To find out and analyse what factors affect the rate of reaction between limestone and acid rain.
Chemistry - Rate of Reaction Coursework Section 1: Planning Aim To find out and analyse what factors affect the rate of reaction between limestone and acid rain. Background Information Most materials that are exposed to outdoor conditions are likely to eventually erode due to a natural weathering process. Limestone and marble are two rocks that are often used in the construction of buildings, and this has been so since the 19th century. Both rock types contain a large amount of calcium carbonate. All carbonate materials are likely to erode due to rain. Pure water has a pH of 7, however rain is slightly acidic, with a pH of approximately 5.6. Rain water in some areas has known to be even more acidic, with a pH of 3 or less. The chemical equation for this reaction is: Calcium Carbonate + Hydrochloric Acid --> Calcium Hydroxide + Carbon Dioxide CaCo3 + H2SO4 --> CaOH2 + CO2` I know that these three main factors could affect the rate of reaction between limestone and acid rain: * Temperature * Surface Area * Concentration (of solution) * Pressure (of gas) However in my experiment I am only going to investigate one of these factors. I have decided that surface area isn't the best one to choose because I only have 3 different sized marble chips so I wouldn't get a very large range of results to plot onto my graphs. I have
Rates of Reaction
Introduction In this investigation I am investigating the reaction between hydrochloric acid and calcium carbonate (known as limestone). The rate of reaction is basically the speed a reaction takes place- meaning how long it occurs for. Chemical reactions only occur when reacting particles collide with each other with sufficient energy to react. The minimum amount of energy that causes them to react is called the activation energy - simply because it activates the reaction. There are many variables that need to be taken under consideration when measuring the rate of reaction. These can include catalysts, surface area, temperature or concentration of the liquid. In this case the dependant variable is the concentration of the liquid. These variables can either decrease or increase the rate of reaction. Theoretical Background When a reaction takes place it has to overcome a minimum energy barrier known as the Activation Energy. If the particles collide with less energy than the activation energy then nothing worth noting happens. "You won't get a reaction unless the particles collide with a certain minimum energy called the activation energy of the reaction." (Taken from www.chemguide.co.uk). Only those collisions, which have energies equal to or greater than the activation energy result in a reaction taking place. The reason why collisions have to overcome the
Rates of Reaction
Rates of Reaction Rates of Reaction Background information: Hydrogen Peroxide is a compound made of hydrogen and oxygen. The formula for hydrogen peroxide is H2O2. Concentrated hydrogen peroxide is a colourless, thick liquid which may blister the. To slow the decomposition of the peroxide into water and oxygen it is stored in dark bottles at a low temperature. It is a powerful bleaching agent and a good disinfectant. It is used to bleach hair, ivory, feathers, and delicate fabrics. Hydrogen peroxide always decomposes into water and oxygen gas: 2H2O2 › 2H2O + O2 The rate Hydrogen peroxide decomposes depends on the temperature and concentration. Hydrogen peroxide has many catalysts that make it decompose faster which include most of the transition metals and their compounds. The release of oxygen and energy of hydrogen peroxide as it decomposes can be dangerous. Spilling high concentration of Hydrogen peroxide on a flammable substance can cause an immediate fire. Factors: Concentration The concentration of a solution is how strong the solution is. If the concentration is increased, there are more particles in the same volume. This means there is a greater chance of them colliding, so the rate of reaction increases. In a low concentration, the number of collisions is low, so the rate of the reaction is slower. The concentration does not change the speed of the
Rates of Reaction
