When iron is heated in oxygen, it forms ferroso ferric oxide `(Fe_3O_4)`.

Write a balanced chemical equation with state symbols for the following reaction : Heated iron metal reacts with steam to iron oxide (Fe3O4) and hydrogen.

Translate the following statements into chemical equation and balance the equations : aluminium metal replaces iron from ferric oxide (Fe2O3) giving aluminium oxide and iron.

Calculate the mass of iron required to be converted into its oxide (Fe_3O_4) by the action of 23.4 g of steam on it .

When steam is passed over hot iron, hydrogen is liberated and Fe_(3)O_(4) is formed according to the chemical equation 3 Fe + 4 H_(2)O to Fe_(3)O_(4) + 4 H_(2)(g) . In a typical reaction, 56 g iron was consumed. Calculate the following: The mass of Fe_(3)O_(4) formed. (R.A.M. : H = 1, O = 16, Fe = 56)

Calculate the mass of iron which will be converted into its oxide ( Fe_3O_4 ) by the action of 8g of steam on it. [At mass of Fe=56] Fe+H_2​O→Fe_3O_4+4H_2 ​

Calculate the mass of iron which will be converted into its oxide ( Fe_3O_4 ) by the action of 17g of steam on it. [At mass of Fe=56] Fe+H_2​O→Fe_3O_4+4H_2 ​