THE EFFECT OF CONCENTRATION ON REACTION RATE INTRODUCTION • Concentration is one factor which has an effect o the rate of a chemical reaction. In chemistry we describe concentration in terms of the number of moles of a substance there are in every cubic decimetre (litre) of solution‚ written as moles.dm-3 of M for short. • In this experiment you will find out how increasing the concentration of the acid solution changes the rate of the reaction between dilute hydrochloric acid and magnesium
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The aim for this investigation is to investigate the effects of varying the concentration of sodium thiosulfate solution on the rate of the reaction when reacting with dilute hydrochloric acid. It is hypothesized that as the concentration of the sodium thiosulfate solution increases‚ the rate of the reaction will also increase proportionately. Variables The independent variable is concentration. This will be varied by increments of 10mL (10mL to 50mL) and distilled water will be added accordingly
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An investigation to show how the rate of reaction between hydrochloric acid and sodium thiosulphate is affected by the concentration of the acid Simple Procedure Place a conical flask on a piece of paper with a cross on it. Add hydrochloric acid and sodium thiosulphate‚ and record the amount of time taken for the cross to disappear through the solution from the top of the flask. Record this time and repeat this for different concentrations of hydrochloric acid. Fair Test The variables in this
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Carbonates react with strong acids to give off carbon dioxide and water. Marble is calcium carbonate and thus behaves in the same way: CaCO3 (s) + 2HCL (aq)  CaCL2 (aq) + H2O (l) +CO2 (g) In this experiment‚ I am going to see if temperature affects the reaction rate between marble chips and hydrochloric acid by timing the release of carbon dioxide in the reaction. I predict the higher the temperature‚ the faster the reaction rate. This is due to the kinetic theory. The more heat
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by the concentration of starch‚ or whether the results I got were due to the amounts of solution used. This would make both my results and conclusion invalid and unreliable. I also made sure that the temperature of the water bath was at the correct temperature and I kept on checking the temperature of both my amylase‚ and starch using a thermometer. I made sure both solutions were at the same temperature at all times throughout my experiments‚ so that temperature would not have an effect on my results
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Investigating How Concentration of Acid Affects the Reaction Between Calcium Carbonate and Hydrochloric Acid Introduction ============ According to the collision theory temperature‚ concentration‚ surface area and catalysts all affect rates of reaction as shown in the diagrams below. Increasing any of these should increase the number of collisions and so increase the reaction rate up to an optimum point. Increasing the temperature causes the particles to collide with more
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involved in burning magnesium metal. Materials Stirring rod Retort stand Ring clamp Clay triangle Crucible and lid Bunsen burner Flint lighter Balance Crucible tongs 40 cm of magnesium ribbon Method 1. Find the mass of a clean crucible and lid. USE THE SAME BALANCE DURING THE ENTIRE EXPERIMENT. 2. Curl the magnesium ribbon around a pencil to make a size that just fits inside the crucible. Do not curl the ribbon too tightly. 3. Describe the magnesium ribbon. 4. Find the
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equipment as diagram shows. The measuring cylinder must be filled with water and then inverted into the tub. 2.Measure the quantity of hydrochloric acid and marble chips to the decided amount. Add water to the acid to change the concentration to what you need. 3.Take note of the amount of water in the measuring cylinder. 4.Put the marble chips and hydrochloric acid into the conical flask. Replace the bung and start the stopwatch. 5.Once the decided amount of time has passed‚ take note of the remaining
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ICSE Class X Chapter 5 Hydrogen Chloride and Hydrochloric Acid Hydrogen chloride (HCl) : Formula : HCl Nature : Covalent. Molecular Mass : 36·5u [i.e. HCl = 1 + 35·5 = 36·5] Occurrence : (i) Present in gastric juices. (ii) Present in volcanic gases. Laboratory preparation of HCl gas : Hydrogen chloride gas is prepared in laboratory by heating conc. H2SO4 with NaCl. NaCl + H2SO4 Heat → NaCl + NaHSO4 Heat → NaHSO4 + HCl Sodium hydrogen sulphate Na2SO4 + HCl
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Summary This experiment will measure the rate of oxidation of iodide ions by persulphate ions to derive the rate law for the reaction. Starch will be added to the reaction to facilitate the measure of time during the reaction. The reactant solutions will contain (NH4)2SO4 and KI‚ represented as: (NH4)2S2O8 + 2KI -> I2 + (NH4)2SO4 + K2SO4 This can be simplified to: S2O82- + 2I- -> I2 + 2SO42- These equations can only be carried out and be visible after the iodine has completely
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