Plan: Aim: The enthalpy change of combustion of a fuel is a measure of the energy transferred when one mole of fuel burns completely. A value for the enthalpy change can be obtained by using the burning fuel to heat water and using fact that 4.2j of energy are required to raise the temperature of 1g of water by 1oC. In this investigation my aim is to find the enthalpy change of combustion of a number of alcohols so that I can investigate how and why the enthalpy change is affected by the molecular
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on the molar enthalpy change of a neutralization reaction Principle H2SO4(aq)+2NaOH(aq)=Na2SO4(aq)+2H2O(l) The reaction is a exothermic reaction‚ when the heat released by it is absorbed by water‚ the temperature of the water increases. The heat produced by the reaction can be calculated if it is assumed that all the heat is absorbed by the water. Heat change of reaction=-heat change of water =-mH2O×cH2O×△TH2O As the water has gained the heat produced by the reaction‚ the heat change of reaction
Free Thermodynamics Temperature Sodium hydroxide
LAB OF ENTHALPY CHANGE IN COMBUSTION Objective: Determine the Enthalpy change of combustion ΔHc of three different alcohols. Methanol‚ Ethanol and Isopropilic acid. Procedure: 1. Fill the spirit micro burner with Ethanol and weight it 2. Pour 100 cm3 of water into the aluminum cup 3. Arrange the cup a short distance over the micro burner 4. Measure the temperature of water 5. When the temperature of the water has risen by 10°C‚ record the temperature. 6. Reweight
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Study of the first element – Hydrogen. Answer the following questions:- 1. Give a reason why hydrogen can be placed in group 1[IA] and group 17[vIIA] of the periodic table. 2. What similarities does it show with group 1[IA] and group 17[VIIA]. With special reference to valency electrons and ion formaton and examples. 3. How does hydrogen occur in the free and combined state? 4. Which metals react with cold‚steam and boiling water to form their respected oxides and hydroxides ? Give examples and
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Candy Au Introduction The reaction between zinc and copper (II) sulphate is endothermic. If an excess of zinc powder is added to a measured amount of aqueous copper (II) sulphate in a calorimeter and the temperature change is recorded over a period of time‚ the enthalpy change of the reaction can be experimentally determined. Assumption 1. Mass of H2O in 100cm3 of CuSO4 solution is 100g 2. Specific heat of solution is 4.18 kJ kg-1 K-1 which is the same as the specific heat of water
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Volumetric Determination of Impure Sodium Carbonate (Na2CO3) Introduction: To determine the total amount of carbonate in unrefined sodium carbonate‚ soda ash‚ a titration is done using a standardized solution of HCl. Aqueous HCl is a strong acid and therefore almost completely disassociates into H+ and CL-. Therefore‚ when HCl is used in a titration‚ the H+ is the titrant. Carbonate in aqueous solution is able to accept a proton‚ i.e. it acts as a base. When carbonate accepts the H+ a bicarbonate ion is
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Experiment ENTHALPY AND ENTROPY OF ZINC WITH COPPER SULFATE The CCLI Initiative Computers in Chemistry Laboratory Instruction LEARNING OBJECTIVES The learning objectives of this experiment are to. . . ! ! determine changes in enthalpy and entropy of the reaction of zinc with copper sulfate using two methods: electrochemistry and calorimetry. compare the enthalpy values obtained by the two methods. BACKGROUND Thermodynamics is concerned with energy changes that occur in chemical and physical process
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5. POTASSIUM PERMANGANATE Potassium permanganate (KMnO4) is used primarily to control taste and odors‚ remove color‚ control biological growth in treatment plants‚ and remove iron and manganese. In a secondary role‚ potassium permanganate may be useful in controlling the formation of THMs and other DBPs by oxidizing precursors and reducing the demand for other disinfectants (Hazen and Sawyer‚ 1992). The mechanism of reduced DBPs may be as simple as moving the point of chlorine application further
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According to Elson (2000)‚ potassium is one of the most common prescribed minerals. This mineral is crucial to cardiovascular and nerve functions. When potassium is low fatigue is the most common symptom. The early symptoms include muscle weakness‚ slow reflexes‚ and dry skin or acne; these initial problems may progress to nervous disorders‚ insomnia‚ slow or irregular heartbeat‚ and loss of gastrointestinal tone. A sudden loss of potassium may lead to cardiac arrhythmia. Low potassium may impair glucose
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Hydrogen Peroxide & Inorganic Peroxy Compounds Hydrogen Peroxide Hydrogen peroxide (H2O2) is the simplest peroxide (a compound with an oxygen-oxygen single bond). It is also a strong oxidizer. Hydrogen peroxide is a clear liquid‚ slightly more viscous than water. In dilute solution‚ it appears colorless. Reactions Decomposition Hydrogen peroxide decomposes exothermically into water and oxygen gas spontaneously: 2 H2O2 → 2 H2O + O2 This process is thermodynamically favorable. It has
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