A chemical report can be made after we have done a simple experiment or in a laboratory, following an experimental sample performed in a chemical laboratory.
1. OBJECTIVES OF EXPERIMENT
- Observe the effect of temperature change on reaction rate
2. LITERATURE REVIEW
2.1 Theoretical Basis
Chemical Kinetics is the assessment of the rate and mechanism of chemical reactions. Iron rusts faster in moist air than in dry air, eating more quickly decomposes when not cooled. This is a typical example of complex chemical changes with varying rates according to reaction conditions (Sunarya, 2002).
Reaction Rate
The reaction rate of a chemical reaction is a measure of how the concentration or pressure of the substances involved in the reaction changes with time. Reaction rate analysis is very important and has many uses, for example in chemical engineering and chemical equilibrium studies. The reaction rate is fundamentally dependent on:
• Reactant concentrations, which usually make the reaction run faster when concentration is increased. This is due to increased atomic impact per unit time,
• Surface area available for reactants to interact, especially solid reactants in heterogeneous systems. Large surface area will increase the reaction rate.
• Pressure, by increasing pressure, we decrease the volume between molecules so that it will increase the collision frequency of the molecule.
• Activation energy, which is defined as the amount of energy required to make the reaction start and run spontaneously. The higher activation energy implies that the reactants need more energy to initiate the reaction than the lower activation energies.
• Temperature, which increases the reaction rate when raised, this is because high temperatures increase the molecular energy, thus increasing collisions between molecules per unit time.
• The presence or absence of a catalyst. The catalyst is a substance that alters the path (mechanism) of a reaction and increases the reaction rate by decreasing the activation energy required for the reaction to proceed. The catalyst is not consumed or altered during the reaction, so it can be reused.
• For some reactions, the presence of electromagnetic radiation, primarily the vitiligo, is required to break the bonds necessary for the reaction to begin. This mainly occurs in reactions involving radicals (Sukamto, 1989).
The rate of reaction is related to the concentration of the substances involved in the reaction. This relationship is determined by the rate equations of each reaction. It should be noted that some reactions It should be noted that some reactions have a speed independent of reaction concentration. This is called a zero-order reaction. Reaction kinetics is a branch of chemistry that deals with reaction rates and the factors that influence them. The rate or rate of the reaction is the change in the concentration of reagents or products in a unit of time. The rate of a reaction can be expressed as the rate of reduced concentration of a reactant, or the rate of increase in the concentration of a product. The concentration is usually expressed in moles per liter. The reaction rate of a chemical reaction can be expressed by the rate equation of the reaction. For the following reactions:
A + B → AB
The reaction rate equation is generally written as follows:
R = k [A] m [B] n
K as the reaction rate constant, m and n are the partial order of each reactant.
The magnitude of the reaction rate is influenced by the following factors:
1. The nature and size of reagents
2. Concentrations of reagents
3. The reaction temperature
4. Catalyst (Sukamto, 1989).
Nature and Size of Reagents
The reagents properties and reagent size determine the rate of reaction. The more relative the reactant nature of the reaction rate will increase or the reaction progresses faster. The more the surface area of the reaction rate reactants will increase, this is explained by the increasing surface area of the reacting agent, the interaction of the reactant agent is wider. The surface of the reagents can be expanded by reducing the size of the reagents. Thus, to increase the rate of reaction, the reactant agent in powder form is preferable when compared in the form of chunks.
The nature of reagents. Substances differ significantly in their rate of chemical change. The hydrogen and flour molecules react violently, even at room temperature, by producing hydrogen fluoride molecules.
H2 + F2 → 2HF (very fast at room temperature)
In similar circumstances, the hydrogen and oxygen molecules react so slowly that no chemical change occurs:
2H2 + O2 → H2O
(Sunarya, 2002).
- Observe the effect of temperature change on reaction rate
2. LITERATURE REVIEW
2.1 Theoretical Basis
Chemical Kinetics is the assessment of the rate and mechanism of chemical reactions. Iron rusts faster in moist air than in dry air, eating more quickly decomposes when not cooled. This is a typical example of complex chemical changes with varying rates according to reaction conditions (Sunarya, 2002).
Reaction Rate
The reaction rate of a chemical reaction is a measure of how the concentration or pressure of the substances involved in the reaction changes with time. Reaction rate analysis is very important and has many uses, for example in chemical engineering and chemical equilibrium studies. The reaction rate is fundamentally dependent on:
• Reactant concentrations, which usually make the reaction run faster when concentration is increased. This is due to increased atomic impact per unit time,
• Surface area available for reactants to interact, especially solid reactants in heterogeneous systems. Large surface area will increase the reaction rate.
• Pressure, by increasing pressure, we decrease the volume between molecules so that it will increase the collision frequency of the molecule.
• Activation energy, which is defined as the amount of energy required to make the reaction start and run spontaneously. The higher activation energy implies that the reactants need more energy to initiate the reaction than the lower activation energies.
• Temperature, which increases the reaction rate when raised, this is because high temperatures increase the molecular energy, thus increasing collisions between molecules per unit time.
