a$)$ Calculate the value of standard molar Gibbs free energy change of chemical reaction at $298K$ using the data given below:

Is the chemical reaction exothermic reaction or endothermic? WHY?

$\frac{4}{3}Al(s)+O_2(g)\frac{2}{3}A{l}_2{O}_3(g)at298K$

b$)$ Calculate the enthalpy and entropy of chemical reaction at $1000K.$ Leave calculations in the integral form after putting $cp$ values. Organize them as we do it in the class.

$\frac{4}{3}Al(l)+O_2(g)\frac{2}{3}A{l}_2{O}_3(g)at1273K$

DATA:

$HAl(s1)=10500$ joules at $932K,$

Standard molar enthalpy formation and entropy at $298K$ :

$H_{f}A{l}_2{O}_3=-1674000$ joules,

$SAl(s)=28\mathrm{.}3\frac{J}{K},SA{l}_2{O}_3=59\mathrm{.}6\frac{J}{K},S{O}_2=205\frac{J}{K}$