Answer:
0.22L of H2
Explanation:
We'll begin by writing the balanced equation for the reaction. This is given below:
Fe3O4 + H2 —> 3FeO + H2O
Next, we shall determine the number of mole present in 2.3g of Fe3O4. This is illustrated below:
Molar mass of Fe3O4 = (56x3) + (16x4) = 232g/mol
Mass of Fe3O4 = 2.3g
Mole of Fe3O4 =..?
Mole = Mass/Molar Mass
Mole of Fe3O4 = 2.3/232 = 9.91x10^-3 mole.
Next, we shall determine the number of mole H2 needed for the reaction. This is illustrated below :
From the balanced equation above,
1 mole of Fe3O4 reacted with 1 mole of H2.
Therefore, 9.91x10^-3 mole of Fe2O3 will also react with 9.91x10^-3 mole of H2.
Finally, we can obtain the volume of H2 required for the reaction as follow:
1 mole of a gas occupy 22.4L at stp.
Therefore, 9.91x10^-3 mole of H2 will occupy = 9.91x10^-3 x 22.4 = 0.22L
Therefore, 0.22L of H2 is required for the reaction.
