Answer Happy

molarity of amonium nitrate: 10.031M
4.4 Determination and comparison of thermodynamic values 4.4.1 The relevant equations are: AG - AH-TAS and AG° = -RTINK. You should also know how to calculate AH, AG and AS values from data as described in Appendix 3 of the Chang text. 4.4.2 The data for ammonium nitrate as well as for the aqueous ammonium ion and nitrate ion are given below. Substance AH° AGºT AS° Ammonium Nitrate (NH4NO3)) -365.6 kJ/mol -184.0 kJ/mol Ammonium ion (NH4 (4) -132.8 kJ/mol -79.5 kJ/mol Nitrate ion(NO3(aq)) -206.6 kJ/mol -110.5 kJ/mol 151.1 J/mol-K 112.8 J/mol-K 146.4 J/mol-K From this data determine the standard values of AH, AG and AS for ammonium nitrate solid becoming ammonium nitrate solution. 4.4.3 From the molarity of the ammonium and nitrate ion determined from the gravimetric analysis calculate the value of the Ksp for ammonium nitrate. Repeat this calculation using the ISE data. 4.4.4 From the relationship between the standard Gibbs Free Energy and the equilibrium constant calculate a value for the standard Gibbs Free Energy using each of the Ksp values in 4.4.3. 4.4.5 From the calculated AG" values and the average AH value calculate the AS values for this reaction using both values of AG° (gravimetric and ISE). 4.4.6 Determine the percent error between the calculated values from 4.4.2 and the average heat of solution, both of AG° (gravimetric and ISE) values and both of AS° (gravimetric and ISE). values.
hermodynamic values 44 Determin Gravimetric Values ISE Values K- INH.NO:1 K= INH. JINO, Percent Difference Kor - Kisex 100% Kavy from ref Calculated Gravimetric Values ISE Values 4G AG AG° Percent Error Calc - Expt x 100% Calc AH° AH ΔΗ Percent Error Calc - Expt x 100% Calc AS AS Percent Error Calc - Expt x 100% Calc