Given `Delta_(r)S^(@)=-266` and the listed `[S_(m)^(@)value]` Calculate `S^(@) "for" Fe_(3)O_(4)(s)`
`4Fe_(3)O_(4)(s)[...] +O_(2)(g)[205] to6Fe_(2)O_(3)(s)[87]`

Fe_(2)O_(2)(s)+(3)/(2)C(s)to(3)/(2)CO_(2)(g)+2Fe(s) DeltaH^(@)=+234.12KJ C(s)+O_(2)(g)toCO_(2)(g) DeltaH^(@)=-393.5KJ Use these equations and DeltaH^(@) value to calculate DeltaH^(@) for this reaction : 4Fe(s)+3O_(2)(g)to2Fe_(2)O_(3)(s)

What is the value of Delta s^(@) for the reaction below? Fe_(2)O_(3)(s)+3CO(g)to2Fe(s)+3CO_(2)(g)

Fe(s)+H_(2)O(l) overset(Boil) to Fe_(3)O_(4)+H_(2)uarr

Write a balanced chemical equation : FeSO_(4)(s) overset("Heat")to Fe_(2)O_(3)(s) +SO_(2)(g) +SO_(3)(g)

Balance the following chemical eqution: Fe(s)+H_(2)O(g)rarrFe_(3)O_(4)(s)+H_(2)(g)

Consider the following reactions. DeltaH^(@) values of the reactions hve been given as -x, -y and z kJ. Fe_(3)O_(4)(s) to 3Fe(s) + 2O_(2)(g), DeltaH^(@) = z kJ 2Fe(s) + O_(2)(g) to 2FeO(s), DeltaH^(@) =-x kJ 4Fe(s) + 3O_(2)(g) to 2Fe_(2)O_(3)(s), DeltaH^(@) =-y kJ Heat of reaction for the reaction, FeO(s) + Fe_(2)O_(3)(s) to Fe_(3)O_(4)(s) is :

Consider the following reactions. DeltaH^(@) values of the reactions hve been given as -x, -y and z kJ. Fe_(3)O_(4)(s) to 3Fe(s) + 2O_(2)(g), DeltaH^(@) = z kJ 2Fe(s) + O_(2)(g) to 2FeO(s), DeltaH^(@) =-x kJ 4Fe(s) + 3O_(2)(g) to 2Fe_(2)O_(3)(s), DeltaH^(@) =-y kJ In the given set of reaction, -x//2 kJ refers to