Question

What volume of STP required to reduce 1 mole of fe2o3 in the following fe2o3 + co - fe + co2

Answer 1

The reaction taking place is as follows:
         Fe2O3 + 3CO → 2Fe + 3CO2
Given,
    Number of moles of Fe2O3 = 0.25 mole
From the above balanced equation,
    1 mole of Fe2O3 needs 3 moles of CO
Therefore,
    0.25 mole of Fe2O3 will need x moles of CO
i.e.,
    1/0.25 = 3/x
Solving, we get
     x = 0.075 moles of CO 
     Molar mass of CO = 28.01 g/mol
Thus,
     Mass of CO     = (0.075 moles) x (28.01 g/mol)
                             = 2.1 g
     Density of CO = 0.001250 g/cm3
Hence,
     Volume of CO required = (2.1 g) / (0.001250 g/cm3)
                                            = 1680 cm3
                                            = 1680 mL = 1.680 L