d) For the process of potassium chlorate decomposition: 2KClO_(3)arrow 2KCl+3O_(2) Delta _(f)H^0_(298)=-89.38kJ/mol and Delta _(r)S_(200)^0=349.51J/moltimes K Calculate Delta G_(298)^0 at 298K and make the conclusion about spontaneity of this reaction.

To calculate the change in Gibbs free energy ( ) for the decomposition of potassium chlorate at 298K, we can use the following equation: where: is the change in enthalpy at 298K, is the temperature in Kelvin, and is the change in entropy at 298K.Given that and , we can substitute these values into the equation: Since is negative, the reaction is spontaneous at 298K.