How Much Does Limestone React With Hydrochloric Acid?
How Much Does Limestone React With Hydrochloric Acid? Planning the experiment. This experiment will show how much limestone fizzes when added to hydrochloric acid. I will gather the gas released from the fizzing and measure how long it takes to gather a certain amount of gas. The light blue area represents the hydrochloric acid, and the white blobs are the limestone. The grey area is the carbon dioxide released from the HCl and CaCO3 reaction, heading in the direction indicated by the arrows. The dark blue areas are water. Using this equipment, I will conduct 5 tests, each one with the same equipment, the same mass of limestone, the same volume of acid, but in each test the acid will be a different strength. This keeps it all a fair test. The 5 acid strengths will be 0.5M, 0.75M, 1.0M, 1.5M, and 2.0M. I will conduct each test twice, so as to obtain two sets of results for each acid strength. This will enable me to take averages. This idea of taking averages will account for any slight mishaps in the tests, for example, different air temperatures can affect how quickly the reaction between the CaCO3 and the HCl takes place. I predict that the stronger the acid is, and the warmer the air is, the faster the limestone will react with the hydrochloric acid. This prediction is based mainly upon the collision theory, for this states that as substances heat up, the molecules
To devise an experiment to determine which group or class of metal oxides are the more efficient catalysts when inserted into hydrogen peroxide.
Chemistry AIM: To devise an experiment to determine which group or class of metal oxides are the more efficient catalysts when inserted into hydrogen peroxide. Introduction Hydrogen Peroxide Hydrogen Peroxide is a chemical compound of hydrogen and oxygen. Its scientific formula is H2O2. If this solution has not been altered and is pure and anhydrous, it is colourless, slightly thick and has a gravity of 1.44. Although I do not think anyone would taste it, hydrogen peroxide has a metallic taste and will blister the skin. Concentrated solutions are unstable, and, if the liquid is still pure, it can explode when heated above a temperature over 100°C. Concentrations of hydrogen peroxide higher than 50 per cent can cause serious burns. Such factors as light, heat, chemical catalysts, dirt, and rust may cause hydrogen peroxide to decompose into water, oxygen, and heat. It is soluble in water. To keep hydrogen peroxide from decomposing, it is kept in dark bottles and at low temperatures. Hydrogen peroxide is widely used in industry. It is manufactured in huge quantities by the electrolysis of aqueous solutions of sulfuric acid or of potassium bisulfate or ammonium bisulphate. Solutions containing 3 to 6 per cent hydrogen peroxide are used as antiseptics and germicides and as a skin cleanser. Higher concentrations are used in the manufacture of many chemical compounds. They also
Group 4 Project - Camembert
Group 4 Project - Camembert by Tiphanie Bedas, Annemarie Desloges, Romain Hottlet, Nathalie Nadeau For the Group 4 project of June 2001, the students of EABJM in Paris have chosen of common agreement CHEESE. Our specific group have chosen to study the chemical aspects of Camembert. Camembert is famous French cheese. Made form unpasteurized milk, this cheese known since WWI has more then 45% of fat. However, Camembert contains many other things. By cliking on each link one can find the experiments on the following components of cheese: * Water content * Organic and inorganic content * Ionic content * Energy content Make a link for conclusion As can be seen in the pie, Camembert is a very good source of energy and water (2 & 3). It is not however a good source of minerals (1). Finding the water content in Camembert: Materials: a slice of Camembert, a plate, oven, balance Method: . Heat the oven to 50 oC. 2. Zero the balance and then weigh the plate. Note its weight. Then add the piece of cheese with the plate. Find the mass of cheese by subtraction. 3. Leave the plate with the cheese in the oven for a week. 4. Weigh the plate with the cheese and calculate the mass lost. This is the mass of water than has so far been lost. 5. Leave the cheese again in the oven for a week and weigh it once more, calculating the mass that has been lost. 6. Repeat until
Determine the Decomposition of Copper Carbonate
Planning Introduction I'm going to produce a piece of coursework, which determine the Decomposition of Copper Carbonate The purpose of decomposing CuCO3 is to determine the volume of CO2 gas that evolves. In this experiment, the water displacement method is used to recover the gas evolved. The volume of CO2 collected is converted to dry conditions, which is then compared to the theoretical volume calculated. As copper has two oxides Cu2O and CuO, when 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) + 1/2O2 Equation 2: CuCO3(s) --------->CuO(s) + CO2 (g) My aim is to find out which of these equations is correct. Hypothesis I predict that the CuO compound will be formed, because this is in line with the pilot results, and would be supported by the background theory. Copper most commonly forms compounds as a divalent ion, so I think that the thermal decomposition will be no exception and the oxide will be CuO. The kinetic stability and the stability of CuO with respect to Cu2O could account for the fact that Cu2O is energetically more stable with respect to its elements. Instructions Develop a table to record the various measurements. Write a balanced equation for the decomposition reaction. Determine the number of moles of the
Determine the equilibrium constant - Kc; of ethanoic acid reacting with ethanol producing an equilibrium to form ethyl ethanoate and water.
