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6 determine δs for the reaction so 3 g h 2 o l h 2 so

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6. Determine ΔS° for the reaction SO3(g) + H2O(l)H2SO4(l).S°(J/K·mol)SO3(g)256.2H2O(l)69.9H2SO4(l)156.9A) 169.2 J/K·molC)169.2 J/K·molE) 29.4 J/K·molB) 1343.2 J/K·molD)29.4 J/K·mol
7. HI has a normal boiling point of–35.4°C, and its ΔHvapis 21.16 kJ/mol. Calculate the molarentropy of vaporization (ΔSvap).
8. The thermodynamic condition for a spontaneous process at constant T and P is:
9. Which of the following conditions must be met for a chemical reaction to be spontaneous at alltemperatures?
ΔG°f(kJ/mol)H2O(l)237.2HNO3(l)79.9NO(g)86.7NO2(g)51.810. Calculate ΔG° for the reaction:2 NO(g) + Cl2(g)2 NOCl (g)using the following ΔGf° (in kJ/mol): NO(g) 86.55, Cl2(g) 0.00, NOCl(g) 66.35.A)40.4 kJ/molC) 40.4 kJ/molE)20.2 kJ/molB) 20.2 kJ/molD) 152.9 kJ/mol11. Use thegiven data at 298 K to calculate ΔG° for the following balanced reaction:2 Cl2(g) + SO2(g)SOCl2(g) + Cl2O(g)Substance:Cl2(g)SO2(g)SOCl2(g)Cl2O(g)ΔH°f(kJ/mol):0296.8212.580.3S°(J/K·mol):223.0248.1309.77266.1A) 129.3 kJB) 133.6 kJC) 196.0 kJD) 199.8 kJE) 229.6 kJ12. Consider the figure below which shows ΔG° for a chemical process plotted against absolutetemperature.From this plot, it is reasonable to conclude that:A) ΔH° > 0, ΔS° > 0B) ΔH° > 0, ΔS° < 0C) ΔH° < 0, ΔS° > 0D) ΔH° < 0, ΔS° < 0E) ΔH° = 0, ΔS° = 013. The reaction of methane with water to form carbon dioxide and hydrogen is non-spontaneousat 298 K.At what temperature will this system make the transition from non-spontaneous tospontaneous?The data refer to 298 K.CH4(g) + 2 H2O(g)CO2(g) + 4 H2(g)Substance:CH4(g)H2O(g)CO2(g)H2(g)ΔH°f(kJ/mol):74.87241.8393.50ΔG°f(kJ/mol):50.81228.6394.40S°(J/K·mol):186.1188.8213.7130.7A) 658 KB) 683 KC) 955 KD) 1047 KE) 1229 K14. Choose the right combination from the choices below for a forward reaction to bespontaneous:A)∆?𝑟𝑥?< 0 then Q > KC)∆?𝑟𝑥?< 0 then Q = KE)∆?𝑟𝑥??< 0 then Q < KB)∆?𝑟𝑥?< 0 then Q < KD)∆?𝑟𝑥??< 0 then Q = K15. Calculate ΔG° for the reaction 3 NO2(g) + H2O(l)2 HNO3(l) + NO(g).A) 8.7 kJB) 192 kJC)414 kJD)192 kJE)155 kJ

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Term
Fall
Professor
BRANT
Tags
Electrochemistry, Redox, buffer solution

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