To work out the concentration of a substance from the heat energy of neutralisation.

To work out the concentration of a substance from the heat energy of neutralisation. In this test we are going to be putting alkali and acid together,We obviously know that it creates a reaction and when something reacts it creates heat.So I think that the results will be that with an equal amount of acids(25cm3) and alkali(25cm3)there will be the most heat rise.from this we can work out the concentration by the equation N=(hcl)= c x v 000 =2 x V (v will come from the graph) 000 = N x 1000 C By predicting myself now what will happen without using the equation-The biggest reaction will come from the acid and alkali with equal amounts which will produce the most heat Safety: The experiment will include a Bunsen burner which can obviously burn and particularly strong acid and alkali which can burn especially the acis,Alkali can irritate the skin.The first thing to put on should be the goggles as our eyes are then protected before we even come into contact with the acid etc. Bags should be placed under the tables out of anyone's way so no one trips up and all loose clothing to be removed or tied back e.g. Hair.During the experiment These things are going to be/should be in use -A Bunsen burner 5-polysteriene cups(to hold acid and alkali when reacting) 2-heat proof mat 6-Buret 3-tongs 7.goggles(to protect eyes) 4-glass beakers Variables: There are

  • Word count: 1268
  • Level: GCSE
  • Subject: Science
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Concnetraion Hydorchloric Acid

How does changing the Concentration of Hydrochloric Acid Affect the Rate of Reaction between Hydrochloric Acid and Magnesium? Dependent Variable Volume of Hydrogen Produced - the volume of hydrogen produced in cm3 will be affected by the independent variable which in this case is the concentration of the hydrochloric acid. There is no way in which the volume of hydrogen produced can be controlled however make sure none is lost by making sure that the gas syringe is correctly connected. Measurements will be taken every 30 seconds for the volume of hydrogen produced for 5 minutes. Independent Variable Concentration - the variable which will be controlled is the concentration of the hydrochloric acid. The concentrations which will be used are 2M, 1.8M, 1.6M, 1.4M, 1.2M, 1.0M, 0.8M, 0.6M, 0.4M and 0.2M. The concentrations will be changed by using different measurements of hydrochloric acid and water. Controlled Variable The equation for the reaction can be seen below; Mg(s) + 2HCl(aq) --> MgCl2(aq) + H2(g) I will be controlling many of the variable which affect the volume of hydrogen which is produced. Temperature - The temperature will be controlled because if the temperature was to be changed this could affect the dependent variable. To control this the experiment shall be done in the same lab with no heating and no cooling will be done while the temperature will also

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  • Level: GCSE
  • Subject: Science
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Halogen element - Production and use

from halogen element Production and use Rock salt deposits are usually mined; occasionally water is pumped down and brine, containing about 25 percent sodium chloride, is brought to the surface. When the brine is evaporated, impurities separate first and can be removed. In warm climates salt is obtained by evaporation of shallow seawater by the sun, to give bay salt. Chlorine is produced on a large scale by any of a number of different methods: . By electrolysis of a concentrated solution of sodium chloride in water. Hydrogen is evolved at the cathode, and chlorine at the anode. At the same time, an alkali metal hydroxide is produced in the electrolyte, and hence this process is often referred to as chlorine-alkali-electrolysis. The chemical reactions that take place at each electrode and the overall cell process are given in the following equations: in which the symbol e- represents a single electron. In the reaction vessel, free chlorine and hydroxide ions must not come in contact with each other, because chlorine would be consumed according to the reaction To accomplish the separation of chlorine gas and the hydroxide ion, a porous wall is inserted between the electrodes (diaphragm process), or the iron cathode is replaced by a cathode consisting of liquid mercury (mercury cathode process) which avoids the production of hydroxide ions at the electrode. Instead, free

  • Word count: 1240
  • Level: GCSE
  • Subject: Science
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To Determine The Concentration Of A Limewater Solution

