The aim of this experiment is to find out how the temperature effects the action of lipase.
Robynne Shipley 10G Factors Effecting Action of Lipase Effect of Temperature on the action of Lipase Aim The aim of this experiment is to find out how the temperature effects the action of lipase. Method * A glass beaker was taken and filled with about halfway with water. * The water was then heated to 50°c * Into a boiling tube 5 cm³ of milk, 7 cm³ of sodium carbonate and a few drops of Phenothalin were placed. * The boiling tube was placed into the water for a few minutes so it could warm to the temperature of the water. * Then 1 cm³ of lipase was added and the stopwatch started. * When the reaction had finished (i.e. the milk wasn't pink anymore) the stopwatch was stopped and the time recorded. * Other groups did different temperatures and all the results were shared. Apparatus * Boiling tube * Milk * Sodium carbonate * Lipase (5% conc.) * Phenothalin * Glass beaker * Tripod * Gauze * Bunsen burner * Heat proof mat * Thermometer * Stop watch Prediction I think that the 30°c experiment will have the fasted reaction rate because it is the closest to body temperature where the enzymes naturally work. At 100°c I predict that there will be no reaction because the enzymes will be de-natured because it is so hot. And at 0°c I predict there will also be no reaction as it will be too cold for the enzymes to
An investigation into how concentration affects the rate of a reaction
An investigation into how concentration affects the rate of a reaction PLANNING AIM The aim of this investigation is to see how differing concentrations of a solution affect the rate of a reaction. In this case, the solution is Hydrogen Peroxide solution (H2O2) and the catalyst is Manganese Oxide (MnO4). VARIABLES The variables that must be controlled in this reaction are: * Temperature * Concentration of solution * pH * Time * Catalysis * Surface area of catalyst (powder or granules) * Volume/Mass (solution/catalyst) The variable I have chosen to control is the concentration of the solution. HYPOTHESIS The reaction that I plan to measure is: MnO4 2H2O2 = 2H2O + O2 I believe that as the concentration of the solution increases, the rate of the reaction will also increase, in the same ratio. Further to this, this will be in a directly proportional ratio, giving a straight-line graph through the origin on a 'rate against concentration' graph. However, this rate cannot continue exponentially, there must be a 'peak rate of reaction', where the rate cannot increase further. This will mean that the graph flattens off, giving a plateau effect. This is what I estimate the graph to look like: Rate (grams of O2 released/minute) Concentration This hypothesis can be explained by a simple quotation from, Chemistry, An Experimental Science: "By increasing the
Investigate, analyse and evaluate the effect on the rate of reaction of varying the concentration of hydrochloric acid in the reaction with magnesium.
Sam Daniels Chemistry Coursework AN INVESTIGATION INTO THE REACTION BETWEEN HYDROCHLORIC ACID AND MAGNESIUM * Aim My aim is to plan, investigate, analyse and evaluate the effect on the rate of reaction of varying the concentration of hydrochloric acid in the reaction with magnesium. The chemical equation of the reaction I am investigating is: Mg (s) + 2HCl (aq) --> MgCl2 (aq) + H2 (G) * Rate of Reaction Rate of Reaction = Gas Produced Time taken To measure the rate of reaction I can use three ways: Precipitation - this is when the reaction's product is a precipitate which clouds the solution. Change in mass - a reaction which produces a gas will lose mass and this can be shown by carrying out the reaction on a balance. Volume of gas given off - A gas cylinder gas be used to collect the gas given off. Rate of reaction depends on four separate things: Temperature, concentration (or pressure for gases), size of particles (or surface area for liquids) and the presence of a catalyst. Rate of reaction is a change in mass or volume or concentration per unit of time. An increased rate could be the product of any of these factors: an increase in temperature, an increase in concentration, an increase in surface area or the introduction of a catalyst. * Variables The variables available to investigate are: Mass of Magnesium Used Temperature of surroundings Time of
Investigate how temperature affects the rate of reaction of the enzyme catalase on its substrate hydrogen peroxide.
