At what temperature the following process would not be spontanous ?
`4Fe(s)+3O_(2)(g)to2Fe_(2)O_(3)(s)`
`DeltaH=-1648 kJ//"mole"`
`DeltaS=-560 J//"mole"`

Justify that the following reactions are redox reactions : Fe_(2)O_(3)(s)+3CO(g)to2Fe(s)+3CO_(2)(g)

Justify the following reactions are redox reactions : Fe2O_(3)(s) +3CO(g)to2Fe(s)+3CO_(2)(g)

Determine DeltaS_(Total) and decide whether the following reaction is spontaneous at 298 K. Fe_2O_(3(s))+ 3CO_((g)) rarr 2Fe_(s) + 3CO_(2(g)) DeltaH^@ =- 24.8 kj, DeltaS^@ = + 15 JK^(-1)

Calculate standard molar entropy O_(2)(g) from the following thermodynamics data at 300 K : 4Cr(s)+3O_(2)(g)to2Cr_(2)O_(3)(s),DeltaG^(@)=-2093.4 " kJ"//mol DeltaH_(f)^(@)Cr_(2)O_(3)(s)=-1129.05" kJ"//"mole" S_(m)^(@)Cr(s)=24" J"//K" mole" S_(m)^(@)Cr_(2)O_(3)(s)=81" J"//K" mole"

Calculate the temperature above which the given reaction become spontaneous. C_((s)) + H_(2)O_((g)) rarr CO_((g)) + H_(2(g)) DeltaH^(@) = + 131.3 KJ//"mole" , DeltaS^(@) = + 0.1336 KJ//"mole" K

Calculate the temperature above which the given reaction become spontaneous. C_((s)) + H_(2)O_((g)) rarr CO_((g)) + H_(2(g)) DeltaH^(@) = + 131.3 KJ//"mole" , DeltaS^(@) = + 0.1336 KJ//"mole" K

How much heat is evolved by the preparation of 100 gm of iron by the following reaction ? 2Al(s)+Fe_(2)O_(3)(s)to2Fe(s)+Al_(2)O_(3)(s) , Delta_(r )H=-202.6 kcal/mol