Standardization of KMnO4 solution Objective: To find out the molarity of the KMnO4 solution Chemical principle: Potassium permanganate is a strong oxidizing agent. It dissolves in water to give intense purple solutions. It reacts with reducing agents and gives colourless Mn2+ ions. So the solution itself acts as the indicator for the titration‚ the end point is noted when the first permanent pink colour appears. The sulphuric acid is used as a catalyst for the reaction. The oxalic acid is
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Results and Discussion Potassium permanganate‚ KMnO4‚ is widely used as an oxidizing agent in volumetric analysis. In acid solution‚ MnO4- ion undergoes reduction to Mn2+ ion as shown in the equation: 8 H+(aq) + MnO4-(aq) + 5e- → Mn2+(aq) + 4 H2O(l). Since the MnO4- ion is violet and the Mn2+ ion is nearly colorless‚ the end point in titrations using MnO4- as the titrant can be taken as the first permanent pink color that appears in the solution being titrated.1 The number of moles of potassium
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On what I have seen‚ the first experiment showed chemical reaction to be more specific‚ combustion. In the experiment the Potassium permanganate (KmnO4) was used as the oxidant‚ and obviously oil as the fuel. As the two were mixed they needed to release energy in form of heat‚ that’s where combustion occurs. I learn that Combustion is the sequence of exothermic chemical reactions between a fuel and an oxidant accompanied by the production of heat and conversion of chemical species. The release of
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RATE OF REACTIONS. The reaction rate (rate of reaction) or speed of reaction for a reactant or product in a particular reaction is intuitively defined as how fast or slow a reaction takes place. For example‚ the oxidative rusting of iron under the atmosphere is a slow reaction that can take many years‚ but the combustion of cellulose in a fire is a reaction that takes place in fractions of a second (right). Chemical kinetics is the part of physical chemistry that studies reaction rates. The concepts
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hydrochloric acid (HCl) on the rate of reaction (mol dm-3 s-1) for the following chemical reaction: CaCO3(s) + HCl(aq) CaCl2(s) + H2O(l) + CO2(g) Research question: How does altering concentration (mol dm-3) of hydrochloric acid (HCl) affect the rate of reaction (g/s) for the following reaction: CaCO3(s) + HCl(aq) CaCl2(s) + H2O(l) + CO2(g) Background information: The reaction between calcium carbonate and hydrochloric acid is an example of a neutralization reaction between an acid and a base.
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Kinetics 6.1 Rates of reaction 6.2 Collision theory 6 16.1 Rate Expression (AHL) 16.2 Reaction mechanism (AHL) 16.3 Activation energy (AHL) 6.1 Rates of reaction 6.1.1 Define the term rate of reaction. 6.1.2 Describe suitable experimental procedures for measuring rates of reactions. 6.1.3 Analyse data from rate experiments. © IBO 2007 Figure 601 An explosion is a quick reaction D ifferent chemical reactions occur at different rates (i.e. speeds). Some
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Rates of Reaction Coursework Aim: To find out how different concentrations of sodium thiosulphate (Na S2 O3) affects the speed of its reaction with Hydrochloric acid (HCL). Introduction When Sodium Thiosulphate and Hydrochloric acid react they produce a cloudy precipitate. Both of the chemicals are clear solutions and they react together to form a yellow precipitate of sulphur‚ the equation for this reaction is: Na2 S2 O3 + HCL‚ H2 O + NaCL + SO2 + S Sodium Thiosulphate + Hydrochloric
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Coursework Rates of Reaction Research The rate of reaction tells us how quickly a chemical reaction takes place. It is important for people in industry to know how fast a reaction goes. They have to know exactly how much of their product they can make each hour‚ day or week. In a shampoo factory‚ the rate might be 100 bottles per minute. We can’t work out the rate of a reaction from its chemical equation. Equations can only tells us how much product we can get. They don’t say how quickly
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The purpose of this lab was to: * Determine the heat of neutralization for the reaction of sodium hydroxide (NaOH) and hydrochloric acid (HCI). Requirement The heat of neutralization (∆Hneutzn ) is the heat transferred when 1 mol of an acid reacts with 1 mol of a base. This heat is generally reported in either kilojoules per mole (kJ/mol) or kilocalories per mole (kcal mol). The reaction of HCI and NaOH solutions is shown in Equation 1. HCI(aq) + NaOH(aq)
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volume). 3. [10 points] The following reaction is found to be first order in A: A −→ B + C If half of the starting quantity of A is used up after 56 seconds‚ calculate the fraction that will be used up after 6.0 minutes. 4. [15 points] The rate law for the decomposition of ozone to molecular oxygen 3 O3 (g) −→ 3 O2 (g) is rate = k [O3 ]2 . [O2 ] The mechanism for this process is k1 O3 O + O2 k−1 k 2 O + O3 −→ 2 O2 Derive a rate law from these elementary steps. Clearly
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