A reaction has `DeltaH=-33kJ and DeltaS=-58J//K`. This reaction would be:

A reaction has DeltaH=-33KJ and DeltaS=-58(J)/(H) . This reaction would be:

For a particular reaction, DeltaH=-38.3 kJ and DeltaS^(@)=-113JxxK^(-1). This reaction is:

Suppose that a reaction has DeltaH=-40kJ and DeltaS =- 50J//K . At what temperature range will it change from spontaneous to non-spontaneous?

Suppose that a reaction has DeltaH=-40kJ and DeltaS =- 50J//K . At what temperature range will it change from spontaneous to non-spontaneous?