Calculate the minimum temperature required for a reaction to be spontaneous if `DeltaS` = 27J/mol and `DeltaH` = 80KJ/mol

Assume DeltaH^(@) and DeltaS^(@) to be independent of temperature, at what temperature with the reaction given below becomes spontaneous? N_(2)(g) + O_(2)(g) to 2NO(g) DeltaH^(@) = 180.8 kJ mol^(-1)

A reaction has a value of DeltaH = -64.5 kJ at 157^(@)C . Above 157^(@)C , the reaction is spontaneous and below this temperature the reaction is not spontaneous.Calculate the value of DeltaG and DeltaS at 157^(@)C .

For the reaction at 298 K 2A+B rarr C DeltaH=400 kJ mol^(-1) and DeltaS=0.2 kJ K^(-1) mol^(-1) At what temperature will the reaction becomes spontaneous considering DeltaH and DeltaS to be contant over the temperature range.

For the reaction at 300 K, 2A + B to C Delta H = 450 kJ mol^(-1) and DeltaS = 0.2 kJ K^(-1) mol^(-1) .At what temperature will the reaction become spontaneous considering DeltaH and DeltaS to be constant over the temperature range?

For the reaction at 298 K 2A + B to C DeltaH = 40 kJ "mol"^(-1) and DeltaS = 0.2 kJ K^(-1) "mol"^(-1) . At what temperature will the reaction beccomes sponatneous considering DeltaH and DeltaS to be constant over the temperature range.

The temperature in K at which DeltaG=0 for a given reaction with DeltaH=-20.5 kJ mol^(-1) and DeltaS=-50.0 JK^(-1) mol^(-1) is

Consider the reaction for the dissolution of ammonium nitrate : NH_(4)NO_(3)(s) to NH_(4)^(+)(aq) + NO_(3)^(-)(aq) DeltaH = +28.1 kJ mol^(-1), DeltaS = 108.7 J K^(-1)mol^(-1) . Calculate the change in entropy of the surroundings and predict whether the reaction is spontaneous or not at 25^(@)C ?