Aim To investigate how temperature affects the rate of reaction of the enzyme catalase on its substrate hydrogen peroxide. Scientific Background Enzymes are biological catalysts which increase the rate of reactions by lowering the activation energy needed for the reaction to tale place. The activation energy is the amount of energy needed for molecules to react when they collide. Molecules need to collide in order to react, this is known as the collision theory. When they collide they may not react as a certain amount of energy is required to break bonds, this energy is the activation energy. Enzymes are made of a long amino acid chain, within this some molecules are attracted to each other, so the chain folds in on itself to form a 3D shape. How enzymes are shaped. An area on the surface of the enzyme is known as the active site. This is where reactions take place to form or break down substances. Enzymes are specific which means a particular enzyme only works on one substance known as its substrate. For example, the substrate of amylase is starch and the substrate of lipase is fats. They only have one substrate because the active site is formed in a different shape for each enzyme, where only one substance can fit. The 'lock and key' hypothesis states that the enzyme is like a lock which will only have one key. 'Lock and Key' hypothesis The substrate shown is the
To investigate how surface area effects the rate of reaction in Calcium Carbonate.
An Nguyen 11P EXPERIMENT TO SEE HOW SURFACE AREA WILL EFFECT THE RATE OF REACTION Aim To investigate how surface area effects the rate of reaction in Calcium Carbonate. Theory This experiment is working on the theory of diffusion. Diffusion is the movement of particles. Three main things effect the rate of diffusion: - The distance of particles. Diffusion is quickest in gases as gas has a larger space between molecules making diffusion occur faster. - The energy of particles. The temperature effects the rate of reaction because the higher the temperature the faster the reaction. - The mass of particles. The effect of mass is caused by the relationship between the speed of particles and their temperature. Diffusion occurs in all the states of matter. However they most noticeably take place in liquids and gases. An example of this is Brownian Motion. Robert Browning noticed that when looking under a microscope pollen grains were moving in a random way. This movement is explained by assuming water molecules were hitting the pollen grains in a random way causing the pollen to move erratically. Brownian motion and diffusion provide evidence to support the kinetic theory. The kinetic theory is kinetic energy cannot be created loss or destroyed. Instead it is converted to another form of energy. Particles have kinetic energy - the energy of movement. Gases have the
An Investigation into the effects of concentration on the reactions between magnesium and hydrochloric acid
Amy Watson 10v An Investigation into the effects of concentration on the reactions between magnesium and hydrochloric acid Introduction There are four factors that affect how fast a reaction happens (its rate.) They are: * Temperature * Surface area * The concentration * A catalyst In this experiment I am going to investigate only one of these factors, the concentration (or pressure in gases.). The concentration can be rise in product or fall in reactant. Rate of a reaction = Change in concentration Change in time I am going to investigate the effect concentration has on the rate of reaction by adding magnesium to hydrochloric acid and measuring how much hydrogen is given off in what time. Metal + acid Salt + hydrogen Magnesium + hydrochloric acid magnesium chloride+ hydrogen Mg (s)+ 2HCl(aq) MgCl (aq) + H (g) Hypothesis I predict that the higher the concentration is the faster the rate of reaction. As the concentration is increased so will the rate of reaction, they are directly proportional. I predict that this will happen because as the concentration is increased so is the number of collisions of particles per second. The chloride ions will collide with the magnesium ions to form MgCl in solution as Mg and Cl . The hydrogen ions will collide with each other to form hydrogen molecules. The following variables will affect
To Investigate How The Concentration Of Reactants Affects The Rate Of a Chemical Reaction.
To Investigate How The Concentration Of Reactants Affects The Rate Of a Chemical Reaction. Introduction/background information For our coursework we are doing an experiment to see how different concentrations of reactants affect the rate of a chemical reaction. * What is a reaction? A reaction occurs when two particles join together to produce different product(s) * What is a reactant? A reactant is a substance that reacts with another substance * What is a rate? The rate is the measure of how fast or slow the reaction takes place * How can we measure the rate? You can either measure how much of a reactant is used up in a given time or how much product is given off in a given time Collision theory Collision theory tells us that particles must collide before they can react and they need enough energy to break their bonds in order for the collision to be successful and result in a reaction. The energy needed is called activation energy. During a reaction the rate does not remain constant, because at first there are lots of particles so it is easier for them to collide. Later on in the course of a reaction there are fewer particles left to collide. The chance of a successful collision can be affected by different variables. These include: * Temperature- the hotter the temperature, the faster the particles are moving and the more likely they are to collide
To see the effects of a change in and concentration on the rate of a reaction.
