Using the standard entropy values: NOG), S = +210.6 J mol-1 K-1 02(0), sº = +205.0...
Using the standard entropy values:SO2(g), So = +248.0 J mol–1 K–1SO3(g), So = +256.0 J mol–1 K–1NO(g), So = +210.6 J mol–1 K–1NO2(g), So = +240.5 J mol–1 K–1calculate the standard entropy change, ?So, for the reaction:NO2(g) + SO2(g) ? NO(g) + SO3(g)Enter your answer in J mol-1 K-1 to one decimal place. Do not enter units.Thanks so much!
Pi T2 = P₂ T 12) Calculate the standard free energy change at 25°C for the reaction 2 NO(g) + O2(g) → 2 NO2(g). 12 46°E AH-TAS Species | AHºf, kJ/mol NO () 91.3 02 (8) 0.0 NO2 (8) 5, J/(K.mol) 210.7 205.0 240.0 33.2 A) -4.7 kJ (B) -72.6 kJ C) -157.8 kJ D) -532.6 kJ 13) The Boltzmann formula is S=k In W. A perfect crystal has a molar entropy of 0 at absolute zero because A) W=NA...
Calculate the standard free energy change at 25°C for the reaction 2 NO(g) + O2(g) → 2 NO2(g). Species ΔH°f, kJ/mol S°, J/(K · mol) NO (g) 91.3 210.7 O2 (g) 0.0 205.0 NO2 (g) 33.2 240.0 A) -157.8 kJ B) -532.6 kJ C) -72.6 kJ D) -4.7 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...
Calculate the standard entropy change for the reaction2Mg(s)+O2(g)→2MgO(s)using the data from the following table:Substance△ Hf (kJ/mol)△Gf (kJ/mol)S0 [J/(K/mol)]Mg(s)0.000.0032.70O2(g)0.000.00205.0MgO(s)-602.0-569.627.00Express your answer to four significant figures and include the appropriate units.
Calculate the standard entropy change for the reaction P4(g)+5O2(g)→P4O10(s) using the data from the following table: Substance ΔH∘f (kJ/mol) ΔG∘f (kJ/mol) S∘ [J/(K⋅mol)] P4(g) 58.9 24.5 279.9 O2(g) 0 0 205.0 P4O10(s) −2984 −2698 228.9
Nitrogen Ahºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 191.6 N2(9) 0 0 N(g) 472.7 455.6 153.3 NH3(g) -46.1 -16.5 192.5 NH3(aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 90.3 86.6 210.8 NO(9) NOCI(g) 51.7 66.1 261.8 NO2(g) 33.2 51.3 240.1 N20(9) 82.1 104.2 219.9 N204(9) 9.2 97.9 304.3 N204(0) -20.0 97.0 209.0 N205(s) -42.0 134.0 178.0 N2H4(0) 50.6 149.3 121.2 N2H3CH3 () 54.0 180.0 166.0 HNO3(aq) -207.4 -111.3 146.4 HNO3(1) -174.1 -80.7 155.6 HNO3(9) -135.1 -74.7 266.4 NH4ClO4(s) -295.0...
The standard entropy change for the reaction 302() 203() is -137.2 J/K mol at 298 K and 1 bar. Calculate the value of AS rx at 460 K, assuming that all values are independent of temperature. [ACP,ran for this reaction is -9.8 kJ/K mol).] Г ЈК - mol
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
ANSWER EACH QUESTION AND SHOW WORK 4) Using the accompanying data, calculate the standard entropy changes for the following reactions at 25 °C: MgCo. (s) → MgO (s) + CO2 AS(/K-moll) 65.69 2 6.78 213.6 AS (J/K-mol) 2 CH. () + 70, (g) → 4CO2(g) + 6H20 (1) 172.8 205.0 213.6 69.9 5) Calculate the free energy change for this reaction at 25°C. Is the reaction spontaneous? 2 Ca (s) + 02 (g) + 2 Cao (s) AH = -1269.8...