Sulphuric acid/ sulfuric acid is a type of organic acid with wide range of uses. It has the molecular formula of H2SO4 and a molecular weight of 98.079 g/mol. This organic acid has an appearance of a colourless to a light yellowish liquid with an odorless scent.
Contact Process is a process that is commonly used to produce sulphuric acid. To date, there are three types of contact process which are the Single-Contact Process, Double-Contact Process and the Wet Contact Process. It is known that the Double Contact Process is more commonly in used due to its high practicality in manufacturing sulphuric acid. In large plants, the production of sulphuric acid and be up to 1.3 tonne in excess per metric tonne. The contact process can be categorized
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Chemical equation: . This reaction is exothermic and catalyst is needed to increase the rate of conversion in this reaction. The catalyst used is the vanadium pentoxide. Vanadium pentoxide is manufactured into different types of shape. However it has been found that the most efficient ones would be the daisy-shaped catalyst though the one more commonly in used would be the ring-shaped.With reference to Le Chatelier’s Principle, the increase of temperature in an exothermic reaction will decrease the equilibrium of the conversion. Therefore, it is important for the reaction to take place in low temperature. The recommended temperature range would be from 400℃ to 450℃. According to the chemical equation, 2 mole of sulphur dioxide and 1 mole of oxygen will give us 2 mole of sulphur trioxide. This makes 3 molecules on the left side of the equation whilst 2 molecules on the right side of the equation. In agreement to Le Chatelier’s Principle, the increase of pressure will favor the conversion of sulphur triodixe. However, it is not conventional for manufacturing therefore pressure will be set at 1 atm.
The third step is the absorber step. The sulphur trioxide gas will then be absorbed from the gas mixture formed previously in the reactor step. As much as 98%wt of sulphuric acid is absorbed from the gas mixture. Heat is produced during this reaction. Chemical equation:
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It is estimated that about 800,000 tonnes of sulphuric acid is produce to meet the market’s demand. This chemical is widely used in the latex industry to coagulate rubber, electronic industry as an etching agent, the palm oil industry as a neutralizing agent, and as a base chemical for many chemical industries. Sulphuric acid is also heavily in used for the manufacturing of fertilizers and in the automotive industry. Blooming agriculture industry in the country and the increasing production of automotive has contributed huge needs for sulphuric acid. The worldwide production of the sulphuric acid stands around 200 million tonnes per annum. In Malaysia, one of the largest manufacturers of sulphuric acid is produced by See Sen Chemical Berhad with an annual capacity of 255,500 metric tonnes. The sulphuric acid plant is located at Kemaman,Terengganu. That being said, with the large amount of acid produced by only just one manufacturer, we can imagine that the demand for sulphuric acid in the country is
The reaction was repeated 3 times and average rate noted. From these rates a graph was plotted which describes the relationship of the pressure produced and number of drops added. The reaction rates were measured by Kpa/min and were written to 4 figures for precise results. Time was measured by stop watch. Table 4 shows a summary of all the groups which participated in the lab session.
How is temperature related to this reaction? The higher the temperature the slower they move.
Given that 3.327 g of product was produced during the reaction, how many grams of water were released as water vapor? (moles = mass/molecular weight). From observation it appeared 1.673 grams of water were released as water vapor. 5. Write a balanced equation for the decomposition of copper carbonate hydroxide hydrate.
The lab started off by measuring critical materials for the lab: the mass of an an empty 100 mL beaker, mass of beaker and copper chloride together(52.30 g), and the mass of three iron nails(2.73 g). The goal of this experiment is to determine the number of moles of copper and iron that would be produced in the reaction of iron and copper(II) chloride, the ratio of moles of iron to moles of copper, and the percent yield of copper produced. 2.00 grams of copper(II) chloride was added in the beaker to mix with 15 mL of distilled water. Then, three dry nails are placed in the copper(II) chloride solution for approximately 25 minutes. The three nails have to be scraped clean by sandpaper to make the surface of the nail shiny; if the nails are not clean, then some unknown substances might accidentally mix into the reaction and cause variations of the result.
ST Report In the experiment, the problem was the contaminants that were affecting the quality of the water samples. To fix this issue, three scientists had to determine the contaminants that were present in the samples. One sample was from the school sink and the second sample was from an unknown source. The scientists conducted many tests to figure out what pollutants were present in the water.
