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This experiment is called "Thermodynamic Properties of Urea". k = [urea]saturated 1. Determination of Equilibroun Constant,...

This experiment is called "Thermodynamic Properties of Urea".
k = [urea]saturated
1. Determination of Equilibroun Constant, k
deltaG = -RTInK from the measured k, calculate deltaG.
mass of urea: 1.2010g
volume of solution: 4.8 mL
t: 9C

2. Determination of deltaH for dissolution of urea.
deltaG = deltaH - T deltaS
q = mCsH2O * deltat
ti = 20C
tf = 16C
mass of urea = 2.6227g
volume sol = 40mL
qsoln - n = -qrxn
qsol - n = m * C * delta t
deltaH = qrxn / #mol urea (kJ/mol)

3. Calculate ΔH for the dissolution of urea. Is the process endothermic or exothermic?

4. Calculate the concentration of urea in a saturated solution. Then, calculate Keq for the dissolution of urea.

5. Using the temperature of the saturated solution you made and the value of Keq, calculate
ΔG for the dissolution of urea. Is the dissolution spontaneous or nonspontaneous at this temperature?

6. Calculate ΔS for the dissolution of urea. Does the dissolution process represent an increase or a decrease in entropy?


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