• The presence or absence of a catalyst. The catalyst is a substance that alters the path (mechanism) of a reaction and increases the reaction rate by decreasing the activation energy required for the reaction to proceed. The catalyst is not consumed or altered during the reaction, so it can be reused.
• For some reactions, the presence of electromagnetic radiation, primarily the vitiligo, is required to break the bonds necessary for the reaction to begin. This mainly occurs in reactions involving radicals (Sukamto, 1989).
The rate of reaction is related to the concentration of the substances involved in the reaction. This relationship is determined by the rate equations of each reaction. It should be noted that some reactions It should be noted that some reactions have a speed independent of reaction concentration. This is called a zero-order reaction. Reaction kinetics is a branch of chemistry that deals with reaction rates and the factors that influence them. The rate or rate of the reaction is the change in the concentration of reagents or products in a unit of time. The rate of a reaction can be expressed as the rate of reduced concentration of a reactant, or the rate of increase in the concentration of a product. The concentration is usually expressed in moles per liter. The reaction rate of a chemical reaction can be expressed by the rate equation of the reaction. For the following reactions:
A + B → AB
The reaction rate equation is generally written as follows:
R = k [A] m [B] n
K as the reaction rate constant, m and n are the partial order of each reactant.
The magnitude of the reaction rate is influenced by the following factors:
1. The nature and size of reagents
2. Concentrations of reagents
3. The reaction temperature
4. Catalyst (Sukamto, 1989).
Nature and Size of Reagents
The reagents properties and reagent size determine the rate of reaction. The more relative the reactant nature of the reaction rate will increase or the reaction progresses faster. The more the surface area of the reaction rate reactants will increase, this is explained by the increasing surface area of the reacting agent, the interaction of the reactant agent is wider. The surface of the reagents can be expanded by reducing the size of the reagents. Thus, to increase the rate of reaction, the reactant agent in powder form is preferable when compared in the form of chunks.
The nature of reagents. Substances differ significantly in their rate of chemical change. The hydrogen and flour molecules react violently, even at room temperature, by producing hydrogen fluoride molecules.
H2 + F2 → 2HF (very fast at room temperature)
In similar circumstances, the hydrogen and oxygen molecules react so slowly that no chemical change occurs:
2H2 + O2 → H2O
(Sunarya, 2002).
Concentrations of reagents
In general, if the greater the concentration of the substance the reaction rate is greater, and vice versa if the concentration also, and vice versa if the sentence of a substance the smaller the reaction rate becomes smaller. For some reactions, the reaction rate is getting smaller. For some reactions, the rate of reaction can be expressed by a mathematical equation known as the reaction rate or reaction law called the order of the reaction. Determining the order of reactions of a chemical reaction in principle determines how much influence the change in reagent concentration to the reaction rate (Keenan, 1979).
Temperature or Temperature Reaction
The rate of a chemical reaction increases with increasing temperature. Usually an increase of 10ºC will tuck two or three rates of a reaction between the molecules. The increase in the rate of this reaction can be explained in part as the faster the molecules move around at higher temperatures and hence collide with each other more often. However, this has not been explained entirely, to more often colliding molecules, but they also collide with greater impact (impact), as they move faster. At large temperatures, as more molecules have greater speed and hence have enough energy to react.
Almost all reactions become faster when the temperature is increased because the given heat will increase the kinetic energy of the particles of the interaction. As a result the number and energy of the collision increase (Sunarya, 2002).
Catalyst
The catalyst is a substance added to a reaction to speed up the course of the reaction. The catalyst usually reacts temporarily and then re-forms as a free agent. A reaction using a catalyst is called a catalyst reaction or a process called catalyst.
Properties of the catalyst:
1. The catalyst does not react permanently, since it does not undergo chemical changes during the reaction.
2. The catalyst does not affect the reaction end result.
3. The catalyst does not start the reaction but only affects its speed.
4. The catalyst works effectively at the optimum temperature.
5. A catalyst affects only the specific reaction rate, meaning the catalyst acts on one reaction or a kind of reaction and not for other types of reactions.
6. The activation of the catalyst may be enlarged by another substance called promoter.
7. The result of a reaction can sometimes act as a catalyst and is called an autocatalyst.
8. The catalyst may react with other substances so that the catalyst properties are lost.
9. A catalyst that can slow down the reaction is called a negative catalyst (Sunarya, 2002).
Catalyst Classification:
Based on the phase can be divided into 2, namely homogeneous catalyst and heterogeneous catalyst.
1. Homogeneous catalyst is a catalyst which has the same phase as the reagent, possibly gas, liquid and solid.
2. Heterogeneous catalysts are catalysts having different phases with reagents. Generally these catalyst substances are solid and liquid or gas reactants (Sunarya, 2002).
In general, if the greater the concentration of the substance the reaction rate is greater, and vice versa if the concentration also, and vice versa if the sentence of a substance the smaller the reaction rate becomes smaller. For some reactions, the reaction rate is getting smaller. For some reactions, the rate of reaction can be expressed by a mathematical equation known as the reaction rate or reaction law called the order of the reaction. Determining the order of reactions of a chemical reaction in principle determines how much influence the change in reagent concentration to the reaction rate (Keenan, 1979).
