3. d. Using the data given, calculate each of the thermodynamic quantities for Bal, dissolving in...
Using the thermodynamic data given in the procedure, calculate ∆H°, ∆S°, and ∆G for the dissolution of each salt in Part 1. Use the initial temperature you recorded in lab for the ∆G calculation. Data Table 1 Salt Observations Mass of Salt (g) Volume of Water (ml) 5.0 Initial Final Temperature Temperature (°C) (°C) 1.0173 23.1 21.9 Sodium Chloride completely dissolved, slightly cooler 5.0 1.0233 22.8 15.2 Potassium Chloride completely dissolved, cold to the touch 5.0 0.9824 23.2 30.7 Calcium...
- T 2 31 5 6 Using the thermodynamic data given in the procedure, calculate AH°, AS, and AG for the dissolution of each salt in Part 1. Use the initial temperature you recorded in lab for the AG calculation. AH (kJ/ S (J/mol K) mol) Salt Observations Volume of Water (ml) 5.0 Mass of Salt (g/ Initial Final Temperature Temperature 411.1 72.12 Sodium Chloride 1.0173 23.1 219 82 NaCl) KCI (5) CaCl (s) Nat(a) 436.7 -795.4 completely dissolved slipy...
Calculate the equilibrium constant from the standard free energy change. Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction 2502(g) + O2(0) 2503(9) AH°F (kJ/mol) AGⓇ, (kJ/mol sº (/mol K) 205.1 Oxygen 02(0) (9) O3(9) 249.2 231.7 161.1 142.7 163.2 238.9 AH°: (kJ/mol Agºr (kJ/mol) 5° (J/mol K) 31.8 0.3 0.3 278.8 3 3.0 167.8 33.0 - 15.0 Sulfur S(s, rhombic) S(s, monodinic) S(g) Sz"(aq) Sg(9) SzCl2(g) SF6(9) H2S(9) soz(9) SO3(0) 1 0....
Given the reference thermodynamic data below taken at 25°C, calculate the value of the equilibrium constant for the reaction shown at 800.0°C COCI, (g) 2 CO (g) + Cl2 (g) AG° = 69.46 kJ AH° = 110.38 kJ AS° = 137.24 J/K at 800.0°C
Use standard thermodynamic data (in the Chemistry References) to calculate AG at 298.15 K for the following reaction, assuming that all gases have a pressure of 10.88 mm Hg. 2NO(g) + O2(g)—>2NO2(g) AG= kJ/mol Nitrogen AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) N2(g) 191.6 N(9) 472.7 455.6 153.3 NH3(9) -46.1 -16.5 192.5 NH3(aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 NO(9) 90.3 86.6 210.8 NOCI(g) 51.7 66.1 261.8 NO2(9) 33.2 240.1 51.3 104.2 N2O(9) 82.1 219.9 N204(9) 9.2 97.9...
Consider the reaction 2 CO2(g) +5 H2(e) C H2(e) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: Submit Answer Retry Entire Group more group attempts remaining AH,(kJ/mol) AG® (kJ/mol) Sº (J/mol K) -238.7 -116.0 126.8 219.0 -363.0 249.0 135.1 -166.3 -110.0 -351.0 125.0 209.2 68.2 - 129.0 202.0 226.7 200.9 52.3 - 166.0 -53.0 -277.7 219.6 250.0 242.0 160.7 -13.0 -235.1 282.7 Carbon CH3OH (1) H2CO...
Consider the reaction 4HCK(g) + O2(1) 2H2O(n) + 2Cl(s) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if the pressure of each gas is 20.21 mmHg ANSWER kJ/mol Submit Answer Try Another Version 2 item attempts remaining The molar solubility of silver chromate in a 0.246 M sodium chromate solution is M. Submit Answer Try Another Version 3 item attempts remaining
Consider the reaction: 12(g) + Cl2(g)—>21CI(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.950 moles of L2(g) react at standard conditions. AGºrxn = kJ Iodine AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 12(s) 0 0 116.1 12(9) 62.4 19.3 260.7 23.0 16.0 137 12(aq) I(g) 106.8 70.3 180.8 1 (9) -197.0 -55.0 -52.0 106.0 I'(aq) ICI(9) 17.8 -5.5 247.6 Chlorine Cl(9) AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) 121.7 105.7 165.2 0 0 223.1 -23.0...
Need to know how to work out problem in steps and the answer to each salt to check my work pls Calculate the molar solubility of salt in pure water. The Ksp value is -The instructors will choose a salt such as CaCO3, Pblz, Hg Clh, Ag PO4, or Ca(PO4)2. The instructors wil give a numerical value for Ksp appropriate to the salt. - Your full-credit answer must show (1) the balanced solubility equilibrium reaction equation, (2) the Ksp equilibrium...
7 and 8 7. Using the Thermodynamic Data from Appendix 3 in your text book, calculate the standard reaction entropy of the following chemical reaction: N2 (g) + O2(g) 2 NO (g) 8. Using the Thermodynamic Data from Appendix 3 in your text book, calculate the standard reaction entropy of the following chemical reaction: Fe2O3 (s) + 3 H2 (g) → 2 Fe (s) + 3 H20 (1) 9. The standard reaction free energy AGº = -64.0 kJ for this...