tribianni Posted April 28, 2014 Report Share Posted April 28, 2014 (edited) My lab report is about calculating the neutralisation enthalpy of HCl and NaOH and then CHCOOH and NaOH. experimental results of both reactions are higher than the theoratical values and i cant find reasons to explain. There is obviously heat loss but how does this make the experimental value greater than the theoratical value? and the theoratical value is the standart molar enthalpy but my experiment was not carried out under standart conditions. Actually the initial temperature was 21 degree celcius, not 25. How does this affect the results? NEED URGENT HELP PLEASE!! Edited April 28, 2014 by dilara Reply Link to post Share on other sites More sharing options...
Emmi Posted April 28, 2014 Report Share Posted April 28, 2014 If there is an error in the value you got from experiment and the theoretical value, aside from random fluctuations in the data that means there are systematic errors that occurred during the lab that you need to discuss. Systematic errors are things that the experimenter did wrong. Did you properly wash all of the equipment between trials and between using a new substance? If not this could affect your value. Did you allow the reaction to completely finish before you took data, or was there still unreacted material? Think about those kinds of things and go from there. 1 Reply Link to post Share on other sites More sharing options...
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