Using the data:
C2H4(g), = +51.9 kJ mol-1, S° = 219.8 J mol-1 K-1
CO2(g), = ‑394 kJ mol-1, S° = 213.6 J mol-1 K-1
H2O(l), = ‑286.0 kJ mol-1, S° = 69.96 J mol-1 K-1
O2(g), = 0.00 kJ mol-1, S° = 205 J mol-1 K-1
calculate the maximum amount of work that can be obtained, at 25.0 °C, from the process:
C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l)
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Using the data: C2H4(g), = +51.9 kJ mol-1, S° = 219.8 J mol-1 K-1 CO2(g), = ‑394 kJ...
12. Using the data: CH«(9), AH; = +51.9 kJ mor', sº = 219.8 J mor' k' CO2(g), AH = -394.0 kJ mor', sº = 213.6 J mor' k' H2O(), AH = -286.0 kJ mor', sº = 69.96 J mor'' O2(g), AH = 0.00 kJ mor', sº = 205 J mor'' calculate the maximum amount of useful work that can be obtained, at 25.0 °C, from the process: C2H4(9) + 3 O2(g) → 2 CO2(g) + 2 H2O(1) a. 1332 kJ...
1.What is ΔGrxno (in kJ) at 440 K for the following reaction? PbO(g) + CO2(g) → PbCO3(s) PbO: ΔHfo = -219.0 kJ/mol and So = 66.5 J/K mol) PbCO3(s): ΔHfo = -699.1 kJ/mol and So = 131.0 J/K mol) CO2: ΔHfo = -393.5 kJ/mol and So = 213.6 J/K mol) 2. At what temperature (in K) does the above reaction become spontaneous?
1-What is ΔGrxno (in kJ) at 338 K for the following reaction? PbO(g) + CO2(g) → PbCO3(s) PbO: ΔHfo = -219.0 kJ/mol and So = 66.5 J/K mol) PbCO3(s): ΔHfo = -699.1 kJ/mol and So = 131.0 J/K mol) CO2: ΔHfo = -393.5 kJ/mol and So = 213.6 J/K mol) 2-At what temperature (in K) does the above reaction become spontaneous? PLEASE answer both
Calculate deltaGϴ for the following balanced reaction at 25 °C using the data in the table below. Calculate AG for the following balanced reaction at 25 °C using the data in the table below. CO(NH2)2(s) + H2O(l) → CO2(g) + 2 NH3(g) A:HⓇ (kJ mor') -333.19 Se (J K-'mol-') 104.6 CO(NH2)2(s) H2O(1) -285.9 69.96 CO2(g) -393.5 213.6 NH3(g) -46.19 192.5
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g).
Calculate ∆Gº for the reaction, CH4(g)+2O2(g)→CO2(g)+2H2O(g), where ∆Gfº=-50.8 kJ/mol for CH4(g), -394 kJ/mol for CO2(g), and -229 kJ/mol for H2O(g): 572 kJ -801 kJ -572 kJ 801 kJ
At 298 K, evaluate deltaG(kJ) and deltaE (V) for 2CH3OH(l) + 3O2(g) -> 4H2O(g) + 2CO2(g) S (J/mol-K) AH°y (kJ/mol) So (J/mol-K) AH(kJ/mol) Substance Substance N2(g) CH-ОН() 126.8 0 191.5 -238.6 CO(g) NH3(g) 197.9 192.5 -110.5 -46.2 CO2(g) NO(g) 213.6 +90.4 210.6 -393.5 NO2(g) +33.8 240.5 H2(g) HNO3(aq) 130.6 146.0 -206.6 H2O( 69.9 -285.8 O2(g) 188.8 H2O(g) 0 205.0 -241.8
Given the values of So given below in J/mol K and the values of ΔHfo given in kJ/mol, calculate the value of ΔGo in kJ for the combustion of 1 mole of propane to form carbon dioxide and gaseous water at 298 K. S (C3H8(g)) = 274 S (O2(g)) = 209 S (CO2(g)) = 216 S (H2O(g)) = 181 ΔHfo (C3H8(g)) = -105 ΔHfo (CO2(g)) = -394 ΔHfo (H2O(g)) = -225
What is ΔGo (in kJ) at 647 K for the following reaction? PbO(g) + CO2(g) → PbCO3(s) PbO: ΔHfo = -219.0 kJ/mol and So = 66.5 J/K mol) PbCO3(s): ΔHfo = -699.1 kJ/mol and So = 131.0 J/K mol) CO2: ΔHfo = -393.5 kJ/mol and So = 213.6 J/K mol) At what temperature (in K) does the above reaction become spontaneous?