...Rate of Reaction The rate of a reaction is the speed at which a chemical reaction happens. If a reaction has a low rate, that means the molecules combine at a slower speed than a reaction with a high rate. Some reactions take hundreds, maybe even thousands, of years while others can happen in less than one second. If you want to think of a very slow reaction, think about how long it takes plants and ancient fish to become fossils (carbonization). The rate of reaction also depends on the type of molecules that are combining. If there are low concentrations of an essential element or compound, the reaction will be slower. There is another big idea for rates of reaction called collision theory. The collision theory says that as more collisions in a system occur, there will be more combinations of molecules bouncing into each other. If you have more possible combinations there is a higher chance that the molecules will complete the reaction. The reaction will happen faster which means the rate of that reaction will increase. Think about how slowly molecules move in honey when compared to your soda even though they are both liquids. There are a lower number of collisions in the honey because of stronger intermolecular forces (forces between molecules). The greater forces mean that honey has a higher viscosity than the soda water. Factors That Affect Rate Reactions happen - no matter what. Chemicals are always combining or breaking down. The reactions happen over and...
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...Investigating Rates of Reaction between Hydrochloric Acid and Magnesium Introduction What is Rate of Reaction? The reaction rate or rate of reaction for a reactant or product in a particular reaction is intuitively defined as how fast a reaction takes place. For example, the oxidation of iron under the atmosphere is a slow reaction which can take many years, but the combustion of butane in a fire is a reaction that takes place in fractions of a second. In this case how fast Magnesium reacts with Hydrochloric Acid. The equation for the reaction is magnesium + hydrochloric acid magnesium chloride + hydrogen Mg(s) + 2HCl(aq) MgCl2(aq) + H2(g) This is the equation for the reaction which will occur during my experiment What am I investigating? I am investigating the rate of reaction when the concentration of hydrochloric acid is increased with magnesium. What I am expecting is when the concentration increases so to will the speed of the reaction backing up the collision theory. This will be timed and put into seconds on how fast I gather an amount of gas and from my results a graph will show this data. Method To measure how long it takes to gather the amount of gas I had to carefully measure out 50ml of Hydrochloric Acid in a measuring cylinder. I kept this the same throughout all of the experiments in order for a fair test. I then poured this into the conical flask. After this I folded the 10cm...
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...Investigation of the Rates of Reaction By Gabriella Azanu 11A Introduction A chemical reaction is when a material is changed from a beginning mass to a resulting substance through the addition of one or more other substances. In a chemical reaction, at least one or more new substances are created and the beginning mass disappears in order to make the new mass. In a chemical reaction however, mass is neither lost nor gained so the resulting mass should still be the same as the beginning mass. A reaction can be perceived by either production of gas or a change in colour or properties. A rate of reaction is the measurement of how quickly a reaction occurs. This can be done through following the formation of a product or the consumption of a reactant. This is turn can measured by observing colour changes or a precipitate forming. There are four factors that can affect the rate of reaction, these are: the concentration, temperature, surface area and catalysts. The factors can be attributed to the collision theory and then each factor explained in more depth. In a reaction, molecules in substances can only react only if they collide into each other. The collision theory therefore states that as molecules collide, bonds between atoms can break whiles new ones form. This in turn creates new molecules. Because molecules are always moving in liquids and gases, there are millions of collisions between them every second. Very...
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...Determination of the Reaction Rate of Mg and HCl Alex Skartvedt Alex Skartvedt, Melanie Ho, Christina Olson, Thor Swerdykiak November 11, 2015 Fall 2015 Semester Abstract: The experimental rate law of the reaction: 2HCl(aq)+Mg(s)→MgCl2(aq)+H2(g) is being determined because kinetics play a large role in the reactions happening in everyday life. The rate law, k value will be obtained in the experiment. To obtain the information a pressure probe was connected to an Erlenmeyer flask in order to record the rate of the reaction of magnesium ribbon and hydrochloric acid. The order of HCl and Mg were then determined using the information found in from the reaction. The order in HCl and Mg were found to be less than the expected...
