The change in enthalpy for the combustion of magnesium metal Essay exam

The lurch in total affectionateness for the combustion of magnesium all(prenominal)oy bunco========Hesss law of heat summation states that the value of DH for a answer is the homogeneous whether it occurs directly or as a serial of steps. This belief was used to determine the change in henryfor a exceedingly exothermic reaction, the combustion of magnesium metal. Enthalpy changes for the reactions of Mg in HCl (aq) and MgO (s) inHCl (aq) were determined experimentally, then added to that for thecombustion of hydrogen gas to capture at a value of587 kJ/ groin Mg. Compared with the accepted value of 601.8 kJ/mol Mg,our experimental fallacy was 2.46%.IntroductionIn this investigation the change in enthalpy go away be determined fromthe following equation 2Mg + O2 2MgO, besides in an indirect manner. Magnesium metal burns with a blazing passing hot flame to producemagnesium oxide. It would be exhausting to rate the heat of thereaction since the reaction is rapid and occurs at a gamy temperature(LeMay et al, 1996). So, to determine the change in enthalpy we result absorb Hesss Law of heat summation It states that the value of DHfor a reaction is the same whether it occurs directly or as a seriesof steps (LeMay et al, 1996). We will perform the two followingreactions Mg + 2HCl MgCl2 + H2 andMgO + 2HCl MgCl2 + H2O, determine their enthalpy changes (DHs), andthey will then be added to that of a given equation, the combustionof water, H2 + 1/2 O2 H2O DH=-285.5 kJ/mol.In this investigation we will be surveying(a) with potentially dangerouschemicals and safety precautions must be made. Magnesium oxide is arespiratory and eye irritant, the dust must not be inhaled and allwork with MgO should be conducted in the fume hood ( Cartwright,... ...te, only having a 2.46% error. These errors may be accounted for by inaccurate measurements,mathematical mis develops, incomplete reactions, scummy heat collection, fallacious recording of data, and poorl y calibrated calamuss. To avoid such error one should label all materials, check each tool onwards use,take extra care in reading and recording of measurements, parlay checkall calculations, and most of all be patient, labs take time and arushed procedure leads to inaccurate data and incorrect analysis. Sources CitedCartwright, H.(last rewrite 2002, November 5). Chemical and otherSafety Information. The Physical and Theoretical alchemy Laboratory,Oxford University.online. (accessed 2002,December, 4)LeMay, H.E.,Beall, H., Roblee, K.M., and Brower, D.C. (1996).ChemistryConnections to our changing world, Laboratory Manual. Upper SaddleRiver, NJ Prentice Hall. The change in enthalpy for the combustion of magnesium metal Essay testThe change in enthalpy for the combustion of magnesium metalAbstract========Hesss law of heat summation states that the value of DH for areaction is the same whether it occurs directly or as a series ofsteps. This principle was used to de termine the change in enthalpyfor a highly exothermic reaction, the combustion of magnesium metal. Enthalpy changes for the reactions of Mg in HCl (aq) and MgO (s) inHCl (aq) were determined experimentally, then added to that for thecombustion of hydrogen gas to arrive at a value of587 kJ/mol Mg. Compared with the accepted value of 601.8 kJ/mol Mg,our experimental error was 2.46%.IntroductionIn this investigation the change in enthalpy will be determined fromthe following equation 2Mg + O2 2MgO, but in an indirect manner. Magnesium metal burns with a bright extremely hot flame to producemagnesium oxide. It would be difficult to measure the heat of thereaction since the reaction is rapid and occurs at a high temperature(LeMay et al, 1996). So, to determine the change in enthalpy we willemploy Hesss Law of heat summation It states that the value of DHfor a reaction is the same whether it occurs directly or as a seriesof steps (LeMay et al, 1996). We will perform the two followingreac tions Mg + 2HCl MgCl2 + H2 andMgO + 2HCl MgCl2 + H2O, determine their enthalpy changes (DHs), andthey will then be added to that of a given equation, the combustionof water, H2 + 1/2 O2 H2O DH=-285.5 kJ/mol.In this investigation we will be working with potentially dangerouschemicals and safety precautions must be made. Magnesium oxide is arespiratory and eye irritant, the dust must not be inhaled and allwork with MgO should be conducted in the fume hood ( Cartwright,... ...te, only having a 2.46% error. These errors may be accounted for by inaccurate measurements,mathematical mistakes, incomplete reactions, poor heat collection,incorrect recording of data, and poorly calibrated tools. To avoidsuch error one should label all materials, check each tool before use,take extra care in reading and recording of measurements, double checkall calculations, and most of all be patient, labs take time and arushed procedure leads to inaccurate data and incorrect analysis. Sources CitedCartwr ight, H.(last revised 2002, November 5). Chemical and otherSafety Information. The Physical and Theoretical Chemistry Laboratory,Oxford University.online. (accessed 2002,December, 4)LeMay, H.E.,Beall, H., Roblee, K.M., and Brower, D.C. (1996).ChemistryConnections to our changing world, Laboratory Manual. Upper SaddleRiver, NJ Prentice Hall.