The factor of AG values is important in metallurgy. The AG values for the following reactions at 800°C are given as; S2(s) +202(9) ► 2502(g); AG = -544 kJ 2Zn(s) + Sz(s) → ZnS(s); AG = - 293 kJ 2Zn(s) + O2(g) → ZnO(s); AG = - 480 kJ Then AG for the reaction : 2ZnS(s) + 302(g) → ZnO(s); 2502 (9) Will be:

The DeltaG values for the following reactions at 800^(@)C are S_(2)(g) + 2O_(2)(g) to 2SO_(2)(g) DeltaG = - 544 kJ 2Zn (s) + S_(2)(g) to 2ZnS(s) DeltaG = - 293 kJ 2Zn(s) + O_(2)(g) to 2ZnO(S) DeltaG = - 480 kJ The DeltaG for the reaction: 2ZnS(s) + 3O_(2)(g) to 2ZnO(s) + 2SO_(2)(g) is

The factor of DeltaG values is important in metallurgy. The DeltaG values for the following reactions at 800°C are given as : S_(2)(s) + 2O_(2)(g) to 2SO_(2)(g), DeltaG =-544 kJ 2Zn(s) + S_(2)(s) to 2ZnS(s), DeltaG=-293 kJ 2Zn(s) + O_(2)(g) to 2ZnO(s), DeltaG = -480 kJ Calculate the DeltaG for the reaction: 2ZnS(s) + 3O_(2)(g) to 2ZnO(s) + 2SO_(2)(g)

Classify each of the following reactions Zn(s)+2AgNO_3 (aq) gives Zn(No_3)_2 (aq)+2Ag(s)

In thebutton cells widely used in watches and other devices the following reaction takes place: Zn (s) + Ag_2O (s) + H_2O(I) --Zn^(2+) (aq) + 2Ag (s) + 2OH-(aq) Determine Delta_rG^0 and E^0 for the reaction.

The equilibrium constant for the reaction, Ag_2O(s) hArr2Ag(s) +1/2 O_2 (g) is given by

The equilibrium constant for the reaction, Ag_2O(s) hArr2Ag(s) +1/2 O_2 (g) is given by

In the button cells widely used in watches and other devices the following reaction takes place: Zn(s) + Ag_2O(s) + H_2O(l) rarr Zn^(2+)(aq) + 2Ag(s) + 2OH^(-) . Determine Delta_rG^@ and E^@ for the reaction.