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...Chemistry Coursework : Rates of Reaction Chemistry Table of Contents Table of Contents 1 Strand Sa 2 The Science 2 Variables 2 Temperature 2 Concentration 2 My Prediction 3 Strand Sb 3 Risk Assessment. 3 Preliminary Equipment 4 Preliminary Method 6 Strand C 7 Preliminary Data 7 Main Method 8 Main Results. 9 Strand Ea 9 Problems Encountered when collecting data. 9 Alternate Methods 10 Light Meter 10 Gas Collection 10 Strand Eb 11 Data Analysis 11 Graph Evaluation 11 Strand Ra 12 Secondary Data 1 12 Secondary Data 2 13 Secondary Data 3 14 Strand Rb 15 Conclusion 15 Bibliography 16 Strand Sa The Science In the experiment, I will be testing how increasing the concentration of the reactant affects the rate of reaction between hydrochloric acid and sodium thiosulfate .Due to Max Trautz’s collision theory, which states that the higher the concentration of the reactant raises the number of collisions, I predict that the less dilute sodium thiosulfate solution will have a higher reaction rate than that of a lower concentration of sodium thiosulfate. The formula for the reaction is: HCl(aq) + Na2S2O3(aq) NaCl(aq) + SO2(g) + S(s) + H2O(l). The formula shows us that the sulphur precipitate is formed along with water, sodium chloride and sulphur dioxide. Sulphur dioxide is a poisonous gas and so extra care will be taken not to inhale any. Figure 1 [18] Variables The Variables that affect the reaction rate of sodium thiosulfate...
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...Practical 12 : Rate Of Reaction Name : AFNAN BIN ABDUL RAHMAN Class : M11J Research Question : How does the reaction between Zinc metal and 0.1M of Hydrochloric Acid using different sizes of Zinc metal (Powdered Zinc, Shredded Zinc strip and Zinc strips) can affect the volume of Hydrogen gas produced at the end of the experiment (after 10 minutes) under same temperature which is room temperature? Variables : Manipulated : Different sizes of Zinc Metal Responding : Volume of Hydrogen Gas produced after 10 minutes. Constant : Constant | Method to control | Possible Effect(s) | Concentration of Hydrochloric Acid | The concentration of Hydrochloric Acid was kept constant to be used in both experiments which is 0.1 Mole. | The difference in concentration might alter the results as the rate of reaction will also differ since the effective collision will occur more when the concentration increases. | Time taken for the reaction to occur | The period of reaction for each reaction was kept constant which is 10 minutes for each experiments. | Longer period of time will increase the possibilities of effective collision between the molecules and alter the final result. | Temperature of surrounding | Both experiments were conducted in a lab with room temperature. | The difference in temperature might cause the difference in kinetic energy of the molecules and will disturb the result of the rate of reaction between Zinc and Hydrochloric Acid. | Material and Apparatus...
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...Laboratory Report The Rate of Reactions Abqari Afandi Grade 10 October 6th 2014 Purpose: To investigate the relationship between the temperatures of Hydrochloric acid with the duration of Magnesium ribbon to dissolve in the acid. Procedure: 1- Prepare four 400ml beaker: one for the hot bath, one for the room temperature, one for ice water bath and one for super hot bath. Fill all beakers half-full. Put one on a hot plate; the temperature of the water on the hot plate should not exceed 60C. Put another one on a hot plate; the temperature of water should not exceed 80C. Control the temperature of both hot plates to keep the temperature of water stays at 60C and 80C. 2- Using a graduated cylinder, add 20ml of 1M hydrochloric acid to each of the two test tubes, (all tubes should be the same size) 3- Place one test tube in the room temperature water, one test tube in the hot water bath, one in the ice water bath, and one in the super hot bath; allow the tubes to sit for approximately 5 minutes to reach thermal equilibrium. 4- Obtain a strip of magnesium ribbon (~16cm). Using scissors cut the ribbon into 4.0 strips. Be as precise as possible. 5- Wrap a piece of copper wire around a pencil to make a small ‘cage’ into which the magnesium ribbon will be inserted. The other end of the wire should be long enough so that the wire can hang over the side of the test tube with the cage submerged beneath the liquid level in the test tube. 6- Measure and...
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...Introduction It has been determined that the rates of chemical reactions are affected by temperature. This experiment is done to test the effect of five different temperatures on the rate of carbon dioxide production in yeast by measuring the fermentation rate. “The fermentation rate is measured in ml/min.” The purpose for performing this experiment is to understand the rate of fermentation of yeast cells which can be determined by measuring the amount of carbon dioxide produced at each temperature. Since there is no direct way to measure the carbon dioxide produced in the lab, an indirect method is used instead. The fermentation rate in this experiment is measured in ml/min which is the rate of carbon dioxide production that is measured over time spent in each water bath. Water will substitute for the carbon dioxide produced at the end of the experiment. The amount of water is measured in milliliters (by the graduated cylinder) will serve as an indirect method of fermentation rate because carbon dioxide is a gas which cannot be measured by means other than indirectly with this experiment. Carbon dioxide production was measured by measuring the volume of water at different temperature; 25°C, 35°C, 45°C, 55°C, and 65°C. The time was also recorded at which all the measurements were taken for the different temperatures. Materials and Method The materials used in this experiment was: Yeast culture (contains yeast and glucose in the form of molasses) Five fermentation tubes...
