For a particular reaction at 128.7 °C, deltaG = – 784.97 kJ/mol, and deltaS = 676.82 J/(mol · K). Calculate deltaG for this reaction at - 77.1 °C.
For a particular reaction at 128.7 °C, deltaG = – 784.97 kJ/mol, and deltaS = 676.82...
Ag2S given DeltaH= -32 kj/mol, DeltaG=-40 kj/mol DeltaS= 146 j/k*mol calculate Gibbs free energy for the reaction of dissolving silver sulfide, Ag2S, in water (25 C.) Do the calculations in two ways. Use the standard Enthalpy of formation, deltaH, and entropy S values, and the formula deltaG=deltaH-TdeltaS. Use the standard free energies of formation deltaG and the formula deltaG=deltaG(products)-deltaG(reactants).
Consider the decomposition of CaCO3 at standard conditions: CaCO3(s) >> CO2(g) + CaO(s) DeltaH=177.8 KJ/mol, DeltaS=160.5 J/K mol, DeltaG=130.3 KJ/mol, K=1.506x10^-23, Nonspontaneous until temp 1107.8 K or higher. What is the new concentration of CO2 at nonstandard temperature (1107.8k)?
Consider the decomposition of CaCO3 at standard conditions: CaCO3(s) >> CO2(g) + CaO(s) DeltaH=177.8 KJ/mol, DeltaS=160.5 J/K mol, DeltaG=130.3 KJ/mol, K=1.506x10^-23, Nonspontaneous until temp 1107.8 K or higher. What is the new concentration of CO2 at nonstandard temperature (1107.8k)?
For a particular reaction at 203.3 °C, AG = 424.99 kJ/mol, and AS - 551.38 J/mol K). Calculate AG for this reaction at -66.6 °C. AG = kJ/mol What is the value of K for this aqueous reaction at 298 K? A + B =C+D AG° = 11.80 kJ/mol
For a particular reaction at 239.1 °C, AG = 363.40 kJ/mol, and AS = 739.34 J/mol. K). Calculate AG for this reaction at -19.0 °C. AGE 554.22 kJ/mol
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.
What is the value of k for this aqueous reaction at 298 K? A+B<——>C+D. DeltaG=15.23 kJ/mol
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 124.8 °C, Δ?=−841.80 kJ/mol , and Δ?=646.52 J/(mol⋅K) . Calculate ΔG for this reaction at 11.9 °C.