To Determine The Concentration Of A Limewater Solution. Aim: To determine the concentration of a limewater solution using hydrochloric acid of a known concentration of 2.00 moldm-3. Ca(OH)2(aq) + 2HCl(aq) --> CaCl2(aq) + 2H2O(l) This shows that the reactants react in a 1:2 ratio. This will be carried out using a titration. However, as the concentration of the calcium hydroxide in the limewater is approximately 1g dm-3 and the concentration of the hydrochloric acid is 2.00moldm-3 the concentration of the hydrochloric acid needs to be reduced. This can be done by a dilution. To make the colour change in the titration distinct and so you know straight away when the solution has been neutralised phenolphthalein indicator will be used, as suggested in Understanding Chemistry. Safety: HCl is high in concentration and so could be irritant. Lab coat and safety goggles must be worn. Apparatus List: For dilution: * Graduated pipette (5cm-3) * 250cm3 volumetric flask. * Distilled Water. * HCl solution. For titration: * Graduated Pipette (25cm3) * Burette, Stand and Clamp * Funnel * Beaker containing 0.02moldm-3 HCl solution. * Beaker containing limewater of unknown concentration. * Conical Flask * Phenolphthalein Indicator & White Tile Preparations: To work out the number of moles we can use the 'n=m/M' equation. Concentration of Ca(OH)2(aq). g dm-3

  • Word count: 722
  • Level: GCSE
  • Subject: Science
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To investigate how varying the temperature of the reaction between amylase and starch affects the rate of reaction.

An experiment to investigate the effect of temperature In the reaction between amylase and starch Aim To investigate how varying the temperature of the reaction between amylase and starch affects the rate of reaction. Prediction I predict that as the temperature of the reaction increases, so will the rate of chemical reaction. Scientific knowledge: As the temperature increases, the particles will have more energy to move around faster, resulting in more collisions which will lead to chemical reactions. This is linked to the collision theory, and as the temperature increases in this experiment, more collisions will occur between the amylase and starch, which should result in more starch being broken down into glucose. Method I will be heating up the starch and amylase separately to the first chosen temperature in a water bath so that the test tube is not directly heated. I will heat them with a Bunsen burner and check the temperature with a thermometer. When at the desired temperature the amylase and starch will be mixed and a stop-clock will be started. A sample of the mixture will be taken after every 30 seconds. Each sample will be mixed with a small amount of iodine on a spotted tile to see what colour the iodine changes to. I will then be able to determine how fast the amylase is breaking down the starch at that temperature. This will be performed at each

  • Word count: 777
  • Level: GCSE
  • Subject: Science
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Investigation to find the effects of different concentrations of sodium thiosulphate mixed with hydrochloric acid. We wanted to find a precise set of results so we used a laptop computer to record the experiment.

AIM 2: For this experiment we had the same aim as the first experiment (i.e. to find the effects of different concentrations of sodium thiosulphate mixed with hydrochloric acid). Although this time we wanted to find a more precise set of results so we used a laptop computer to record the experiment. APPARATUS: The apparatus used included: a flask, a measuring cylinder, an empty flask lined with black paper, a laptop computer and a sensor lamp. METHOD 2: We put sodium thiosulphate into the flask and some dilute sulphuric acid into the cylinder; water was also prepared so that it could be used to mix with the sodium thiosulphate. In addition to this the laptop computer was connected to the sensor lamp, which pointed into the empty flask lined with black paper. For the first experiment we added the two liquids and then began the program on the laptop. This program is used to record the time taken for the mixture to turn opaque in 2 minutes. When the lamp's light is cut off from the sensor, it means the reaction has finished. For the second experiment, instead of pure sodium thiosulphate being added to the hydrochloric acid, some of it was replaced by water. In this way the experiment shows how long it takes for the reaction to take place using different concentrations of sodium thiosulphate. Five experiments were intended to be performed in total (although we only managed to

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  • Level: GCSE
  • Subject: Science
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investigate the effects of temperature on the reaction between sodium thiosulphate and hydrochloric acid.

Science Coursework: Rates of Reaction Skill section P Aim: To investigate the effects of temperature on the reaction between sodium thiosulphate and hydrochloric acid. Scientific Knowledge: Reaction: When atoms or groups of atoms re-arrange resulting in the change of molecular structure in substances, is only possible when the particles collide with the other reactants with enough energy to form the transition state and change it into other products. Without such circumstances reaction will not be possible. This is collision theory. The factors that affect the rate of reaction are: - Temperature - Pressure - Size of surface area in which reaction will take place - The concentration of reactants The reaction will take effect faster if any of these are increased. That is all because of collision theory. Reactants also need to have sufficient energy, activation energy, to react. If increasing temperature, the reactants will vibrate more making it more likely for them to collide and collide harder as they have more energy, meaning that they will have the activation energy to make reaction more likely. If pressure is high then there is more chance for the reactants to collide as they will be closer to each other. If surface area is increased then more reactants can collide with each other as there is more space for collision. When there is a higher concentration of

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  • Level: GCSE
  • Subject: Science
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How does the concentration of the reactants affect the rate of reaction when sodium thiosulphate and hydrochloric acid are combined?

