For a reaction at `25%(@)C, DeltaG^(@)=-33.3kJ and DeltaS= -198kJ xxK^(-1).` What is the value of `DeltaH%(@)?`

For a hypothetical reaction nX to mY , the value of DeltaH =-133 kJ and DeltaS = -145 J K^(-1) . Calcualte the value of DeltaG at 700 K.

DeltaG^(@) for a reaction 25^(@)C is 3.5kJ xx mol^(-1) . What is the value of K?

For a reaction DeltaG^@ = -51.4 KJ/mol and Delta H^@ = 49.4 KJ/mol at 300K, then value of DeltaS^@ in J/K is

For a gaseous reaction A+3BhArr 2C,DeltaH^(@)=-90.0kJ, DeltaS^(@)=-200.0jk^(-1) AT 400k. The DeltaG^(@) for the reaction (1)/(2)A+(3)/(2)B rarr C at 400K is :

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

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: