Calculate ΔGºrxn for a chemical reaction with ΔHºrxn = 778 kJ/mol and ΔSºrxn = 145 J/mol·K at 298K. ΔGºrxn =__________kJ/mol
Calculate ΔGºrxn for a chemical reaction with ΔHºrxn = 778 kJ/mol and ΔSºrxn = 145 J/mol·K...
For a particular reaction at 209.8 °C, ΔG = -318.09 kJ/mol, and ΔS = 994.40 J/(mol·K). Calculate ΔG for this reaction at -58.2 °C.
For a particular reaction at 134.8 °C, ΔG = -1319.75 kJ/mol, and ΔS = 863.35 J/(mol·K). Calculate ΔG for this reaction at -79.1 °C.
For a particular reaction at 139.3 °C, ΔG = 354.61 kJ/mol, and ΔS = 658.46 J/(mol·K). Calculate ΔG for this reaction at -55.9 °C.
A reaction has ΔHºrxn = –201 kJ/mol and ΔSºrxn=-394 J/mol·K. Below what temperature is the reaction spontaneous?
A reaction has ΔHºrxn = –201 kJ/mol and ΔSºrxn=-282 J/mol·K. Below what temperature is the reaction spontaneous? Spontaneous below _________ °C.
A certain reaction has ΔH°= -19.5 kJ/mol and ΔS°= +42.7 J/mol K a) Is the reaction exothermic or endothermic? b) Does the reaction lead to an increase or decrease in the disorder of the system? c) Calculate ΔG° for the reaction at 298K. d) Is the reaction spontaneous at 298 K under standard conditions?
a) calculate the standard reaction entropy (in J K-1 mol-1) at 298K for the complete combustion of sucrose. b) Calculate the standard Gibbs reaction energy (in kJ mol-1) for the reaction
For a particular reaction at 205.1205.1 °C, ΔG=−45.90 kJ/molΔG=−45.90 kJ/mol, and ΔS=395.61 J/(mol⋅K)ΔS=395.61 J/(mol⋅K). Calculate ΔG for this reaction at −6.1−6.1 °C.
For a particular reaction at 212.3 °C, AG = -889.99 kJ/mol, and AS = 385.90 J/(mol · K). Calculate AG for this reaction at -2.8 °C. AG= 193.97 kJ/mol
For a particular reaction at 172.4 °C, Δ?=−269.73 kJ/mol ΔG=−269.73 kJ/mol, and Δ?=970.33 J/(mol⋅K) Calculate ΔG for this reaction at 14.3 °C.