Science Course Work - How does the dilution of Hydrochloric acid affect the rate of reaction between itself and Sodium Thiosulphate? Aim: To see how changing the concentration of Hydrochloric Acid affects the rate of reaction. Prediction: In this experiment I predict that the more diluted the acid is, the longer it takes for it to react. For example, If 2 molar HCL added to X molar Na2S2O3 took 40sec to react, 1 molar HCL added to X molar Na2S2O3 will take 80sec to react. This is my prediction of the results table (not necessary the times, but the pattern of the times and rate) HCL(cm3) H20(cm3) Na2S2O3(cm3) Time (sec) Rate (sec) (1/X) (2mol/dm3) 25(from bottle A) 0 25 40 0.025 (1mol/dm3) 25(from bottle B) 0 25 80 0.0125 (0.5mol/dm3) 12.5(from bottle B) 2.5 25 60 0.00625 (0.25mol/dm3) 6.25(from bottle B) 8.75 25 320 0.003125 (0.125mol/dm3) 3.125(from bottle B) 21.875 25 640 0.0015625 I believe this will happen because each time the acid becomes more diluted, the amount of acid particles is halved. Therefore if there are half of the acid particles to react with, the time must be doubled because it will take twice as long for the Sodium Thiosulphate particles to collide with the Hydrochloric acid particles. Also the rate of reaction is halved each time, there for it will take double the time to react. Although the particles may hit each
rate of reaction
Rate of reaction The rate of reaction is how quickly a reaction takes place and the rate of the transformation of a product throughout a chemical reaction. The rate of reaction is measured by dividing 1 by the time taken for the reaction to take place. If a reaction has a low rate, that means the molecules unite at a slower speed, than a reaction with a high rate. Aim The aim is investigating the rate of reaction between Sodium Thiosulphate and Hydrochloric acid, and the effects of changing the concentration have on them. The equation for the reaction between Sodium Thiosulphate and Hydrochloric acid is: The sulphur created appears in the form of very small particles of solid. This leaves a white/yellow precipitate. Safety There are a lot of safety issues that we have to be careful with, as things are very unpredictable. It is important to wear goggles throughout this experiment, as it will protect the eyes. We must be careful with the chemicals, and not eat or drink in the science lab as we can get chemicals on to our hands. We should also dispose the mixture of chemicals of down a well-flushed sink. Equipment * Hydrochloric acid * Sodium thiosulphate * A paper with a black cross drawn on it * A conical flask * 2 measuring cylinders * 1 stopwatch * A pair of goggles Collision Theory The collision theory explains how a higher amount of collisions
Rate of Reaction Chemistry Coursework
The effect of temperature on rate of reaction Introduction Our investigation in rate of reaction involved us performing an experiment which involved us chemically reacting hydrochloric acid and magnesium. Different reactants cause different speeds and chemical reactions can vary from a small reaction to a large reaction. Reactions occur when particles of reactants collide together and react. The chemical reaction that we will be performing is: Magnesium+ Hydrochloric Acid› Magnesium Chloride+ Hydrogen Through this reaction I will be measuring the amount of hydrogen that is produced. I will have to choose certain apparatus and a certain method which I will test in preliminary and then perform in my method. Preliminary Investigations Variables Temperature- The higher the temperature, the faster the rate of reaction. This happens because at higher temperatures the particles have more energy meaning that they collide more with each other because the particles are moving around quicker. If you imagine a box of balls, if the balls have more energy they are moving faster and are more likely to bump into each other than balls with less energy and are moving slower. We can measure temperature in our experiment by heating the hydrochloric acid at different temperatures and measuring how much hydrogen is produced. This is the variable I will be changing and is going to be the
The Effect of Concentration on the Rate of Reaction between Hydrochloric Acid and Calcium Carbonate (marble) Chips.
