CHM270L expt 6 - , Experiment6 HeatofCombustion Section:A31...

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MAPUA INSTITUTE OF TECHNOLOGY School of Chemical Engineering, Chemistry and Biotechnology P h y s i c a l   C h e m i s t r y   L a b o r a t o r y   1 Experiment 6 Heat of Combustion Section: A31 Group No.4: Date Performed:   May 8, 2007 Members: Date Submitted:   May 15, 2007 Javier, Sandra        Ko, Denniel Gaviola, Catherine Gososo, Shelamae Olivete, Jasper Ryan  Abstract The Heat of combustion (ΔH c 0 ) is the energy released as heat when a  compound undergoes complete combustion with oxygen. The chemical reaction is  typically a hydrocarbon reacting with oxygen to form carbon dioxide, water and heat.  The heat of combustion is traditionally measured with a bomb calorimeter. It may  also be calculated as the difference between the heat of formation (Δ f H 0 ) of the  products and reactants. Heat of combustion was of high priority within this  experiment.  With the use of a bomb calorimeter the heat of combustion of benzoic  acid, naphthalene and sucrose were 6318.2044, 9476 and 3927.86 respectively.  Using the Bomb calorimeter the heat acquired in specific compounds such as  Benzoic acid, naphthalene, and sucrose and compares it to the actual or literature 
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value of that compound which on the verge yielded to a 0%, 1.47% and 0.41% of  percentage difference. I. Introduction In this experiment, we are after to “heat of combustion”—which is the heat  released during combustion. In particular, it is the amount of heat released when a  given amount (usually 1 mole) of a combustible pure substance is burned to form  incombustible   products   (water   and   carbon   dioxide);   this   amount   of   heat   is   a  characteristic   of   the   substance.   Heats   of   combustion   are   used   as   a   basis   for  comparing the heating value of fuels, since the fuel  that produces the greater  amount of heat for a given cost is the more economic. Heats of combustion are also  used in comparing the stabilities of chemical compounds. Equal quantities of two  isomeric hydrocarbons burn to produce equal amounts of carbon dioxide and water,  the one releasing more energy (with the higher heat of combustion) is the less  stable, since it was the more energetic in its compounded form. The actual process occurring in the calorimeter involves the conversion of 
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This note was uploaded on 07/31/2011 for the course CHE-CHM-BT CHM170L taught by Professor Maynardaustria during the Spring '11 term at Mapúa Institute of Technology.

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CHM270L expt 6 - , Experiment6 HeatofCombustion Section:A31...

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