Investigating the rate of reaction between magnesium and hydrochloric acid.
Investigating the rate of reaction between magnesium and hydrochloric acid Aim In this experiment I aim to investigate the rate of reaction between magnesium and hydrochloric acid. This reaction rate will be affected by different variables, which can be changed; these are Temperature of the hydrochloric acid, mass of magnesium and concentration of the hydrochloric acid. Others things can effect the reaction rate but these are the main variables. In this experiment I will only alter one of the variables and keep the rest at a constant rate. For this experiment I will concentrate on the concentration of the hydrochloric acid and see what the effects are on the rate of reaction when this is altered. Prediction I predict that the higher the concentration of the acid the quicker the reaction time I no this because, "rate plus concentration are directly related" (Salter's A-level chemistry second edition chapter 10). This tells me that the concentration will directly affect the rate of reaction. To back this prediction up I have to look at the collision theory, this states that for the two different reactants to react the particles of each have to collide and hit each other hard enough so that it is possible to create enough energy for the to particles to break or form new bonds with the other particles this is called a successful collision. When there is not enough energy for the
Investigating the Rate of Reaction Between Sodium Thiosulphate and Hydrochloric Acid
Investigating the rate of reaction between Sodium Thiosulphate and Hydrochloric Acid Aim: an experiment to find out how the rate of reaction changes with differing concentration of Sodium Thiosulphate (Na S O), Hydrochloric Acid (HCL) and water (H²O). Prediction : I predict that the rate of reaction will increase (and get more cloudy, more quickly) when the solution of Sodium Thiosulphate and Hydrochloric Acid are strongest, and there is no water. The reason for this is that it will be easier for the Sodium Thiosulphate to react with the Hydrochloric Acid, as they are the only two chemicals in the beaker, and there is not water to hinder the rate of the reaction. There will also be more Sodium Thiosulphate to react with the Hydrochloric Acid, regardless of how much water there is. For a reaction to take place there has to be a collision with two different chemical particles. If the concentration of the hydrochloric acid was to be high the more acid particles there would be. The more acid particles there are the more likely of a collision to occur. By adding to water to the hydrochloric acid would make the acid less concentrated, meaning there would be less acid particles and also a less likely of that a sodium thiosulphate would collide into acid particle. Equipment : Beakers, Measuring cylinders Blank piece of paper with a cross Stop watch Sodium Thiosulphate
Titration Experiment
Titration practical Introduction In this practical I will be using a form of quantitative analysis called titration. Titrations are often used for neutralisation reactions. I will be carrying out the practical safely and following all the precautions in the risk assessment. Materials Burette Conical flask Pipette Sodium hydroxide solution Distilled water Bromothymol blue indicator Clamp stand Hydrochloric acid Funnel Risk assessment Risk Danger Precaution Action Clamp stand could break Could cause cuts Handle carefully and at all time and secure properly Tell the teacher immediately Acid is corrosive Could harm or damage skin Handle carefully at all times Tell teacher immediately and wash off with water Method . First I washed out a 25 cm3 graduated pipette with sodium hydroxide solution. (0.1-mol dm3) 2. I used the pipette to measure out 25 cm3 of sodium hydroxide solution using a graduated pipette (with pipette filler) into a 250 cm3 conical flask that has been washed with distilled water. 3. I added 3-4 drops of bromothymol blue indicator 4. I secured the burette in a clamp and stand and washed a burette twice with a few cm3 of hydrochloric acid (0.1 mol dm cubed). The concentration was to be checked. 5. I carefully poured in the 0.1 mol dm3 of hydrochloric acid. (Caution: I brought the burette down to my eye level and used a filter funnel
To find if changing the concentration of an acid will increase or decrease the rate of the reaction when marble is dissolved in hydrochloric acid.
