Measuring the Enthalpy change of combustion Abstract This simple experiment is carried out to show the difference in the enthalpy change of combustion between two fuels‚ hexane and methanol. These fuels are individually weighed before and after used as heat source to heat water in a calorimeter. The result is used to find out amount of heat transferred by the fuel‚ amount of fuel used and the enthalpy change of combustion. Introduction Enthalpy change of combustion is the enthalpy change when a substance
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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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I am going to investigate the enthalpy change of combustion for the alcohol homologous series. I will investigate how alcohols with increasing number of carbons affect the enthalpy change when an alcohol goes under combustion. The energy that alcohols release when being used is called the enthalpy change of combustion. This is defined as "Standard enthalpy change of combustion‚ is the enthalpy change when one mole of a substance burns completely in oxygen under standard conditions (298K‚ 100 KPa
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Title Page: Module Code: FC 511 2T Module Title: Skills for study Tutor Name: Emma Duffy Assessment title: Formative Lab Report: Enthalpy of Combustion of Butanol Student ID Number: 201233920 Date of submission: 6/3/2017 Past tense recapping what you did in the experiment Present tense explain theory and compare theory THINGS TO IMPROVE : Reference Introduction Discussion Avoid Plagiarism Table of Contents Introduction P.3 Aim Materials
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From the experimental data and through its analysis‚ the enthalpy of combustion for the five alcohols were determined; methanol‚ ethanol‚ propanol‚ butanol‚ and pentanol. As the line of best fit in the graph suggests‚ the enthalpy of combustion increased as the sizes of the molecules increased. This was predicted in the hypothesis and proves it to be correct. As seen on the graph‚ the enthalpy of combustion increases from 140kJ/mol for methanol‚ which has the smallest molecular mass‚ to 530kJ/mol
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Task 1: Assessment criterion 2.1 Determine the enthalpy change for the reaction (ΔHfθ) between zinc and copper sulphate solution‚ giving full practical details. Aim To determine the enthalpy change for the reaction between zinc and copper sulphate. Zn (s) + CuSO4 (aq) ZnSO4 (aq) + Cu (s) Introduction In the study of energy (thermodynamics) the system refers to the reacting chemicals (zinc and copper sulphate solution) and the surroundings is everything else (atmosphere
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Chemistry Internal Assessment: Determining the Enthalpy Change of a Displacement Reaction AIM: To determine the enthalpy change for the reaction between copper(II) sulfate and zinc. BACKGROUND THEORY: Bond breaking is endothermic while bond forming is exothermic. The reaction between copper(ll) sulfate and zinc is exothermic as the energy required to form the bonds of the products is greater than the energy required to break the bonds of the reactants. In an exothermic reaction‚ heat is
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Alkanols Heat of Combustion Aim: To determine the molar heat of combustion of methanol‚ ethanol and 1-propanol Materials: 3 spirit burners‚ one containing methanol‚ one containing ethanol and one containing 1-propanol. A thermometer A copper calorimeter 100 ml measuring cylinder Retort stand and clamps Stopwatch Matches Electronic balance Safety assessment: This experiment contains flammable materials remove loose clothing such as ties which could be set alight
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transformations. A reaction may release or absorb energy‚ and a phase may change‚ such as in melting and boiling. Thermochemistry focuses on these energy changes‚ particularly on the system ’s energy exchange with its surroundings. In combination with entropy determinations‚ it is used to predict whether a reaction is spontaneous or non-spontaneous‚ favourable or unfavourable. Chemical reactions can be divided into two based on the energy changes that occur during the reaction which are endothermic and exothermic
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This experiment will test the suggestion that the enthalpy change between a metal and a solution of a salt is related to the relative position of the two metals in the reactivity. Presumably the further apart in the series the bigger the enthalpy change will be. The experiment is as follows‚ 1) Zn(s) + CuSO4(aq) ZnSO4(aq) + Cu(s) 2) Zn(s) + Pb(NO3)2(aq) Zn(NO3)2 (aq) + Pb(s) Both of the solutions will be in 1mol.dm-3 Apparatus: Distilled Water Polystyrene Cup
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