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G of hclg of solutionweight of hcl g of

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g of HCl/g of solution=weight % of HCl g of solution=(weight of cup+H2O+HCl)-(Weight of Cup+H2O) g of solution=14.84g 1.367g/14.84=0.092 or 9.2% Discussion In part A, using the known concentration of HCl we calculated the theoretical q(rxn) as 55.8kJ/mol just slightly 0.1 under the actual q(rxn) was. For part B we calculated the weight percent of the unknown HCl and found the theoretical to be 9.8%, the actual was 9.83%. In Part C, using titration to calculate the theoretical % composition of HCl, we calculated it to 9.2%, since the HCl in this experiment is the same unknown as in Part B the actual was 9.83%. Assuming that no heat was lost to the calorimeter or surrounding air would be a source of error because our calorimeter wasn’t a perfect insulator, therefore heat would be released into the surroundings. This would result in a lower theoretical heat flow, which was true for part B. Part C proves to have greater error in the procedure then Part B. This could be due to multiple sources of error such as an increase in heat caused by stirring due to increased kinetic energy, or adding the NaOH inconsistently in relation to the time. Also there is
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error in the additions of the NaOH, an addition of too much or too little NaOH will affect the change in temperature over time. With relation to green chemistry this reaction is a good example of a neutralization reaction. Because the reaction produces H2O and NaCl or water and a salt it is safe to dispose of in a waste bucket. However, any excess HCl and NaOH would need to be neutralized because HCl is acidic and cannot be disposed of without a certain amount of NaOH, which is basic.
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