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 ΔGrxn at 298 K under the conditions shown below for the following reaction. 3 O2(g)...
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
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
Part A Calculate AGxn at 298 K under the conditions shown below for the following reaction: AGⓇrx = -180.8 kJ 2 Hg (g) + O2(g) → 2 Hgo (s) PiHg) = 0.153 atm, P02) = 0.107 atm +808 kJ 0-166 kJ O-154 kJ +14.7 kJ 0 -171 kJ Submit Request Answer
Please show all work A.)Choose the statement below that is TRUE. a.If K < 1, the reaction is spontaneous in the forward direction. b. If K < 1, the reaction is spontaneous in the reverse direction. c, If K < 1, the reaction is at equilibrium. d. Not enough information is given. B.)Place the following in order of decreasing molar entropy at 298 K. H2 Cl2 F2 a. H2 > F2 > Cl2 b. H2 > Cl2 > F2 c....
Consider this reaction at 298 K: H2 (g) + I2 (g) ⇌ 2 HI(g) Calculate ΔGrxn under the following conditions: PH2 (g) = 0.161 atm PI2 (g) = 0.186 atm PHI(g) = 0.307 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
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...
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...
Calculate Δ G for the reaction 2 SO2 (g) + O2 (g) → 2 SO3 (g) when P of SO2 = 0.500 atm, P of O2 = 0.0100 atm, and P of SO3 = 0.100 atm. The value for Δ G^o for this reaction at 298 K is -141.6 kJ. ΔG = ???? kJ I got -160.9 kj but it is incorrect.