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

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

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 given reaction, DeltaH=35.5kJ*mol^(-1) and DeltaS=83.6J*mol^(-1) . The reaction is spontaneous at (assume that DeltaH and DeltaS do not vary with temperature)-