The enthalpy changes will be determined by examining the effect the alcohols have on the water’s temperature change. Balanced Equations for the Combustion reactions of Ethanol and Butanol: Ethanol combustion: CH3CH2OH(l)+ 3O2 (g) --> 2 CO2 (g) + 3
Copper Cycle Lab Report Ameerah Alajmi Abstract: A specific amount of Copper will undergo several chemical reactions and then recovered as a solid copper. A and percent recovery will be calculated and sources of loss or gain will be determined. The percent recovery for this experiment was 20.46%.
The results do not support the hypothesis that a higher surface area to volume ratio would result in sulphuric acid being diffused into the agar cubes in the shortest amount of time. This is evident in the results as the exact opposite to what was predicted occurred. Instead of the smallest cube with the largest surface area to volume ratio of 1cm3 having the quickest diffusion rate, it conversely took the longest at 0.092 cm3 per second, whilst the 2cm3 cube with 0.0384 cm3 per second took the least amount of time. This directly refutes the hypothesis. There was also no consistent trend evident in the results.
Jaspreet Singh Professor Paratore Biology 1 November 1, 2014 Spectrophotometry Identifying Solutes and Determining Their Concentration Statement of the Exercise or of the Problem The purpose of the lab experiment was to attain the following objectives: • Learning to Operate the Spectrophotometer • Construct absorption spectra for cobalt chloride and chlorophyll. Hypothesis If greater and higher concentrations of cobalt chloride are added to each solution then greater amounts of light would be absorbed by each solution. Thus a liner relationship will result in which the absorbance of a substance would be proportional to its concentration, which will be depicted, in a linear graph.
CLAIRE MUNTING 29/01/2018 Criterion C EFFECTS OF SURFACE AREA OF CALCIUM CARBONATE UPON RATE OF REACTION Calcium Carbonate Chips 1 Introduction: Within the current investigation, the effects of the surface area of Calcium Carbonate (CaCO3) in combination with Hydrochloric acid (HCl) upon its rate of reaction. CaCO3, commonly referred to as limestone, is an organic substance and is, in a sense, the crystallised “carbonic salt” of the element, calcium2. In addition to being a salt, the pH level of Calcium Carbonate is 9.91, and it is therefore, a basic substance, due to the fact that it is comprised of a pH level higher than 7, which is neutral3. HCl, however, is the bodily acid found in the stomach of human beings.
Aim: To find out the relationship between the greater concentration of sodium thiosulfate when mixed with hydrochloric acid and the time it takes for the reaction (the time it takes for the solution to turn cloudy) to take place and to show the effect on the rate of reaction when the concentration of one of the reactants change. Introduction: The theory of this experiment is that sodium thiosulfate and hydrochloric acid reach together to produce sulfur as one of its products. Sulfur is a yellow precipitate so, the solution will turn to yellow color while the reaction is occurring and it will continue until it will slowly turn completely opaque. The reaction of the experiment happens with this formula: “Na2 S2 O3 + HCL =
n=cV n=1.00 mol dm^(-3)×(25 dm^3±0.16%)/1000=0.025 mol±0.16 % The enthalpy of neutralization is then calculated. ∆H=(-1356.5 J±3.104% )/(0.025 mol±0.16%)=-54260 J 〖mol〗^(-1)±3.3 % ∆H=-54260 J m〖ol〗^(-1)±3.3%÷1000=-54 kJ 〖mol〗^(-1)±3.3 %
Biochemical tests are the tests used for the identification of bacterial species based on the differences in the biochemical activities of different bacteria. Bacterial physiology differs from one species to the other. These differences in carbohydrate metabolism, protein metabolism, fat metabolism, production of certain enzymes and ability to utilize a particular compound help them to be identified by the biochemical tests. Gram’s stain was originally devised by histologist Hans Christian Gram in 1884. Gram-positive bacteria stain purple, while Gram-negative bacteria stain pink when subjected to Gram staining.
Introduction The goal of the experiment is to examine how the rate of reaction between Hydrochloric acid and Sodium thiosulphate is affected by altering the concentrations. The concentration of Sodium thiosulfate will be altered by adding deionised water and decreasing the amount of Sodium thiosulphate. Once the Sodium thiosulphate has been tested several times. The effect of concentration on the rate of reaction can be examined in this experiment.
Abstract The unknown concentration of benzoic acid used when titrated with standardized 0.1031M NaOH and the solubility was calculated at two different temperatures (20◦C and 30◦C). With the aid of the Van’t Hoff equation, the enthalpy of solution of benzoic acid at those temperatures was determined as 10.82 KJ. This compares well with the value of 10.27KJ found in the literature.