`Al_((s))+Fe_(2)O_(3(s))rarrAl_(2)O_(3(s))+Fe_((s))`
`54_((g))+160_(g)rarr 102g+112`
was given, Then, the amount of aluminium required to get 1120 grams of iron is

Fe_(2)O_(3(s))+2Al_((s))rarr 2Fe_((s))+Al_(2)O_(3(s)) is a/an …………….

Al_(s) + Fe_2O_3(s) rarr Al_2O_3(s) + Fe_(s) (atomic masses of Al = 27 U Fe = 56 U and O = 16 U).Suppose that you are asked to calculate the amount of aluminium, required to get 1120 kg of iron by the above equation.

Al_((s)) + fe_(2)O_(3(s)) to Al_(2) O_(3(s)) + Fe_((s)) (atomic masses of Al = 27U, Fe = 56U, and O = 16U) 2Al_((s)) +Fe_(2)O_(3(s)) to Al_(2)O_(3(s)) + 2Fe_((s)) , is a balanced equation. (2 xx 27)U + (2xx 56 + 3xx 16)U to (2xx 27 + 3 xx 16) U + (2 xx 56) U {:(54U+160U,,to102U+112U),(or2" mol" + "1 mol",,to 1"mol" + 2"mol"),(54g + 160g ,, to 102 g + 112 g):} Suppose that your asked to calculate the amount of aluminium, required to get 1120 kg of iron by the above reaction.

If DeltaG = - 177 K cal for (1) 2 Fe(s) + (3)/(2)O_(2)(g) rarr Fe_(2)O_(3)(s) and DeltaG = - 19 K cal for (2) 4 Fe_(2)O_(3)(s) + Fe(s) rarr 3 Fe_(3)O_(4) (s) What is the Gibbs free energy of formation of Fe_(3)O_(4) ?

Calculate the amount of aluminium, required to get 1120 kg of iron from the given chemical equation. 2Al_((s))+Fe_(2)O_(3(s))rarrAl_(2)O_(3(s))+Fe_((s))" " (atomic mass of Al = 27U, Fe = 58U and O = 16 U)

Balance the following chemical equations. ii) Fe_(2)O_(3(s))+C_((s))rarr Fe_((s))+CO_(2(g))

Select (i) combination reactions (ii) decomposition reactions and displacement reactions from the following (i) ZnCO_(3)(s) to ZnO(s) + CO_(2)(g) (ii) Pb(s) + CuCl_(2)(aq) to PbCl_(2)(g) + Cu(s) (iii) H_(2)(g) + Cl_(2)(g) to 2HCl(g) (iv) Fe_(2)O_(3)(s) + 2Al(s) to Al_(2)O_(3)(s) + 2Fe(s) (v) 3H_(2)(g) + N_(2)(g) to 2NH_(3)(g) (vi) CaCO_(3)(g) overset("heat")to CaCO_(3)(g) + CO_(2)(g)