Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction shown at 25.0ºC
H₂ (g) + I₂ (g) ⇄ 2 HI (g)
ΔHº = -9.48 kJ
ΔSº = +21.79 J/K
K = Answer at 25.0ºC
Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction shown...
Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction shown at 25.0ºC H₂ (g) + I₂ (g) ⇄ 2 HI (g) Given the thermodynamic data below, calculate the value of the equilibrium constant for the reaction shown at 25.0°C H2(g) + 12 (g) = 2 HI(g) AH° = -9.48 kJ AS° = +21.79 J/K K= at 25.0°C Check
Given the reference thermodynamic data below taken at 25°C, calculate the value of the equilibrium constant for the reaction shown at 800.0ºC COCl2 (g) ⇄ CO (g) + Cl2 (g) ΔGº = 69.46 kJ ΔHº = 110.38 kJ ΔSº = 137.24 J/K K = Answer at 800.0ºC
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
Calculate the value of the free energy change, ΔG, for the reaction below at 227.0ºC when the pressures of NO (g) = 2.00 atm, O₂ (g) = 10.00 atm, and NO₂ (g) = 0.0250 atm. 2 NO (g) + O₂ (g) → 2 NO₂ (g) ΔGº = -70.54 kJ ΔHº = -114.14 kJ ΔSº = -146.43 J/K ΔG = ? kJ
Calculate the value of the free energy change, ΔG, for the reaction below at 175.0ºC when the pressures of H2S (g) = 0.0100 atm, SO2(g) = 0.0250 atm, and H2O (g) = 2.50 atm. 2 H2S (g) + SO2 (g) → 3 S (s) + 2 H2O (g) ΔGº = –90.88 kJ ΔHº = –146.47 kJ ΔSº = –186.45 J/K
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 641 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ /kJ mol-1 -314.4 -45.9 -92.3 Smº /JK-mol-1 94.6 192.8 186.9 Cp.m /JK-mol-1 84.1 35.1 29.1 Do not use the Van't Hoff equation, In(K/K) = -(AHR/R) (T2-1-T1-1) The value of the thermodynamic equilibrium constant is Kp = Number
1) Calculate the equilibrium constant at 138 K for the thermodynamic data in the previous question. Notice that Keq is larger at the larger temperature for an endothermic reaction. 2) Endothermic reaction; increase in entropy Calculate the equilibrium constant at 40 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = 100 J/K.
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 839 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ 7 kJ mol-1 -314.4 -45.9 -92.3 Smº JK-1 mol-1 94.6 192.8 186.9 Cp,m 84.1 35.1 29.1 /JK-1 mol-1 Do not use the Van't Hoff equation, In(K /K1) = -(AHR/R) (T2-1 - 7,-1) The value of the thermodynamic equilibrium constant is Kp= 7.6e14
6) Given the following thermodynamic data, calculate the equilibrium constant for the dissolution of galena, PbS, at 298 K and 1 bar according to the reaction PbS(solid) + H-Pb(aq) + HS. From this, can you calculate the solubility of PbS at pH-2? (Hint: assume [Pb2] [HS] and note that PbSl-1 for pure galena; at pH-2, [H+] 0.01) AHf, lbar (kJ/mol) 97.7 (kJ/mol-K) 0.091 (cm3/mole) 31.5 Galena (PbS, solid H+ (aqueous ion,1 molal Pb2+ (aq. ion, 1 molal HS-(aq. ion, 1...
Using standard thermodynamic data (linked), calculate the equilibrium constant at 298.15 K for the following reaction. HCl(g) + NH3(g)--->NH4Cl(s) K =