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...A Kinetics Experiment The Rate of a Chemical Reaction: A Clock Reaction Andrea Deoudes February 2, 2010 Introduction: The rates of chemical reactions and the ability to control those rates are crucial aspects of life. Chemical kinetics is the study of the rates at which chemical reactions occur, the factors that affect the speed of reactions, and the mechanisms by which reactions proceed. The reaction rate depends on the reactants, the concentrations of the reactants, the temperature at which the reaction takes place, and any catalysts or inhibitors that affect the reaction. If a chemical reaction has a fast rate, a large portion of the molecules react to form products in a given time period. If a chemical reaction has a slow rate, a small portion of molecules react to form products in a given time period. This experiment studied the kinetics of a reaction between an iodide ion (I-1) and a peroxydisulfate ion (S2O8-2) in the first reaction: 2I-1 + S2O8-2 I2 + 2SO4-2. This is a relatively slow reaction. The reaction rate is dependent on the concentrations of the reactants, following the rate law: Rate = k[I-1]m[S2O8-2]n. In order to study the kinetics of this reaction, or any reaction, there must be an experimental way to measure the concentration of at least one of the reactants or products as a function of time. This was done in this experiment using a second reaction, 2S2O3-2 + I2 S4O6-2 + 2I-1, which occurred simultaneously with the reaction under investigation. Adding...
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... 15: Kinetics 15.1 15.2 15.3 15.4 15.5 15.6 15.7 15.8 15.9 Week 15 Reaction Rates Rate Laws Forms of Rate Laws Integrated Rate Law Rate Laws: A Summary Reaction Mechanisms Steady-State Approximation A Model for Chemical Kinetics Catalysis CHEM 1310 - Sections L and M 1 Reaction Rates: Example Recap: Avg. Reaction rate = +∆[Product]/∆t Avg. Reaction rate = -∆[Reactant]/∆t Butane, C4 H 10, burns in oxygen to give CO2 and H2 O vapor. If the butane concentration is decreasing at a rate of 0.20 M/s, what is the rate at which the oxygen is decreasing? What is the rate at which the products are increasing? 2C4H10(g) + 13O2(g) Week 15 8CO2(g) + 10H2O(g) 2 CHEM 1310 - Sections L and M Reaction Rates: Example Butane, C4 H 10, burns in oxygen to give CO2 and H2 O vapor. If the butane concentration is decreasing at a rate of 0.20 M/s, what is the rate at which the oxygen is decreasing? What is the rate at which the products are increasing? 2C4H10(g) + 13O2(g) 0.20 M/s For oxygen: 0.20 mol C4 H 10 Ls Week 15 8CO2(g) + 10H2O(g) ? ? ? x 13 mol O2 2 mol C4 H 10 CHEM 1310 - Sections L and M = 1.3 M O2 /s 3 1 Reaction Rates: Example Butane, C4 H 10, burns in oxygen to give CO2 and H2 O vapor. If the butane concentration is decreasing at a rate of 0.20 M/s, what is the rate at which the oxygen is decreasing? What is the rate at which the products are increasing? 2C4H10(g) + 13O2(g) 0.20 M/s For CO2: 0.20 mol C4...
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...biochemical reactions. The enzymatic reactions were looked at by the use of two comparable reactions of enzyme invertase and a acidic form of the reaction. The order of the nonacidic enzymatic reaction was zero order due to substrate concentration and due to the fact that the reaction was time dependent. It is also due to having large R2 value at 0.9932 for D run and a smaller R2 value at 0.9902 for C run. The acidic runs had a first order reaction, which had a lower R2 values at 0.9028 for run D and 0.9028 for run C. Also, the percent error in run C at 33.31% was found to be much lower than the percent error in run D at 55.77%, which mean the concentration of run C is more effective than run D. I. Introduction In this experiment the chemical kinetics of the enzyme catalyzed inversion of sucrose was studied. The reaction that we will study in this experiment is the inversion of sucrose, catalyzed by the enzyme invertase that is derived from yeast: The rate of reaction of this reaction was compared to the same reaction that is to be catalyzed by hydrogen ions. Enzymes make up an important class of proteins that are used to catalyze a wide array of biochemical reactions. The enzyme that was used to catalyze the reactions in this lab experiment was the enzyme invertase (β-fructofuranidase). The first to propose the basic mechanism for enzyme-catalyzed reactions was Michaelis...
