Add 50ml 2mol / L H2SO4 solution to the mixture of Fe3O4 and Fe in a certain amount, and just dissolve the mixture completely under certain conditions, releasing 448ml (under standard conditions) gas. Add KSCN solution to the resulting solution, and there is no red. Then fully react with the mixture of the same mass with sufficient CO at high temperature, and what is the mass of iron?

Add 50ml 2mol / L H2SO4 solution to the mixture of Fe3O4 and Fe in a certain amount, and just dissolve the mixture completely under certain conditions, releasing 448ml (under standard conditions) gas. Add KSCN solution to the resulting solution, and there is no red. Then fully react with the mixture of the same mass with sufficient CO at high temperature, and what is the mass of iron?

[the idea of solving this problem is to determine the quality of the final reduced Fe, then determine the amount of Fe element in the mixture] the amount of sulfuric acid participating in the reaction n (H2SO4) = 0.05 * 2 = 0.10 (mol) from the relationship Fe ~ H2SO4 ~ H2, it is known that n (H2) = 0.448 / 22.4 = 0.02 (mol), so N1 in the first part