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Using the thermodynamic data provided below, calculate Ka2 for H2CO3(aq) at 25° H*(aq) H:CO3(aq) HCO3 (aq)...
Using the thermodynamic data provided below, calculate Ka2 for H2CO3(aq) at 25° H*(aq) H:CO3(aq) HCO3 (aq) CO3(aq) AH° (kJ/mol S (J/K mol) 0 0 -698.7 191 -691.11 95.0 -676.26 -53.1 Multiple Choice 4.3910-9 459-10-11 459-10-10 None of the above 409-10-11
Use the following data to calculate the Ka of carbonic acid at 253 K. H2CO3 (aq) <==> H+ (aq) + HCO3- (aq) A G° (kJ/mol) -623.2 Substance H2CO3 (aq) HCO3- (aq) H+ (aq) -586.8 0.00 Submit your answer in the following format: 1.23e4, use three sig figs
Using the data provided in the Table, calculate the various entropies below for H2S(aq) ⟶ H+(aq) + HS-(aq) Enter your numbers to 1 decimal places. substance or Ion ΔH°f (kJ/mol) S° (J/mol K) H2S(aq) -39 122 H+(aq) 0 0 HS-(aq) -17.7 61.1 Calculate ΔSsystem (J/K) Calculate ΔSsurrouding (J/K) Calculate ΔSuniv (J/K)
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...
Using the thermodynamic data provided below, calculate Ksp for Mg(OH)2(5) at 25 AH。f (kJ/mol) So (J/K.mol) Mg(aq) 117.99 -10.5 63.1 2+ -461.96 -229.94 -924.66 OH-(aq) Mg(OH2(5)
Consider the reaction: 2HBR(g) >H2(g) + Br2() Using standard thermodynamic data at 298K, calculate the free energy change when 1.51 moles of HBr(g) react at standard conditions AG° kJ rxn AHof (kJ/mol) AG°F (kJ/mol) s° (J/mol K) Beryllium Вe(s) 0 9.5 -569.0 ВeO(s) -599.0 14.0 Be(ОН)2(s) -902.5 -815.0 51.9 AH°f (kJ/mol) AG°f (kJ/mol) s° (J/mol K) Bromine Br(g) 111.9 175.0 82.4 Br2() 152.2 0 0 Br2(g) 30.9 3.1 245.5 Br2(aq) -3.0 4.0 130.0 -121.0 -175.0 82.0 Br (aq) BrF3(g) -255.6...
Consider the following reaction: A ↔ B Using the thermodynamic data provided below at 25 °C, determine the equilibrium constant for this reaction. R = 8.314 J/mol K . ΔGof(A) = -2.2 kJ/mol ΔGof(B) = -4.8 kJ/mol My key says the correct answer is 2.9, what do you use to get there?
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....
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...