The Determination of an Equilibrium Constant Determine the equilibrium constant - Kc; of ethanoic acid reacting with ethanol producing an equilibrium to form ethyl ethanoate and water. CH3COOH(aq) + C2H5OH(aq) <=> CH3COOC2H5(aq) + H2O(l) Following the method as detailed, I conducted experiment 4 and these results were obtained: Titration Trial Volume of Sodium Hydroxide Neutralised (cm3) 7.65 2 7.75 3 7.80 4 7.70 5 7.75 µ 7.75 To calculate Kc, the concentrations of each reactant must be calculated from the point of equilibrium at which the titration was taken. Therefore, using 7.75cm3 as the average titre, Moles = 0.2M x (7.75cm3 / 1000 cm3) = 1.55 x 10-3. However, this represents the total amount of acid in the system which included ethanoic acid but also the acid catalyst: hydrochloric acid. Therefore this must be taken away from the number of moles of acid to calculate number of moles of ethanoic acid. Since 25 cm3 of 1.0M HCl was included in the initial 250 cm3 mixture, Moles = 1 x (25 / 250) = 0.1 moles. But 1cm3 samples were taken at a time, therefore: Moles = 0.1 x (1 cm3 / 1000 cm3) = 1 x 10-4. Taking this away from the total amount of acid = 1.55 x 10-3 - 0.1 x 10-3 = 1.45 x 10-3 (moles of ethanoic acid). Considering the stoichiometry of the equation, there is equal amounts of ethanol as there is ethanoic acid, therefore there is 1.45 x
Experiment: To determine the correct equation for the decomposition
Experiment: To determine the correct equation for the decomposition of copper carbonate Introduction and background information: Important points to note: 'At room temperature, 25°C and atmospheric pressure at 1 atmosphere, I mole of any gas will occupy a volume of 24 dm³.' We will need this to work out how much copper carbonate to decompose to obtain a sufficient amount of carbon dioxide gas. To work out the amount of copper carbonate to use I will need to use the following equations: Number of moles = Mass / Mr PV = nRT P = Pressure V = Volume n = Number of moles R = Gas constant T = Temperature We can substitute n (number of moles) with the first equation to get: PV = (mass/Mr) x RT When rearranged this gives: Mass = (Mr x PV) / RT This will allow me to work out the mass needed. Aim: The aim of this experiment is to determine which of the following equations is correct: Equation 1: 2CuCO3 (s) Cu2O (s) + 2CO2 (g) + 1/2 O2 (g) Equation 2: CuCO3 (s) CuO (s) + CO2 (g) I will do this by decomposing the copper carbonate. I will need to calculate if the volume of carbon dioxide produced is equal to what the equation suggests. Equipment: * Heatproof mat * Bunsen burner * Boiling tube * Bung * Delivery tube * Water bath * Measuring cylinder (250 cm³) * Digital weighing scales * Spatula * Clamp and stand * One molar copper carbonate
In this experiment you will prepare a complex compound of iron, potassium trioxalatoferrate(III), K3Fe(C2O4)3. In this compound each oxalate ligand has two bonds to the iron(III) ion
Preparation of an iron complex Chemicals: Iron(II) ammonium sulphate, FeSO4 ? (NH4)2SO4 ?6H2O, (7.5g) Oxalic acid (10 g in 100 cm3 water), (45 cm3) Potassium oxalate, (5 g in 15 cm3 water) H2O2 (1.8 M), (12.5 cm3) Ethanol. (25 cm3) Apparatus: Burette, Funnel, Filter paper, Burner, Thermometer. Principle: In this experiment you will prepare a complex compound of iron, potassium trioxalatoferrate(III), K3Fe(C2O4)3. In this compound each oxalate ligand has two bonds to the iron(III) ion, and hence this compound is an example of a chelate. You will aim at obtaining the maximum yield of product of the highest purity permitted by this method. Your final product should be in the form of bright green crystals. The compound will be prepared by first preparing iron(II) oxalate, FeC2O4?2H2O, and then oxidizing this with hydrogen peroxide, in the presence of potassium oxalate, to convet it to the ferric-oxalate ion, Fe(C2O4)33-. C2O42- H2O2, K2C2O4 H2C2O4 Fe2+ ?????? FeC2O4 ?2H2O ?????? Fe(OH)3 ?????? K3Fe(C2O4)3 ?3H2O 2H2O + K3Fe(C2O4)3 Thus all the iron in the iron(II) ammonium sulphate is converted to ferrioxalate, one third of the ferrioxalate being formed from the iron(III) hydroxide. Both H2O2 and Fe(OH)3 are unstable to heat. Potassium trioxalatoferrate(III) is photosensitive, i.e. it decomposes when exposed to
Determining the iron content in a sample of steel wool.
