hydrocloric acid. Hypothesis: If the concentration of hydrocloric acid is increased‚ the rate of reaction will increase and the volume of gass will increase. The reasoning behind the hypothesis is that when there are more molecules in the solution the reactants collide more often‚ so more product is made in a shorter periode of time. The equation was: Mg + 2HCl → MgCl2 + H2 Independent variable | Dependent variable | Controled variables | Value | How to control the CV | Concentration of acid | Rate
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Interpretation of Data When looking at my results i can safely say that the change in HCl concentration does affect the rate of reaction with the Calcium carbonate pebbles. The relationship between the change in HCl and reaction rate can be seen in the graph and raw data table presented above. If you compare the lowest concentration with the highest concentration you’d be able to see that there is a very large contrast between their averages. The average gas production of 0.1M HCl was 0.00693 kPa/s
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nitrogen. 1. The overall reaction for the conversion of sugar(glucose) to acetic acid is: C6H12O6 + 2O2 2CH3COOH + 2CO2 + 2H2O A given volume of nipa sap contains 69.0 g of glucose. If all of this sugar is fermented ‚ how many grams of acetic acid would be produced? 2. How many molecules of oxygen are produced when 29.2 g of water is decomposed forming hydrogen gas and oxygen gas? 3. Hydrofluoric acid‚ HF(aq)‚ cannot be stored in glass bottles because compounds called silicates in the
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fume cupboard • UV light • Clingfilm • Individuals sample of aspirin • Pure sample of aspirin • Sample of salicylic acid Method: 1. Firstly mark a line across the TLC paper approximately 0.5cm from the bottom‚ then mark three spots along the line ensuring to label them according to whether they are your own individual sample‚ the pure sample of aspirin or the sample of salicylic acid during the part of the experiment be sure not to press down too hard on the paper as it could affect the absorbance
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prepared by precipitation method previously reported in literature []. Typically‚ Precursor solution and surfactant solution were prepared by dissolving required amount of aluminium nitrate nonahydrate and sodium dodecyl sulfate in distilled water. Molar composition ratio of both the aluminium precursor and surfactant solutions was taken as 4:1. Mixture was stirred for 15 minutes at room temperature then precipitation was carried out by gradual addition of 30% ammonia solution at pH of 10.5. The subsequent
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Na ions which attaches tothe allosteric site changing the shape of the enzyme to fit a substrate. Materials: • Peroxidase (enzyme in potato) • Hydrogen peroxide‚ 3% • A strong acid‚ pH3 (lemon juice‚ or HCL) 0.5 • A strong base‚ pH 10 (drain cleaner‚ NaOH) 0.5 mol/L • A weak acid‚ pH 6 (vinegar‚ acetic acid( CH3COOH)) 0.5
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EXPERIMENTAL PROCEDURE: 1. 2.07 g of the mixture of naphthalene and benzoic acid was weighed accurately on a balance. The mixture was then dissolved in 40 ml dichloromethane and the solution was poured into a separatory funnel. 2. 20 ml of aqueous sodium bicarbonate solution was added to the dichloromethane. A stopper was placed on the separatory funnel and was shaken and pressure was frequently released. The 2 liquids separated into clear layers and the lower layer (dichloromethane layer) was
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NaCl product‚ showing all of your work in the space below. (5 points) NaHCO3 – The Empty Dish 37.06 (grams) – 24.35 (grams) = 12.71 (grams) NaHCO3 12.71 (grams) NaHCO3 ÷ 84.01 (grams/mole) = 0.1513 moles of NaHCO3 0.135 Moles of NaHCO3 × 58.4428 (Molar mass of NaCl) Giving me 8.8240 (grams) NaCl as my theoretical yield. 4. What is the actual yield of NaCl in your experiment? Show your work below. (4 points) The actual yield is: 31.52 (grams) – 24.35 (grams) = 7.14 (grams) NaCl (After the evaporation
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Soda Ash Analysis and Volumetric Analysis of a Carbonate-Bicarbonate Mixture De Guzman‚ Danica Justine R. Department of Chemical Engineering‚ Faculty of Engineering University of Santo Tomas Espana‚ Manila Abstract Titration is a laboratory method in which the endpoint of a reaction is determined quantitatively. In this experiment‚ the amount of soda ash present in a sample was determined and the alkalinity reported as it was titrated using HCl as the titrant. Also‚ the percentage
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experiment‚ we assembled a reflux apparatus in the fume hood with a 100 mL round bottom flask and a condenser. Next we added 44 mL of sulfuric acid to a 125 mL Erlenmeyer flask. We also measured 4.75g ammonium chloride and 8.75g ammonium bromide into a 125 mL beaker‚ crushed the lumps‚ and placed in a 250 mL Erlenmeyer flask along with the sulfuric acid. We used heat to help the solutes dissolve. When they had dissolved‚ we allowed the flask to cool and then poured 17 mL of the solution into a
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