Science Rate Of Reaction
Aim: to investigate the effects of concentration, on the rate of reaction, between hydrochloric acid and sodium thiosulphate Scientific Knowledge: Sodium Hydrochloric Sodium sulphur water sulphur Thiosulphate acid chloride dioxide Na2s2o3 2hcl 2nocl s so2 h2o The collision theory believes that as the kinetic energy of particles increase so does the rate of reaction. Activation energy is the level of energy needed for a successful reaction to take place. For example the chemical reaction between methane and oxygen doesn't occur at room temperature but when heated they react. The reason for this is that some substances have extremely strong bonds which need more energy to break whilst others have weaker bonds which take less energy to collapse. The effects of surface area: The effects of concentration: The effects of temperature: 2mph 25mph In order to calculate the rate of reaction I will use this formula: 1 Average time When sodium thiosulphate solution reacts with hydrochloric acid a solid is formed. The time taken for a certain amount of sulphur to form can be used to indicate the rate of reaction. In this experiment the effects of the concentration of the sodium thiosulphate on the
Study on food colourings
Food colourings - Should they be used? Contents: Why use food colourings? 2 The two main types of food colourings 2 Health risks of artificial food colourings 3 Case Studies . Cancerous Colouring in Sausages 3 2. No more blue Smarties 4 3. Colourful curries 5 Hyperactivity in children 6 Should food colourings be used at all? 7 Conclusion 8 Bibliography 9 Why use food colourings? As there is doubt over what food colourings do to your health wouldn't you think people would just leave them out of food? Manufacturers still have many reasons to still put them in such as: * Offsetting colour loss due to light, air, extremes of temperature, moisture, and storage conditions. * Masking natural variations in colour. * Enhancing naturally occurring colours. * Providing identity to foods. * Protecting flavours and vitamins from damage by light. * Decorating purposes such as cake icing * Food that looks good will sell more The two main kinds of food colourings As well as artificial colourings you can get natural colourings which also work, these are things such as Caramel colouring which is used is cola products, which is found in caramelised sugar and Annatto which is made from the seed in a tropical tree and used to create a reddish orange dye for food. Also natural food colourings can be made from many plants other plants.
Rates of reaction between hydrochloric acid and magnesium
Introduction The question I am investigating is the rate of reaction when hydrochloric acid reacts with magnesium. Background The rate of a reaction can be measured by the rate at which a reactant is used up, or the rate at which a product is formed. In other words measuring how quickly a reaction is progressing. It involves measuring how much of the reactants are being used up or how much of the products are formed in a certain amount of time. Rate of Reaction = Change in amount of reactants/products Time taken The rate of reaction is measured by cm³/s (centimetres per second) or g/s (grams per second). Factors which affect the rate of reaction are temperature, surface area, catalysts and concentration. Factor How it affects the Rate of Reaction Temperature When the temperature increases the energy of the reactant particles rise. This leads to a large number of reactants having enough energy to react. The reactant particles will also move more quickly so the collision frequency increases. Surface Area If the surface area increases the rate of reaction also increases. When solid reactants (at least one reactant must be a solid) are involved, the reactions will only occur on the surface. Increasing the surface area of the solids means that more reactants are exposed and more successful collisions will happen in the same amount of time. Catalysts A Catalyst
Measuring the Rate of Reactions between Magnesium and Sulphic Acid