We must produce a piece of coursework investigating the rates of reaction, and the effect different changes have on them. The rate of reaction is the rate of loss of a reactant or the rate of formation of a product during a chemical reaction. It is measured by dividing 1 by the time taken for the reaction to take place. There is five factors which affect the rate of a reaction, according to the collision theory of reacting particles: temperature, concentration (of solution), pressure (in gases), surface are (of solid reactants), and catalysts. I have chosen to investigate the effect concentration have on a reaction. This is because it is the most practical to investigate. the use of a catalyst complicates things, and if used incorrectly could alter the outcome of the experiment. Aim: - To see the effects of a change in and concentration on the rate of a reaction. The reaction that will be used is: Sodium Thiosulphate + Hydrochloric Acid Na2S2O3 (aq) + 2HCl (aq) Sodium Chloride + Water + Sulphur Dioxide + 2NaCl (aq) + H2O (l) + SO2 (g) + Sulphur S (s) Both the sodium thiosulphate and the Hydrochloric acid are soluble in water, so the concentration of either can be changed. However I have chosen to vary the sodium thiosulphate as it is available in larger amounts, and various concentrations are prepared. When the temperature is constant room temperature will be
Investigating Factors Affecting the Rate of a Chemical Reaction
Manaan Malik 5f presents... Mr Phillips- Chemistry "INVESTIGATING FACTORS AFFECTING THE RATE OF A CHEMICAL REACTION" Introduction I will be conducting an experiment investigating two different factors that can affect the rate of reaction in a chemical experiment. The reactants, which I will be experimenting with, are HYDROCHLORIC acid (aq) and SODIUM THIOSULPHATE (aq). With rate meaning the speed of the reaction. We know that there are many factors that can affect this, such as; * Surface area * Concentration of reactants * Temperature of the reactants * Catalyst * Light * Mixing From this list I must choose two suitable factors affecting rate of reaction to investigate. I will be looking for the most practical and which factors would hopefully give us the most varied set of results. As for the other factors, which I'm not investigating but could affect the rate, these must be controlled. The effects of, and controlling, the factors. Catalyst- The job of a catalyst is to weaken bonds and therefore lower the activation energy thus increasing the rate of reaction as it makes it easier for both reactants to react. I will control this by making sure there is no catalyst present. Light Intensity- light intensity will have little effect on the rate of reaction so therefore I will take minimal caution in controlling this factor. I will simply carry out my
Effect of concentration on the rate of reaction between Sodium Thiosulphate and Hydrochloric acid
Effect of concentration on the rate of reaction between Sodium Thiosulphate and Hydrochloric acid Aim: The aim of the experiment is to find out if the concentration of Hydrochloric acid effects the rate of reaction between sodium thiosulphate and hydrochloric acid. Equation: Na2 S2 O3(aq) + 2HCL(aq) H2O(1) + SO2(g) + S(s) + 2NaCL(aq) Sodium thiosulphate + Hydrochloric acid Water + Sulphur dioxide + Sulphur + Sodium Chloride Preliminary work: The main aim of this experiment is to find out about concentration. This means that I will require having knowledge on the subject. Concentration is the number of molecules of a certain substance in a solution with other substance. An easy way of explaining this is with Ribena drink. When you first pour the ribena into a glass the ribena is 100% concentrated. After that you then add water, the water dilutes the ribena and alters the concentration of it. This means that the drink has been diluted and is not so concentrated. The diagram below illustrates this (diagram 1). Diagram 1: Each of the circles represents a molecule of either ribena or water, purple for ribena and blue for water. When the two are mixed together you are left with a solution. The solution is made up of a number of both molecules. This is very similar to the reaction between sodium thiosulphate and hydrochloric acid, which
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