How does the concentration of the reactants affect the rate of reaction when sodium thiosulphate and hydrochloric acid are combined? Introduction: A chemical reaction is a process in which one set of chemical substances, known as the reactants, are changed into another substance or set of substances, called the products. The factors that affect the rate of chemical reactions include: * Particle size. * The use of a catalyst * Concentration. * Pressure. * Temperature. For my investigation I have chosen to analyse the way in which the rate of reaction is altered by the concentration of the reactants. When the reactants, sodium thiosulphate and hydrochloric acid, are combined they produce 4 different products as shown in the following equation: Sodium Thiosulphate + Hydrochloric Acid --> Sodium + Water + Sulphur + Sulphur Chloride Dioxide Na2S2O3 (aq) + 2HCl (aq) --> 2NaCl (aq) + H2O (l) + SO2 (g) + S (s) In my experiment I intend to change the concentration of the sodium thiosulphate and measure the effect this has on the rate of the reaction. The rate will be indicated by how much light is obscured by the precipitated sulphur at certain time intervals. The actual time taken for the reaction is measured by the time taken for the sulphur to be precipitated. The sulphur becomes a milky yellow colour, which obscures a cross, drawn

  • Word count: 3034
  • Level: GCSE
  • Subject: Science
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To Show How the Volume of Fuel Affects the Energy Output In the Form of Heat

Investigation To Show How The Volume Of Fuel Affects The Energy Output In The Form Of Heat Prediction The choice of variables are as follows volume/mass of fuel, volume of water, distance from can & burning time. I chose volume/mass of fuel. I predict that the larger the volume/mass of fuel the more energy will be released. I believe this because if you have a larger volume/mass of fuel it will contain more bonds than a smaller volume/mass and so will have the potential to give off more energy when bonds are formed. This is backed up by the fact that atoms have a mass, and so when there is a larger mass it obviously means there is more atoms and where there is atoms there is bonds to hold the atoms together to form a compound. Thus having more atoms(weight) means there is more bonds(energy potential) to form and give off energy. Ethanol Bond Values H H C? C ?347j x 1=347j ? ? C? H ?413j x 5=2065j H? O ? C? C ? H C? O ?358j x 1=358j * ? O ? H ?464j x 1=464j H H 347+2065+358+464=3234 joules So 1 molecule of ethanol has the potential bond energy of 3234joules. The equation for this experiment is as follows:- CH3CH2OH + 3O2 ??Combustion??? 3H2O + 2CO2 Ethanol + Oxygen

  • Word count: 1286
  • Level: GCSE
  • Subject: Science
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The aim of this investigation is to study how temperature would affect the rate of reaction.

EFFECT OF TEMPERATURE ON THE RATE OF REACTION. AIM: The aim of this investigation is to study how temperature would affect the rate of reaction. PREDICTION: The rate of a chemical reaction is the speed at which it takes place. Temperature is a major factor in this as increasing or decreasing the temperature changes the movement of particles in a substance therefore changing the rate of reaction. When a reaction mixture is heated up, each particle in it acquires more energy and collides more with other particles. I have shown below what the particles state would be when either hot or cold. I predict that if you increase the temperature of a particular reaction, you increase the speed at which it takes place. This is simply because the particles carry more energy and collide more often thus speeding up the reaction time. Particles, when moving faster, collide with greater power. The reaction therefore becomes faster. Collisions between particles are useless unless they break the energy barrier and this is exactly what increasing the temperature will allow them to do. I also predict that my graphs will look like the ones shown below. METHOD: The formula I will use in this investigation is: Sodium Thiosulphate+ Hydrochloric Acid> Sodium Chloride+ Sulphur Dioxide+ Sulphur+ Water (Na S O (aq)

  • Word count: 1287
  • Level: GCSE
  • Subject: Science
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