Measuring the Rate of Reactions between Magnesium and Sulphic Acid Aim: Investigating the effect of changing concentrations of H2SO4 (Sulphuric Acid) on reaction rates. Background Information: The formula for experimenting the change of reaction rates when concentration is varied is: Mg (s) + H2SO4 MgSO4 (aq) + H2 (g) When this reaction takes place, certain characteristics can be noticed. The reaction will cause fizzing and produces H2 (Hydrogen Gas), which can be identified by the white smoke given off when Magnesium is reacted with Sulphuric Acid. Magnesium is not the only element that could have been used to perform this reaction. Any of the following similar elements could have been used (in order of reactivity): Potassium Sodium Calcium Magnesium Iron Lead Gold This is just a selection of the elements available to complete this experiment, however, Magnesium was chosen because it is not too fast that it is difficult to record accurately when the gas is given off into the cylinder and also as it is not so reactive that it because a safety hazard. A less reactive element such as Lead or Gold was not used; as it would have made the experiment so slow that it would have taken hours to complete - a waste of scientists' time. Thus was Magnesium selected as a happy median. Reactions occur because of collisions between atoms. The faster the atoms move or the more
Rates of reaction throughout the year
Corroding Statue I am trying to find out if a statue made of magnesium corrodes at different rates through out the year. Scientific Knowledge: Some scientific knowledge, like the collision theory and information and equations on the origin of acid rain, will help me in my investigation. Useful definitions: Activation energy: this is the minimum energy that two particles must posses for a reaction to occur when they collide. Catalyst: A catalyst speeds up a reaction by reducing the activation energy. Collision Theory: For a reaction to occur, the reactant particles must collide with each other and with enough energy (activation energy). How different conditions affect the rate of reaction: Temperature- Low temperature High temperature -Low temperature- few collisions, low rate of reaction. -High temperature- more collisions, high rate of reaction. . Concentration- Low concentration High concentration -Low concentration: particles far apart, few collisions, low rate of reaction. -High concentration: particles more crowed more collisions high rate of reaction Surface area- Low surface area ............ High surface area
For my experiment I am finding out the effects on the reaction rate when magnesium is put into different concentrations of hydrochloric acid.
Chemistry coursework: Rate of reaction Introduction My investigation is about reaction rates and finding out what affects them and the correlation between reaction rates and the factors which affect them. Therefore in my experimentation I tried to find out the effects of concentration (the amount of a specific substance in a certain volume of space) on reaction rate. Rate of reaction is the rate or speed at which the chemical reaction (a reaction that changes one set of chemicals to another) takes place. For my experiment I am finding out the effects on the reaction rate when magnesium is put into different concentrations of hydrochloric acid. 2HCL (aq) + Mg (s) MgCl2 (aq) + H2 (g) Hydrochloric acid (HCl) Hydrochloric acid, also known as spirits of salt or muriatic acid is a solution of chlorine and hydrogen. It is a highly corrosive, strong mineral acid which has many uses in industries. It is a clear liquid so if it gets on your skin you will not notice it which means that it would start burning your skin and could get onto food as well. Therefore always wash your hands after handling hydrochloric acid. Collision theory Collision theory is simply understood as the higher the concentration of the reactants, the higher the reaction rate. The more reactants there are the more successful collisions there will be. This theory
How does varying the concentration in a reaction affect the rate of reaction?
How does varying the concentration in a reaction affect the rate of reaction? Introduction To investigate how concentration affects the rate of reaction, I shall be reacting magnesium with hydrochloric acid. I will keep the length and weight of the magnesium the same and will change the concentrations of the hydrochloric acid. Fair testing To make it a fair test, I will keep the length and weight of the magnesium the same at all times. I will change the concentrations of hydrochloric acid and I will measure the volume of hydrogen produced. At all times during the experiment, I will stop the stopwatch when the volume of hydrogen produced reaches 20cm3. Preliminary Experiments Experiment 1 An experiment was set up in which a 3cm strip of magnesium was reacted with 1M of hydrochloric acid. The aim was to set up the actual experiment and to time how long it would take for certain volumes of hydrogen to be produced from the reaction. This would mean I could make a decision on how I would conduct my own experiment. Firstly, the magnesium was placed inside the hydrochloric acid. The bung was closed and after every 5 cm3 of hydrogen produced, the time was recorded. These were the results obtained from the experiment: Volume of hydrogen produced / cm3 Time / s 0 0 5 7 0 0 5 3 20 6 25 9 30 22 35 34 45 36 As a result of the experiment, I have decided to stop
