For a reaction, `DeltaH=10000" kJ "mol^(-1) and DeltaS=25" kJ "k^(-1)mol^(-1)`. The minimum temperature, above which the reaction would be spontaneous is

A process has DeltaH=200Jmol^(-1) and DeltaS=40JK^(-1)mol^(-1) . The minimum temperature above which the process will be spontaneous is ___________K.

A process has DeltaH=200Jmol^(-1) and DeltaS=40JK^(-1)mol^(-1) . The minimum temperature above which the process will be spontaneous is ___________K.

The value of DeltaH and DeltaS for a reaction are respectively 30 kJ mol^(-1) and 100JK^(-1)mol^(-1) . Then temperature above which the reaction will become spontaneous is:

The values of DeltaH and DeltaS for a reaction are respectively "30 kJ mol"^(-1) and 100 KJ^(-1) mol^(-1) . Then the temperature above which the reaction will become spontaneous is ____

For the reaction at 298 K : 2A +B to C DeltaH="400 KJ mol"^(-1) , DeltaS ="0.2 JK"^(-1) "mol"^(-1) Determine the temperature at which the reaction would be spontaneous .