- Data Table 1 Determination Of Kht Saturation Temperatures Mass Of Flask 120 88 G Mass Of Flask Kht 121 98 G Mass Of 1 (45.59 KiB) Viewed 42 times
- Data Table 1 Determination Of Kht Saturation Temperatures Mass Of Flask 120 88 G Mass Of Flask Kht 121 98 G Mass Of 2 (37.7 KiB) Viewed 42 times
- Data Table 1 Determination Of Kht Saturation Temperatures Mass Of Flask 120 88 G Mass Of Flask Kht 121 98 G Mass Of 3 (50.55 KiB) Viewed 42 times
- Data Table 1 Determination Of Kht Saturation Temperatures Mass Of Flask 120 88 G Mass Of Flask Kht 121 98 G Mass Of 4 (32.26 KiB) Viewed 42 times
- Data Table 1 Determination Of Kht Saturation Temperatures Mass Of Flask 120 88 G Mass Of Flask Kht 121 98 G Mass Of 5 (51.3 KiB) Viewed 42 times
Data Table 2: Observation of the Common Ion Effect
Discussion Part 1 Discuss the equilibrium reaction, common ion effect, the KsR obtained, \% error, Discussion Part 2 Explain the graph, what it means, the equation of the graph, what it means and what you can discern from the graph. Discussion Part 3 Explain the results you obtained (eg, values obtained for Entropy, Enthalpy, Gibbs free energy and Ksp). What does it tell you about the process occurring? Was this what you expected? Why or why not? Explain those results in depth (what do the numbers mean). That is why this part is one of the most important from your report where the student demonstrates their understanding of the experiment and the obtained values. Discussion Part 4 Link the concepts from the introduction with the experimental results Discussion Part 5 What changes did you notice to the saturation temperature upon increase of volume? What does this tell you?
a. Use the value obtained for the slope of the graph to solve for ΔH∘ using the equation derived in Question 2. loK =−11903.3 K/T+32.6 Slope =−ΔH/R=−11903.3 KΔH=98964.04 J/mol i b. Use the value obtained for the y-intercept of the graph to solve for ΔS∘ using the equation derived in Question 2. ΔS/R=32.6 ΔS=32.6R ΔS=271 J/molK 7/13/202220.53 Linear Rearessonfor Datali-B:
Calculate ΔG∘ at 298 K using the equation provided in the introduction - this represents the free energy associated with dissolving KHT in water at 25∘C. ΔG=ΔH−TΔSΔG=98964.04 J/mol−298 K(271 J/molK)ΔG=18206 J/molΔG=18.21 kJ/mol To calculate the standard enthalpy change of a reaction (ΔHrxn∘) for the process KHT(s)⇌KHT(aq) the following equation can be used: ΔHrxn∘=∑ΔHf∘( products )−∑ΔHf∘( reactants ) Given the following information, calculate ΔHrxn∘ and compare to the experimentally obtained value (Question 3a). Calculate the percent error between the theoretical and experimental values. ΔHf∘ of KHT(s)=−1545 kJ/molΔHf∘ of KHT(aq)=−1497 kJ/mol AH reaction ≡(−1497+1545)kJ/mol =48 kJ/mol