Temperature or Temperature Reaction
The rate of a chemical reaction increases with increasing temperature. Usually an increase of 10ºC will tuck two or three rates of a reaction between the molecules. The increase in the rate of this reaction can be explained in part as the faster the molecules move around at higher temperatures and hence collide with each other more often. However, this has not been explained entirely, to more often colliding molecules, but they also collide with greater impact (impact), as they move faster. At large temperatures, as more molecules have greater speed and hence have enough energy to react.
Almost all reactions become faster when the temperature is increased because the given heat will increase the kinetic energy of the particles of the interaction. As a result the number and energy of the collision increase (Sunarya, 2002).
Catalyst
The catalyst is a substance added to a reaction to speed up the course of the reaction. The catalyst usually reacts temporarily and then re-forms as a free agent. A reaction using a catalyst is called a catalyst reaction or a process called catalyst.
Properties of the catalyst:
1. The catalyst does not react permanently, since it does not undergo chemical changes during the reaction.
2. The catalyst does not affect the reaction end result.
3. The catalyst does not start the reaction but only affects its speed.
4. The catalyst works effectively at the optimum temperature.
5. A catalyst affects only the specific reaction rate, meaning the catalyst acts on one reaction or a kind of reaction and not for other types of reactions.
6. The activation of the catalyst may be enlarged by another substance called promoter.
7. The result of a reaction can sometimes act as a catalyst and is called an autocatalyst.
8. The catalyst may react with other substances so that the catalyst properties are lost.
9. A catalyst that can slow down the reaction is called a negative catalyst (Sunarya, 2002).
Catalyst Classification:
Based on the phase can be divided into 2, namely homogeneous catalyst and heterogeneous catalyst.
1. Homogeneous catalyst is a catalyst which has the same phase as the reagent, possibly gas, liquid and solid.
2. Heterogeneous catalysts are catalysts having different phases with reagents. Generally these catalyst substances are solid and liquid or gas reactants (Sunarya, 2002).
3. METHOD OF EXPERIMENT
3.1 Tools and Materials
3.1.1 Tools
- 6 Test tubes
- Drop pipette
- Stopwatch
- 3 cup goblets
- Bunsen
3.1.2 Materials
- 2 ml of 0.1 M oxalic acid
- 0.5 ml of H2SO4 6 M
- KMnO4 0.1 M
3.2 Work Scheme
3.2.1. The influence of temperature on the reaction rate
For this experiment, there is an example of a reaction between oxalic acid and potassium permanganate in an acidic atmosphere
1. take 6 test tubes, fill each with 2 ml of 0.1 M oxalic acid and 0.5 ml of 6 M sulfuric acid.
2. Prepare 3 cups of trophy, fill half with water. The first cup of the cup was boiled, the 2nd cup cup was heated to 50 ° C, and the third cup was not heated.
3. Insert 2 test tubes into each cup. After 10 minutes, into each tube plus 3 drops of KMnO4 0.1 M. notice the color change and record the time and reaction in each tube.
4. RESULT AND DISCUSSION
4.1. Results
From the experiment conducted got the following results:
3.1 Tools and Materials
3.1.1 Tools
- 6 Test tubes
- Drop pipette
- Stopwatch
- 3 cup goblets
- Bunsen
3.1.2 Materials
- 2 ml of 0.1 M oxalic acid
- 0.5 ml of H2SO4 6 M
- KMnO4 0.1 M
3.2 Work Scheme
3.2.1. The influence of temperature on the reaction rate
For this experiment, there is an example of a reaction between oxalic acid and potassium permanganate in an acidic atmosphere
1. take 6 test tubes, fill each with 2 ml of 0.1 M oxalic acid and 0.5 ml of 6 M sulfuric acid.
2. Prepare 3 cups of trophy, fill half with water. The first cup of the cup was boiled, the 2nd cup cup was heated to 50 ° C, and the third cup was not heated.
3. Insert 2 test tubes into each cup. After 10 minutes, into each tube plus 3 drops of KMnO4 0.1 M. notice the color change and record the time and reaction in each tube.
4. RESULT AND DISCUSSION
4.1. Results
From the experiment conducted got the following results:
|
repeated
|
temperatures
|
||
|
100
|
50
|
25
|
|
|
1
|
purple 0 s
brown 10 s
Bening 13 s
|
purple 0 detik
brown 17 detik
Bening 22 detik
|
purple 0 detik
purple young 17 detik
brown 34 detik
Bening 51 detik
|
|
2
|
old
|
old
|
old
|
|
averages
|
7,67 s
|
13 s
|
25,5 s
|
4.2. Discussion
So based on the experiment can be seen the color changes that occur and how many seconds the reaction rate of the experiment. The higher the temperature the faster the reaction rate progresses.
5. REFERENCES
Keenan, et al. 1979. Chemistry for Universities. Jakarta: Erland.
Sukamto. 1989. Chemical Physics. Jakarta: PT.Bhineka Cipta.
Sunarya, Yayan. 2002. Basic Chemistry II Based on Recent Chemical Principles. Bandung: Alkemi Grafisindo Press.
6. APPENDIX
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