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Part A Calculate AGxn at 298 K under the conditions shown below for the following reaction:...
Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = +326 kJ P(O2) = 0.20 atm, P(O3) = 0.038 atm kj = ?
Calculate Grxn at 298 K under the conditions shown below for the following reaction. 2 H2S(g) + 3 O2(g) 2 SO2(g) + 2 H2O(g) G°rxn = ? G°f (kJ/mol) -33.4 -300.1 -228.6 P(H2S) = 1.4 atm, P(O2) = 0.5atm P(SO2) = 2.2atm and P(H2O) = 0.8 atm
Calculate ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g) → 2 O3(g) ΔG° = +326 kJ P(O2) = 0.41 atm, P(O3) = 5.2 atm
4. Calculate ΔGrn at 298 K under the conditions shown below for the following reaction. 3 02g) 2 Os(g) P(O2) 0.41 atm, P(O) 5.2 atm AGo +326 kJ a. +341 kJ b. +17.8 kJ c. +332 kJ d. -47.4 kJ e. -109 kJ
Use Hess' law and the data below to calculate AG, in kJ, for the following reaction: NO(g) + O (9) NO2 (g), AG° = ? 2 03 (9) - 3 O2 (g), AG° = +489.6 kJ 02 (9) 20 (9), AGⓇ = +463.4 kJ NO(g) + O2 (9) - NO2 (g) + O2 (g), AG° = -199.5 kJ QUESTION 14 Calculate AG for the following reaction, in kJ, at 0 °C under the following non-standard conditions shown below. 2 Hgo...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(g) 2 NO ( g ) + O 2 ( g ) ↽ − − ⇀ 2 NO 2 ( g ) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol Δ G ° = − 72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.300 atm P NO...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(g) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.500 atm , ?O2=0.400 atm , and ?NO2=0.750 atm ?
Calculate ΔGron (kl) at 298 K under the conditions shown below for the following reaction. SO3lg)+ H20(e) -H2SO4() AG--90.5kJ P(SO3)-0.20 atm, P(H20)-0.88 atm Input your answer with one decimal place. No unit
Under the conditions shown below for the following reaction. Fe2O3(s) + 3 CO(g) - 2 Fe(s) + 3 CO2(g) AG° = -28.0 kJ P(CO) - 3.1 atm, P(CO2) - 1.7 atm Calculate Arxn at 298 K, and indicate if the reaction is more or less spontaneous under these conditions than under standard conditions? -4.5 kJ, more spontaneous than under standard conditions None of these -4.5 kJ, less spontaneous than under standard conditions -23.5 kJ, more spontaneous than under standard conditions...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction the standard change in Gibbs free energy is delta G degree = -72.6 kJ/mol. What is delta G for this reaction at 298 K when the partial pressures are PNO = 0.l00 atm, PO2 = 0.150 atm, and PNO2 = 0.650 atm Number delta G = kJ/mol