Using listed informations, calculate `Delta_(r)G^(@)` (in kJ/mol) at `27^(@)C`
`Co_(3)O_(4)(s)+4CO(g)rarr3Co(s)+4CO_(2)(g)`
Given : At 300 K `DeltaH_(f)^(@)(kJ//mol)-891,-110.5,0.0,-393.5`
`S^(@)(J//K-mol)102.5, 197.7, 30.0, 213.7`

Calculate Delta_(r) H^(@) for Fe_(2) O_(3) (s) + 3 CO(g) to 2 Fe (s) + 3 CO_(2) (g) Given : Delta_(f) H^(@) (Fe_(2) O_(3) , s) = -822.2 kJ/mol Delta_(f) H^(@) (CO , g) = -110.5 kJ//mol , Delta_(f) H^(@) (CO_(2) , g) = -393.5 kJ/mol

Calculate the standard enthalpy of reaction ZnO(s)+CO(g)rarrZn(s)+CO_(2)(g) Given, Delta H_(f)(ZnO,s)=-350KJ//"mole",DeltaH_(f)^(@)(CO_(2),g)= -390KJ//"mole", DeltaH_(f)^(@)(CO,g)=-110KJ//"mole"

Calculate the standard enthalpy of reaction ZnO(s)+CO(g)rarrZn(s)+CO_(2)(g) Given, Delta H_(f)(ZnO,s)=-350KJ//"mole",DeltaH_(f)^(@)(CO_(2),g)= -390KJ//"mole", DeltaH_(f)^(@)(CO,g)=-110KJ//"mole"

Calculate Delta_(f)H^(@) for the reaction, CO_(2)(g) + H_(2)(g) to CO(g) + H_(2)O(g) Given that Delta_(f)H^(@) for CO_(2)(g) , CO(g) and H_(2)O(g) are -393.5, -111.3 and -241.8 kJ mol^(-1) respectively.

Calculate Delta_(f)H^(@) (in kJ/mol) for Cr_(2)O_(3) from the Delta_(r)G^(@) and the S^(@) values provided at 27^(@) 4Cr(s)+3O_(2)(g)rarr2Cr_(2)O_(3)(s)," "Delta_(r)G^(@)=-2093.4kJ//mol S^(@)("J//K mol") : S^(@)(Cr,s)=24," "S^(@)(O_(2),g)=205," "S^(@)(Cr_(2)O_(3),s)=81

Calculate Delta_(f)H^(@) (in kJ/mol) for Cr_(2)O_(3) from the Delta_(r)G^(@) and the S^(@) values provided at 27^(@) 4Cr(s)+3O_(2)(g)rarr2Cr_(2)O_(3)(s)," "Delta_(r)G^(@)=-2093.4kJ//mol S^(@)("J//K mol") : S^(@)(Cr,s)=24," "S^(@)(O_(2),g)=205," "S^(@)(Cr_(2)O_(3),s)=81

The fat, C_(57)H_(104)O_(6)(s) , is metabolized via the following reaction. Given the enthalpies of formation, calculate the energy (kJ) liberated when 1.0 g of this fat reacts. C_(57)H_(104)O_(6)(s)+80 O_(2)(g)rarr57CO_(2)(g)=-52 H_(2)O(l) Delta_(f)H^(@)(C_(57)H_(104)O_(6),s)=-70870" kJ"//"mol, "Delta_(f)H^(@)(H_(2)O,l)=-285.8 " kJ"//"mol" , Delta_(f)H^(@)(CO_(2),g)=-393.5 " kJ"//"mol"

The fat, C_(57)H_(104)O_(6)(s) , is metabolized via the following reaction. Given the enthalpies of formation, calculate the energy (kJ) liberated when 1.0 g of this fat reacts. C_(57)H_(104)O_(6)(s)+80 O_(2)(g)rarr57CO_(2)(g)+52 H_(2)O(l) Delta_(f)H^(@)(C_(57)H_(104)O_(6),s)=-70870" kJ"//"mol, "Delta_(f)H^(@)(H_(2)O,l)=-285.8 " kJ"//"mol" , Delta_(f)H^(@)(CO_(2),g)=-393.5 " kJ"//"mol"