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- Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)arrow_forwardWhat determines Ssurr for a process? To calculate Ssurr at constant pressure and temperature, we use the following equation: Ssurr = H/T. Why does a minus sign appear in the equation, and why is Ssurr inversely proportional to temperature?arrow_forwardConsider the reaction 2SO2(g)+O2(g)2SO3(g) (a) Calculate G at 25C. (b) If the partial pressures of SO2 and SO3 are kept at 0.400 atm, what partial pressure should O2 have so that the reaction just becomes nonspontaneous (i.e., G=+1.0 k J)?arrow_forward
- The melting point for carbon diselenide (CSe2) is 46C. At a temperature of 75C, predict the signs for Ssurr and Swater for the following process: CSe2(l) CSe2(s).arrow_forwardDiscuss the effect of temperature change on the spontaneity of the following reactions at 1 atm: (a) Al2O3(s)+2Fe(s)2Al(s)+Fe2O3(s) H =851.4kJ;S =38.5J/K (b) N2H4(l)N2+2H2(g) H =50.6kJ;S =0.3315kJ/K (c) SO3(g)SO2(g)+12 O2(g) H =98.9kJ;S =0.0939kJ/Karrow_forwardWhat is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)arrow_forward
- Under what conditions is N2 O3(g) ⟶ NO(g) + NO2(g) spontaneous?arrow_forwardThe Haber process for the production of ammonia involves the equilibriumN2(g) + 3 H2(g)⇌ 2 NH3(g)For this reaction, ΔH° = -92.38 kJ and ΔS° = -198.3 J/K. Assume that ΔH° and ΔS° for this reaction do not change withtemperature. (a) Predict the direction in which ΔG for the reaction changes with increasing temperature. (b) Calculate ΔG at25 °C and at 500 °C.arrow_forwardPredict the sign of ∆Ssys for each of the following processes: Gaseous Cl2 dissociates in the stratosphere to form gaseous Cl atomsarrow_forward
- Consider the reaction: 2A(g) + B(g) → 2C(g) If ΔG° = −5.4 kJ/mol at T = 25°C and PA = PB = 1 atm and PC = 4 atm, which of the following statements is correct? (R = 8.314 J/K • mol) This reaction favors the products because ΔG > 0. K < 1, because ΔG° < 0. Under the current conditions, ΔG > 0. Hence, this reaction will go in the reverse direction to reach equilibrium. K < 1, because ΔG > 0.arrow_forwardthe value of delta G at 181 degree celcius for the formation of calcium chloride from calcium metal and chlorine gas is __ kJ/mol. at 25 degree celcius for this reaction delta H is -795.8 kJ/mol, delta G is -748.1 kJ/mol and delta s is -159.8 J/karrow_forwardConsider ethylene (C2H4) a) write a balanced chemical equation for the combustion of 1 mole of ethylene gas with oxygen to produce carbon dioxide and liquid water. b) calculate Delta H° for the reaction at 25 degrees C c) Calculate Delta S° For the reaction at 25 degrees C d) calculate Delta G° for the reaction at 25 degrees C e) calculate Delta G° for the reaction at 125 degrees C f) at which temp if any will the reaction be at equilibrium?arrow_forward
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