Investigating the Effect of Concentration on the Rate of Reaction between Hydrochloric Acid and Sodium Thiosulphate
Planning Section Investigating the Effect of Concentration on the Rate of Reaction between Hydrochloric Acid and Sodium Thiosulphate I think that the higher the concentration of the Sodium Thiosulphate, the faster the reaction will take place. The more water there is in the solution, the slower the rate of reaction will be. This is because the greater the concentration, the more reactant particles there are in that certain solution. There will be more successful collisions and therefore the rate of reaction is increased. Apparatus To successfully carry out this experiment, I will need the following apparatus: * Hydrochloric acid * Sodium Thiosulphate * Distilled water * A beaker * 2 measuring cylinders (one 50cm³ and the other 25cm³) * A piece of paper with an "X" on it * Safety goggles * 2 pipettes * Stopwatch * Calculator * Results table * Pencil Preliminary Experiment In order to see in what way to carry out the main experiment, I have carried out a preliminary experiment. I have only recorded two results. For the preliminary, I used 0.1M sodium Thiosulphate. Volume of Sodium Thiosulphate Volume of Distilled Water Volume of Hydrochloric Acid Time taken (seconds) 25cm³ 0cm³ 5cm³ 41 5cm³ 20cm³ 5cm³ 398 After doing the preliminary experiment, I decided to alter the main experiment for practicality reasons - using just 5cm³ of 0.1M
Formula of Magnesium Oxide
Chemistry Practical Assessment: Finding the formula of Magnesium Oxide (Skill 3) Results: Table showing measurements before experiment: Mass of crucible (g) Mass of lid (g) Mass of magnesium (g) Mass of crucible and magnesium (g) st try 4.21 1.91 0.9 5.11 2nd try 4.23 1.91 0.9 5.13 3rd try 4.21 1.92 0.8 5.11 Average 4.21 1.91 0.9 5.11 Table showing measurements after experiment: Mass of crucible (g) Mass of lid (g) Mass of contents (g) Mass of crucible and contents (g) st try 4.21 1.91 0.07 5.18 2nd try 4.23 1.91 0.06 5.19 3rd try 4.21 1.92 0.05 5.16 Average 4.21 1.91 0.06 5.18 Mass of products and reactants: ? mass of crucible: 14.21g ? mass of crucible and magnesium before heating: 15.11g ? mass of crucible and magnesium after heating: 15.18g ? mass of magnesium before heating: 0.90g ? mass of magnesium oxide: 0.97g ? mass of oxygen: 0.07g Changes occurring during the reaction: • Magnesium stripe glowed and burned bright orange • Sparks appeared on the surface of the magnesium stripe • Started to shrink and change into white powder form but still glowing This shows that magnesium has reacted with oxygen to form magnesium oxide, a white powder. Appearance of contents at the end of experiment: • White powder • Not in a shape of a coil Number of moles of magnesium and oxygen in magnesium oxide:
Reaction Rates Investigation
Reaction Rates Investigation In this experiment I will be investigating into how the change in concentration of acid can affect the rate of the chemical reaction. To keep the results precise, the variable I am changing will be the concentration of Hydrochloric acid but the volume of the solution, temperature of environment and the measured time will stay the same. But I will be considering changing the amount / surface area of Magnesium to help achieve the most precise and reliable results. I predict that the change in concentration of Hydrochloric Acid will notably affect the speed of the chemical reaction mainly due to my knowledge of Collision Theory which will be explained later in the investigation. Planning To decide on the best volume and concentration of hydrochloric acid and best mass of magnesium we first practiced a preliminary experiment. The equation for the reaction is: Magnesium(s) + Hydrochloric Acid(aq) - Magnesium Chloride(aq) + Hydrogen(g) Mg(s) + 2HCL(aq) = MgCl2(aq) + H2(g) We experimented first with different molarity of the Hydrochloric acid, the length of the magnesium ribbon strip etc. This will be explained more in the description of the Preliminary work. The reason we carried out a pilot experiment beforehand was to ensure reliability and accuracy for the final results. This will in turn provide a reliable conclusion for the original question
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