Identify the correct set of statements for ( S _ Total =-80 KJ K ⁻¹ ~mol ⁻¹, H _ System =4000 ~kJ ~mol ) Temperature (=800 ~K ) (a) ( G =+64000 KJ mol ⁻¹ ) (b) ( S _ System =+75 KJ mol ⁻¹ ) (c) Reaction is non-spontaneous (d) Reaction is spontaneous Choose the correct answer from the options given below:

Step-by-step solution

To determine the correct set of statements, we can use the Gibbs free energy equation: ( G= H-T S_ Total ) Given: - ( H_ System =4000, ~kJ / mol ) - (T=800, ~K ) - ( S_ Total =-80, ~kJ / K / mol ) Calculate ( G ) ( G=4000 ~kJ / mol -(800 ~K -80 k ) Calculating (T S_ Total ) : (T S_ Total =800 -80=-64000 ~kJ / ) Now substitute back into the Gibbs equation: ( G=4000+64000=68000 ~kJ / mol ) Analyze the statements - (a) ( G=+64000, ~kJ / mol ) : Incorrect (it should be (+68000 ~kJ / mol )). - (b) ( S_ System =+75, ~kJ