PLANNING Aim To find if changing the concentration of an acid will increase or decrease the rate of the reaction when marble is dissolved in hydrochloric acid. Equipment I will be using the following apparatus, One conical flask to put the marble chips in and also to put the acid in so they react. . A piece of delivery tube, this carries the gas to the measuring cylinder this also has a stopper on the end to go on the top of the conical flask to stop the gas escaping. Two measuring cylinders, one to measure the amount of acid and one for the amount of water to make my acid concentrations, so that I don't make mistakes when measuring just in case I out both liquids in the same test tube and have to much then have to pour away it would not be a fair test One clamp One clamp stand Thermometer 5 sets of 3grams of marble chips 2 Molar Hydrochloric acid Water Gas Syringe Stopwatch Method Since I will be working with strong acid, I will wear safety goggles while conducting the experiment. I will use Marble chips all of which will be weighed for 3g for each different concentration. The amount of acid concentration I have decided on is 50cm3 I will firstly select the first concentration of acid, which will be the lowest concentration solution, which is 40cm3 acid and 10cm3 water and measure that out. Place the marble chips in the flask and then as quickly as
Which equation is correct?
Which equation is correct? Aim Copper has two oxides, Cu2O and CuO. Copper carbonate, CuCO3 decomposes on heating to form one of these oxides and an equation can be written for each possible reaction: Equation 1: 2CuCO3(s) Cu2O(s) + 2CO2(g) + 0.5O2(g) Equation 2: CuCO3(s) CuO(s) + CO2(g) Using ideas that I have learnt about the mole, I will plan and design an experiment to measure a volume of gas that will prove which of the two equations is correct. Background Information Cu2O is known as cuprous oxide. It is a red crystalline material, which can be produced by electrolytic or furnace methods. CuO is cupric oxide. This, a black powder, can be prepared by the ignition of suitable salts such as the carbonate, the hydroxide, or the nitrate of copper, or by heating of cuprous oxide. The planning of this experiment requires previous knowledge about the mole. One mole of any substance, be it element or molecular compound, contains Avogadro's number of atoms. Avogadro's number is a constant, L, and is approximately 6.023 x 1023 mol-1. At room temperature and pressure, all gases occupy that same volume. One mole of any gas will occupy a volume of 24dm3. This information is useful for working out what amount of copper carbonate should be decomposed. Another important equation will be required in order to do this: Moles = Mass / Mr Therefore:
Which Equation is correct?
Chris Ellison Which Equation is correct? Introduction Copper has two oxides, Cu2O and CuO. When heated Copper carbonate, CuCO3 decomposes to form into one of these two oxides. An equation can be written for both- Equation 1: 2CuCO3(s)› Cu2O(s) + 2CO2(G) + 1/2O2(g) Equation 2: CuCO3(s) › CuO(s) + CO2(g) To find out which equation is correct we need to find out how many moles of CO2 and O2 are produced by one mole of CuCO3. Equation 1 g of CuCo3 will produce 247.2cm3 of gas. Number of moles = Mass Mr 1 124 = 0.0081 moles of CO2 0.0081 = 0.0020 moles of O2 4 = 0.0103 moles of gas produced for 1g of CuCO3. 0.0103 x 24000 = 247.2cm3 Equation 2 g of CuCO3 will produce 194.4cm3 of gas. 0.0081 moles of Co2. 0.0081 x 24000 = 194.4cm3 Using this we can find out which equation is correct by the amount of gas produced. Apparatus Conical Flask Rubber Tubing Rubber Bung Clamp Stand Clamp Gauze Water Bowl Bees Hive Measuring Cylinder (500cm3) Heat Proof Mat Bunsen Burner Copper Carbonate (At least 4g) Stop Watch Diagram Variables and Fair Test In this experiment I want to keep everything the same so I don't get anomalous results. The Copper Carbonate will need to be heated so the gas given off will also be hot, because of this the gas will need to be left to cool before being recorded. When weighing the copper carbonate first zero the scales
What affects the rate of reaction between Sodium thiosulphate and Hydrochloric acid?
