxn: Speed of Rxn II
Slide 14 of 23
Practice Questions
1. N02/6/3. Dilute nitric acid
was added to a large
amount of magnesium
carbonate in a conical
flask as shown.
The flask was placed on a
balance and the mass of
the flask and contents
recorded every minute.
Write a balanced equation
for the reaction.
15. M5 Rate of Rxn: Speed of Rxn II
Slide 15 of 23
Practice Questions
The results are shown in the table.
(a) Plot the results on the grid and draw a smooth line graph. [3]
16. M5 Rate of Rxn: Speed of Rxn II
Slide 16 of 23
Practice
Questions
17. M5 Rate of Rxn: Speed of Rxn II
Slide 17 of 23
Practice Questions
(b) (i) Which result appears to be inaccurate? Why have you selected this
result? [2]
(ii) Suggest a source of experimental error that may have caused
that result to be inaccurate. [1]
(c) Why does the mass of the flask and contents decrease? [1]
18. M5 Rate of Rxn: Speed of Rxn II
Slide 18 of 23
Practice Questions
(d) Suggest the purpose of the cotton wool. [1]
(e) At what time did the reaction finish? [1]
(f) Determine the rate of the reaction by determining the slope of the
tangent at time=0.
(g) On the grid, sketch the graph you would expect if the experiment
were repeated using nitric acid at a higher temperature. [2]
19. M5 Rate of Rxn: Speed of Rxn II
Slide 19 of 23
Practice Questions
2. J01/2/6g. A student investigated the reaction between calcium
carbonate and hydrochloric acid. Balance the quation.
CaCO3(s) + …HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g)
(ii) The student
measured the rate
of this reaction,
using the apparatus
shown to the right.
Describe how the
student could use
this apparatus to
follow the rate of
reaction. [2]
20. M5 Rate of Rxn: Speed of Rxn II
Slide 20 of 23
Practice Questions
(iii) The student wanted to find out if the concentration of hydrochloric acid
affected the rate of reaction. The student repeated the experiment using
hydrochloric acid of different concentrations.
State two things the student should keep the same in each experiment.
[2]
21. M5 Rate of Rxn: Speed of Rxn II
Slide 21 of 23
Practice Questions
(iv) Draw representative plots on the same graph for results on study of
effect of concentration using 1M and 2M hydrochloric acid with everything
else kept constant. [3]
22. M5 Rate of Rxn: Speed of Rxn II
Slide 22 of 23
Practice Questions
3. N00/2/5c. (a) The apparatus below was used to measure the volume
of gas produced when zinc reacted with hydrochloric acid.
A student measured
the volume of gas
produced during the
first minute of the
reaction.
The student
repeated the
experiment altering
one condition at a
time.
23. M5 Rate of Rxn: Speed of Rxn II
Slide 23 of 23
Practice Questions
What effect would each of the following have on the volume of gas
produced during the first minute of the reaction.
(i) decreasing the concentration of acid
(ii) increasing the temperature
(iii) using finely divided zinc instead of lumps of zinc [3]
(b) Using the collision theory explain each effect. [3]