At what temperature (in K) does the following reaction become spontaneous, if Δ𝐻∘ = 311.1 kJ/mol and Δ𝑆∘ = 707.3 J/mol*K?

For a reaction, H0 = 206 kJ/mol and S0 = 0.215 kJ/(K•mol). At what temperatures is this reaction spontaneous?A.At no temperatureB.At temperatures greater than 958 KC.At all temperaturesD.At temperatures less than 44 K

At which temperature would a reaction with H = -92 kJ/mol, S = -0.199 kJ/(molK) be spontaneous?A.400 KB.500 KC.600 KD.700 KSUBMITarrow_backPREVIOUS

Consider a specific reaction with ΔH° = 66.8 kJ/mol and ΔS° = 105.3 J/mol•K. Assuming that these values do not change with temperature, at what temperature range is the reaction spontaneous in the forward direction?The reaction is spontaneous for temperatures (less than, greater than) T = ________ K.

What can be said about a reaction with H = 62.4 kJ/mol and S = 0.145 kJ/(mol·K)?A.It is spontaneous at 500 K.B.It is spontaneous at 298 K.C.It is never spontaneous.D.It is always spontaneous.

For the reactionA + B → Ccalculate ΔG in kJ.mol–1 at temperature 298 K using the following thermochemical data for the reaction:ΔH = –51.2 kJ.mol–1 ΔS = 126 J.mol–1.K–1. Enter your answer to 3 significant figures. Do not include units. Include the sign.Is this reaction spontaneous?