`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.

The mass of oxygen required for the rusting of 4.2g of iron is (Fe = 56)

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.

C_((s))+O_(2(g))rarr CO_(2(g))+Q is ………………….

Given that S_((s)) + 3/2 O_(2(g)) rarr SO_(3(g)) + 2xK.cal SO_(2(g)) + ½ O_(2(g)) rarr SO_(3(g)) + y K.Cal . Which would be the enthalpy of formation SO_2 ?

Fe_(2)O_(3)+2Al rarr Al_(2)O_(3)+2Fe Name the compound which is oxidized in the above reaction.