What affects the rate of reaction between Sodium thiosulphate and Hydrochloric acid? Prediction I predict that the more concentrated the acid the faster the rate of reaction. Theory to back up my prediction Particle theory tells us that the more particles the more frequent successful collisions there will be. When the concentration of the acid is increased the rate of reaction increases because of more successful collisions. Low concentrated acid High concentrated acid Variables: Catalyst Concentration Temperature Plan In this experiment I am going to investigate what affects the rate of reaction between sodium thiosulphate and hydrochloric acid. A chemical reaction can only happen if the molecules frequently and successfully collide into each other. These molecules have to hit each other in the right direction and at the right speed and with the right amount of energy. Apparatus * 500ml Beaker * Stopwatch-- So I can accurately time the rate of a reaction to 1/100th of a second. * Measuring Cylinder-with accurate scale, there needs to be two different cylinders because if you measure both of the solutions in the same cylinder it might contaminate it. What will I keep constant? * The volume of sodium thiosulphate * Use the same 250ml beaker What I will vary? * I will vary the concentration of hydrochloric acid. (by adding the correct amount
Volumetric analysis
Volumetric analysis Volumetric analysis is the measurement (in volumes) of solutions by titration experiments. Thus via the titration method we are able to determine the concentration of a substance in a given solution. Volumetric analysis is very important as with medicines, it is very important to know the concentration of the medicine in order to make sure the required dosage is being used and to limit the chances of overdoes. Volumetric analysis also helps us determine factors such as the amount of carbon dioxide in soft drinks and the amount of alkali in a cleaning solution, or even the amount of acid in a bottle of vinegar. Materials and Apparatus: * Burette * 25cm³ pipette * Retort stand * Clamp * Conical flask * Pipette filler * Phenolphthalein * Sulphuric acid * 25cm³ of 0.1 ml/dm³ Sodium hydroxide Procedure: . Wash all equipment 3 times with distilled water 2. Rinse the burette with a little of the acid and then fill it up 3. Rinse the pipette with a little of the base before accurately transferring 25.0cm³ of it to a titration flask. 4. Place 2 to 3 drops of an appropriate indicator in the flask and titrate rapidly, until the end-point is reached 5. repeat experiment 2-3 times until you obtain precise results Precautions * Avoid parallax error when taking readings, by placing eyes perpendicular to the scale. * In order to get accurate
Volumetric Analysis
Volumetric Analysis Aim The aim of this investigation is to find the various measurements of concentration (Also called the morality) of acid that will neutralise 1 mole of sodium hydroxide. This is found using the titration method. Prediction I predict that the volume of acid that will be used to neutralise the given solution would depend on the concentration. The more acid I add to an alkali, the more neutral it will become. If I add too much acid, the solution will not neutralise, so therefor it will turn to an acidic solution. This happens in all scientific experiments. Apparatus x conical flask x burette x clamp stand x 50ml bottle of universal indicator (any amount as long as it can do 40 drops) x solution 1 - HCI (Hydrochloric acid) x solution 2 - H2SO4 (Sulphuric acid) x solution 3 - HNO3 (Nitric acid) x White tile x measuring cylinder x funnel x safety glasses Diagram Safety with apparatus * Do not shake the conical flask too vigorously or the solution will spill. * Always be prepared for a spill. * Make sure that the burette is closed when not in use. * Do not fill the burette right to the top. * Make sure the clamp stand is held tightly by your partner. * Make sure the burette is held tightly by the clamp stand. * Make sure the solution are put in a safe place and is not put on the edge of the table. * Make sure every solution, liquid, etc,
What factors affect the rate of reaction?
What factors affect the rate of reaction? By Alex Willmott I am trying to find out what factors affect the rate of reaction. Here are the four things that affect the rate of reactions under normal circumstances: * Concentration * Catalysts * Temperature * Surface Area In this experiment we will be looking at how concentration affects the rate of reaction. Here is the word equation for our experiment: Magnesium + Sulphuric Acid Hydrogen + Magnesium Sulphate Mg(s) + H SO H (g) + MgSO Prediction In my experiment I expect that when I increase the amount of acid the reaction will occur faster. Increasing the amount of acid is increasing the concentration, which I think will speed up the reaction. If I dilute the sulphuric acid by adding water then the rate of reaction will slow down because of decreased concentration. This will all happen because of something called 'The Collision Theory'. The particles in a liquid move continuously, so this causes collisions. So if the collisions have enough energy a reaction will take place, but if there is not enough energy no reaction occurs. This is where the factors I mentioned come into play; for example if there is more particles a reaction is less likely to occur, this is when surface area is involved. When temperatures are higher the particles move around more quickly resulting in more reactions, faster. So if a
