The rusting of iron is formulated as `Fe_(2)O_(3)*xH_(2)O` which involves the formation of:

The rusting of iron occurs as 4Fe(s)+3O_(2)(g)to 2Fe_(2)O_(3)(s) . Enthalpy of formation of Fe_(2)O_(3)(s) is -824.2 kJ mol^(-1) and entropy change for the reaction, i.e., Delta S_("system") , is -549 J K^(-1) mol^(-1) . Calculate Delta S_("surrounding") and predict whether rusting of iron is spontaneous or not at 298 K.

The brown ring complex compound of iron is formulated as [Fe (H_(2)O)_(5) (NO)] SO_(4) . The oxidation state of iron is

The brown ring complex compound is formulated as [Fe(H_(2)O)_(5)(NO)]SO_(4) . The oxidation state of iron is :

The brown - ring complex compound of iron is formulated as [Fe(H_2O)_5(NO)]SO_4 . The oxidation state of iron is :

The chemical formula of rust is Fe_(3)O_(4).xH_(2)O

T/F Rust is Fe_2O_3. xH_2O

The formula of Gibsite is Al_(2)O_(3), xH_(2)O there 'x' is