Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains...

Iron(III) oxide reacts with carbon monoxide according to the equation:
Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)
A reaction mixture initially contains 23.00 g Fe2O3 and 16.00 g CO.

Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?

Solutions

Expert Solution

Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)

no of moles of Fe2O3 = W/G.M.Wt

= 23/159.69 = 0.144 moles

no of moles of CO = W/G.M.Wt

= 16/28 =0.57 moles

Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g)

1 mole of Fe2O3 react with 3 moles of CO

0.144 moles of Fe2O3 react with = 3*0.144/1 = 0.432 moles of CO

CO is excess reactant

The no of moles of excess reactant left after complete the reaction = 0.57-0.432 = 0.138 moles

The amount of excess reactant left after complete the reaction = no of moles * gram molar mass

= 0.138*28 = 3.864g of CO >>answer

queen_honey_blossom answered 1 year ago

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