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...Enzyme Lab INTRODUCTION: What would happen to your cells if they made a poisonous chemical? You might think that they would die. In fact, your cells are always making poisonous chemicals. They do not die because your cells use enzymes to break down these poisonous chemicals into harmless substances. Enzymes are proteins that speed up the rate of reactions that would otherwise happen more slowly. The enzyme is not altered by the reaction. You have hundreds of different enzymes in each of your cells. Each of these enzymes is responsible for one particular reaction that occurs in the cell. In this lab, you will study an enzyme that is found in the cells of many living tissues. The name of the enzyme is catalase (KAT-uh-LAYSS); it speeds up a reaction which breaks down hydrogen peroxide, a toxic chemical, into 2 harmless substances--water and oxygen. The reaction is: 2 H2O2 ----> 2 H2O + O2 This reaction is important to cells because hydrogen peroxide (H2O2) is produced as a byproduct of many normal cellular reactions. If the cells did not break down the hydrogen peroxide, they would be poisoned and die. In this lab, you will study the catalase found in liver cells. You will be using chicken or beef liver. It might seem strange to use dead cells to study the function of enzymes. This is possible because when a cell dies, the enzymes remain intact and active for several weeks, as long as the tissue is kept refrigerated. MATERIALS: 1molar HCl solution 1molar NaOH...
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...Title: The effect of the concentration of hydrogen peroxide on the rate of reaction of catalase from potato Focus question: How will the concentration of the substrate hydrogen peroxide affects the rate of reaction of the enzyme catalase. Apparatus/Materials: Goggles, Lab coat, Potato, Core, 100mL beaker, Hose and stopper, Different concentrations of hydrogen peroxide (3.0%, 6.0% and 9.0%), Gas collecting tube Variables: Dependent variable: (1) rate of oxygen production Independent variable: (1) Concentrations of hydrogen peroxide (3.0%, 6.0% and 9.0%) Controlled variable: (1) The size and mass of the potato slices (2) The amount of time each experiment was left (3) The volume of hydrogen peroxide placed in the cylinder (4) The size of the test tubes (5) Temperature was left constant at room temperature (optimum temperature for catalase) Procedure: 1. The lab coat and googles were put on 2. A potato was sliced into two equal pieces using a core 3. The potato slices was placed into a test tube 4. The gas collection tube was completely filled with water and placed into a 100mL beaker which was also filled with water. 5. The hose in the ‘stopper and hose’ was placed in the gas collection tube 6. 10 mL of 3% hydrogen peroxide was added and the stopper was immediately attached to the test tube as seen in the diagram below 7. The amount of oxygen produced was measured every minute for five minutes 8. Observations...
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...Title: Enzyme Introduction The main reason for conducting this experiment is to establish the various factors that affect enzymes and reaction rates. Various experiments have been conducted to help gain a wide range of the factors that affect enzyme controlled reactions. Enzymes are affected by very many factors. It was the main aim of this experiment to establish these factors and the manner in which they affect them. This experiment also seeks to establish the manner in which some enzymes like Catalase affect the rates of reactions (Cohnheim 2009). Methods To establish the factors that affect enzymes, the procedures for the experiments to be carried out had to be almost perfect. For this reason the apparatus to be used had to be cleaned thoroughly just before commencing the experiment. To avoid differentiated results, similar kinds of apparatus were used all through the experiment. In this case glass test tubes were used. Also measuring apparatuses used were of the same size and volume. In this case four experiments were carried out. The first experiment is to establish the manner in which the enzyme Catalase affects reaction rates. The procedure of this experiment is as follows; using a pencil, label tree test tubes as test tube 1, 2 & 3. On these test tubes, label two marks using the pencil. These are at the 1cm mark and at the 5 cm mark. For the first test tube, pour in Catalase enzyme up to the first mark and add Hydrogen Peroxide up to the...
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...The rate of a chemical reaction can be raised by temperature, concentration of solutions, catalysts, etc. Increasing the surface area of a solid reactant is one way the rate of reaction can be sped up. If the surface area is increased, then more particles are exposed to reactants, there are more collisions, and these two variables overall speed up the rate of reaction. (BBC, 2014) A solid that is found in a solution can only react when particles collide with the surface area of the solid. When the area of the surface of the solid is bigger, then more particles are able to collide against it per second and the rate of the chemical reaction happening increases. (Chem4kids.com)A powdered solid will produce a faster reaction than if the same mass of the solid is presented in a single clump or small pieces....
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