CONTENTS PAGE PLANNING 2 INTRODUCTION 2 BACKGROUND KNOWLEDGE 2 The collision theory 2 Diagrams to show the particles reacting in a high concentration level and a low concentration level of hydrochloric acid 3 PREDICTION 5 THE EXPERIMENT 5 The outline of the plan 5 Measurments 6 Fair Test 6 Apparatus 7 Diagram to show the setup of appartus 7 Safety 7 Method 8 OBTAINING EVIDENCE 9 INTRODUCTION 9 Results Table 9 Tables to show the results obtained from the effects of different concentrations on marble chips on the varied rates of reaction. 9 Table of results to show the set of averages processed from each experiments concentration results. 10 Graph - Showing the rate of reaction from differnet concentrations 10 ANALYSING AND CONSIDERING EVIDENCE 11 The Effect of Concentration on the Rate of Reaction between Hydrochloric Acid and Calcium Carbonate (marble) Chips Planning Introduction This investigation is to obtain a set of reliable results and a strong conclusion, of the effects from different hydrochloric acid concentrations, reacting on small calcium carbonate chips; measuring the rate of reaction of which carbon dioxide is produced as a product. My primary aim is to find the change in reaction rate when the concentration is increased. Below is a balanced word and symbol equation of this reaction and its products, between hydrochloric acid and calcium
Investigation of the rate of reaction between Magnesium and Hydrochloric acid
Investigation of the rate of reaction between Magnesium and Hydrochloric acid By Hashim Al-Hasani 11R Introduction Chemical reactions occur when reactant particles collide with each other, Collision Theory If particles collide with less energy than the activation energy, they will not react. The particles would just crash into each other. The more regularly particles collide, and the greater the number of collisions with right amount of energy, the faster the rate (speed) of reaction. In this investigation I will be investigating the rate of reaction between a metal and acid. The rate of reaction is affected by numerous factors; these factors are: * Temperature * Surface area * Concentration * Use of Catalyst Temperature Temperature affects the rate of reaction because heat affects the movement of the particles; the higher the temperature, the faster the movement of the particles, therefore the faster the reaction. Surface Area Surface Area affects the rate of reaction because the bigger the area for the particles to react, more collisions occur, meaning the rate of reaction is greater. Concentration Concentration affects the rate of reaction because an increase in concentration means more particles to react with each other - therefore increasing the successful collisions between the particles and resulting in a higher rate of reaction. Use of Catalyst A
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The Effect of Concentration on the Rate of Reaction between Magnesium [Mg] and Hydrochloric acid [Hcl]
The Effect of Concentration on the Rate of Reaction between Magnesium [Mg] and Hydrochloric acid [Hcl] By Mohammed Thamid Azad Candidate Number- 5021 Centre Number- 13317 Rates of Reaction INTRODUCTION - This coursework will be investigating the effect of concentration on the rate of reaction between a metal-Magnesium [Mg] and Hydrochloric Acid [HCL]. Rate of reaction is the measurement of how quickly a reaction is progressing. It also includes how much products are being formed and what portion is being used up. Rate of reaction just means 'the speed of the reaction'. It is measured by the rate of formation of a product. When you are doing an experiment in order to make a product you should know how long the reaction takes to complete, before the product is produced. This coursework will be experimenting the reaction speed of Magnesium Metal with Hydrochloric acid. I will be observing 'the rate of reaction between Magnesium and Hydrochloric acid to measure how long a solution takes to react within different level of concentrations. 'In the experiments it is predicted that the reactions are not at a steady rate, meaning that they begin at a curtain speed then decrease until they stop which then decreases the concentration of reactants. AIM- To investigate the effect of concentration of acid on rate of reaction Mg(s) +2HCl (aq) --> MgCl2(aq) +H2(g)
An Experiment to Find the Amount of Heat Energy Released When 1g of Candle Wax Burns
An Experiment to Find the Amount of Heat Energy Released When 1g of Candle Wax Burns Aim The aim of this experiment is to discover how much energy is released when we burn 1g of candle wax. Method The best way to conduct this experiment is to use the candle as it burns, to heat up water. The reason for this is because we know water's 'specific heat capacity' is. A specific heat capacity is how much energy is required to raise the temperature of 1kg of a material by one degree Celsius. 4200 joules are required to raise 1kg of water by one degree Celsius. We will carry out the experiment in the following way: • Make sure we measure the mass of the water before the experiment (we can do this by measuring the beaker mass, and taking it away from the mass of the water AND the beaker mass) • Also make sure we know the mass of the candle (and its holder) • Then we need to take note of the initial temperature of the water with the thermometer • Set up the equipment as shown in the Diagram • Light the candle • Keep observing the thermometer readings until a significant gain in temperature is noticed and then take note of the mass of the candle and its holder in order to find out the mass of wax burned (by subtracting its mass after the experiment, by its mass beforehand) Before we undertake the experiment there are some points we must consider. First of all, an
