Calorimetry

# One was labeled with the proper concentration the

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this laboratory there were two solutions of HCl for use. One was labeled with the proper concentration; the other was an unknown concentration that our lab groups would have to calculate the concentration. There was also NaOH, with a specified concentration, set out to use in Part A and B and to titrate the HCl with in Part C. In Part A & B of this experiment we were to gather a set mL of NaOH and HCl. Pour the HCl in a styrofoam cup then use the thermometer to record the starting temperature and the final temperature after the HCl and NaOH reaction. In part C we slowly added the NaOH 1mL by 1mL every minute and calculated each data point using the LabPro software. Experimental After measuring out 40mL of HCl into a sytrofoam cup we placed the temperature probe into the HCl and recorded the initial temperature. Then we started the Logger Pro computer software to record a graph of the temperature change.We quickly poured 45mL of NaOH into the solution and stirred rapidly. After one minute we stopped the Logger Pro and recorded the final temperature. Then we weighted the ending solution. This table 1 shows the experimental data collected before the experiment of Part A Concentration of HCl Density of HCl Weight of Styrofoam Cup Weight of Cup+HCl Weight of Cup+ HCl+NaOH 10.53 (+/-) 0.01 1.0488(+/-) 0.0001 1.82 g/mL (+/-) 0.01 44.37 g/mL 93.26 g/mL Sample Calculations To calculate the heat flow we use q=mc∆T c is the specific heat of the solution, which is given to us as 3.62 J/gC m= (weight of cup+HCl+NaOH)-weight of cup m=93.26g/mL-1.82g/mL m=92.01g/mL ∆T is found using the Logger Pro technology T(final)=41.36C T(initial)= 20.77 ∆T=T(final)-T(initial) ∆T=41.36-20.77 ∆T=20.59 q=(92.01g/mL)(3.62J/gC)(20.59C) q=6858.04J

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In the book we are given the accepted value for the reaction of kJ/mol so we must find the theoretical value in kJ/mol as well. To calculate our q/mol we must divide by how many moles of HCl are present in the given concentration.
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