Determining the iron content in a sample of steel wool Natalie Loo 12A Aim: To find the percentage of iron in a sample of steel wool. Method: . Weigh accurately about 1g of steel wool and add enough dilute sulphuric acid to cover it in a conical flask. Heat the flask gently until the reaction starts. 2. When all the steel wool has dissolved, filter the solution and the washings from the flask into a beaker. 3. Make the solution up to 250ml in a volumetric flask with boiled, cooled distilled water, washing the beaker out with boiled distilled water twice. 4. Calculate the mass of KmnO4 needed to make up 500ml of 0.02M solution. 5. Weigh out approximately this mass of solid KmnO4 and dissolve in 500ml of water in a 1L beaker. 6. Cover the beaker with a watch glass and boil it for 10 minutes. 7. Cool the solution and filter it through glass wool into a clean storage bottle. Label the bottle. 8. Calculate the mass of oxalic acid needed to make up 250ml of 0.05M solution. 9. Weigh out accurately about this amount of oxalic acid and transfer to a beaker. Dissolve with about 150ml of distilled water. 0. Transfer the solution to a 250ml volumetric flask and dilute to 250ml. 1. Calculate the concentration and transfer to a labeled bottle. 2. Fill a burette with the KmnO4 solution to be standardized. 3. Pipette 20ml of standard oxalic acid solution into a flask
Rate of reaction - I will be trying to find a pattern in which the amount of acid will be measured against the molarity of the alkali to find out how it effects reaction time .
The Rate of reaction AIM For this experiment I will be trying to find a pattern in which the amount of acid will be measured against the molarity of the alkali to find out how it effects reaction time .The molarity of the alkali will fluctuate, but the molarity of the acid will stay constant. METHOD I will collect evidence by recording down the work I have done dew to the experiment. I will collect this evidence by doing the experiment that I will set out to do like this. First of all I will collect a large beaker to put the experiment into. I will also collect 2 measuring cylinders of 100ml to collect the acid and alkali. I will have 1 25ml-measuring cylinder to collect water in and 2 for each of the chemicals (Hydrochloric acid, and sodium thiosulphate) I will measure out 25ml of the acid (molarity of 2) and then make a mixture of alkali (base molarity is 2) and water, this will depend on the molarity that I want to set my alkali to. When I have the mixture I will give it a stir to make sure the alkali is completely mixed with the water. When I have done this I shall pour my acid into the experiment beaker then I make sure the stopwatch is working (and reset it if need be). When I have done this I make sure that when I pour my mixture of alkali and water in that I press the stopwatch start button at the same time. I will repeat the experiment 3 times and work out an
I am using 10cm3 of limewater I predict that I will use roughly the same amount to neutralise it, and therefore I think that I will use about 10cm3 of acid in each titration.
PRELIMINARY WORK Before the main experiment I carried out some preliminary work. This was for me to decide which indicator would be suitable for the main experiment. For an indictor to be suitable the indicator needs to have- -a sharp colour change rather than gradual, no more than one drop of acid or alkali needed to give a complete colour change. -a distinct colour change -an end point of the titration the same as the equivalence point, otherwise the titration will give a wrong answer. From my preliminary work I picked two suitable indicators, phenolphthalein and methyl orange. The reason these two were the best is because they gave distinct and sharp colour changes. In the end I choose to use methyl orange. This indicator has a ph of 3.1 - 4.4, and is used in reactions involving a strong acid and a weak base. PREDICTION Because of the fact that I am using 10cm3 of limewater I predict that I will use roughly the same amount to neutralise it, and therefore I think that I will use about 10cm3 of acid in each titration. I also used my preliminary work to help me with this as I used around 20cm3 of acid when using 20cm3 of limewater. I think that my end concentration of limewater in gdm is going to be around 1.0. APPERATUS Limewater Volumetric flask- measures 250cm3 very accurately, therefore is suitable for the experiment. Conical flask- used for the titration
