Consider the reaction listed below along with the accompanying thermodynamic data, carried out at 25 °C and 1 atm: 2SO2(g) + O2(g) ↔ 2SO3(g)
Substance ∆Hf° (kJ/mol) S° (J/K • mol)
SO2(g) -297 248
O2(g) 0 205
SO3(g) -396 257
A.Calculate ∆H°.
B. Calculate ∆S°.
C. Calculate ∆G°. Is this reaction spontaneous? Briefly explain.
D. At what temperature will this reaction first become spontaneous?
E. Calculate the equilibrium constant for this reaction.
Consider the reaction listed below along with the accompanying thermodynamic data, carried out at 25 °C...
Calculate the equilibrium constant for the reaction below if a 5.50 L tank contains 0.526 mol O2, 0.1032 mol SO3 and 0.01658 mol SO2. 2SO3 (g) ↔ 2SO2 (g) + O2 (g)
Exercise 4-The Equilibrium Constant, Enthalpy and Free Energy of Formation The following reaction was carried out in an airtight container: 2SO2(g) + 02(g) 2SO3 (g). The starting concentration of SO2(g) is 0.4 mol L-1, the starting concentration of 02 (g) is 1 mol-L-1. The reaction reaches equilibrium when 80% of So2(g) is converted to SO3 (g), please calculate the concentration of three gas and the 1) equilibrium constant. Exercise 4-The Equilibrium Constant, Enthalpy and Free Energy of Formation The following...
3. The following reaction is carried out at 25°C and 1 atm. Determine the AGºsys using the thermodynamic data tables. Is the reaction spontaneous? Explain. 2 SO2(g) + O2 (g) → 2 503 (9)
Consider the reaction 2SO2(g) + O2(g)2SO3(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 2.11 moles of SO2(g) react at standard conditions. S°surroundings = J/K
Use the given data at 500 K to calculate ΔG°for the reaction 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g) Substance H2S(g) O2(g) H2O(g) SO2(g) ΔH°f(kJ/mol) -21 0 -242 -296.8 S°(J/K·mol) 206 205 189 248
Consider the reaction CO(g) + Cl2(g)---COCl2(g) Use the standard thermodynamic data in the tables linked above. Calculate delta G for this reaction at 298.15K if the pressure of COCl2(g) is reduced to 20.15 mm Hg, while the pressures of CO(g) and Cl2(g) remain at 1 atm. ANSWER: kJ/mol Consider the reaction 2SO2(g) + O2(g)----2SO3(g) Using the standard thermodynamic data in the tables linked above, calculate delta Grxn for this reaction at 298.15K if the pressure of each gas is 25.11...
-89 -470 -419 -203 0 0 0 205 0.3 0.1 249 232 86 143 163 161 239 33 102 -1209 50 NHACIO4(s) NH4Cl(s) Oxygen O2(g) O(g) 03(g) Phosphorus P(s) (white) P(s) (red) P(s) (black) P4(g) PF5(g) PH3(g) HPO4(s) NaOH(aq) Sulfur S(s) (rhombic) S(s) (monoclinic) S2-(aq) S8(g) SF.g) HS(g) SO2(g) SO3(g) SO42- (aq) H2SO4(1) H2SO4(aq) -1105 431 292 206 248 0 41 -18 -39 -21 - 297 23 280 257 -12 -33 24 - 1509 13 -1119 20 -34 -300 -371...
Look at the following reaction. O The Stoichiometry for this reaction affects your calculations for AG SO3 (g) 2SO2 (g) O2 (g) O To calculate AG for the decomposition of one mole Suppose that you are given the following information for of SO3(g), you use the expression AGO (AGof for this reaction at room temperature: O2 AG for SO (AGOf for SO 2)- AGof for SO2(g) 300.19 kJ /mol O If AG is negative, the reaction is spontaneous AGof for...
Consider the reaction of sulfur dioxide gas with oxygen carried out at 25°C and latm. Appropriate data provided in the table at the end of your exam are to be used to help you calculate the requested items below. 2 SO2 (g) + O2 (g) <=> 2 SO3(g) a) Calculate AHO: b) Calculate ASO c) Calculate AGO:
Consider the reaction of sulfur dioxide gas with oxygen carried out at 25°C and latm. Appropriate data provided in the table at the end of your exam are to be used to help you calculate the requested items below. 2 SO2 (g) + O2 (g) <=> 2 SO3(g) a) Calculate AH°: b) Calculate ASO: c) Calculate AGº: