Question

In: Chemistry

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 2 years ago
Next > < Previous

Related Solutions

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 22.25 g Fe2O3and 14.18 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?
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 22.90 g Fe2O3 and 15.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant is left?
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 22.10 g Fe2O3 and 14.00 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains? Express your answer to three significant figures. Suppose that in an alternate universe, the possible values of l were the integer values from 0 to n(instead of 0 to n−1). Assuming no other differences from this universe, how many...
(Sig Figs) Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture...
(Sig Figs) Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) A reaction mixture initially contains 22.20 g Fe2O3 and 14.00 g CO. The online website said the answer is m = 2.32g ( 3 sig figs) While my answer was 2.318 ( 4 sig figs) Heres my calculations 22.20 g Fe2O3 / 159.69 = 0.13901934999060680067631035130565 mols of Fe2O3 14.00 g CO / 28.01 = 0.49982149232416993930739021777936 mols of  CO 0.13901934999060680067631035130565 x 3 = 0.41705804997182040202893105391696 mols of Fe2O3 needed to...
Constants | Periodic Table Iron(III) oxide reacts with carbon to give iron and carbon monoxide. Fe2O3(s)+3C(s)→2Fe(s)+3CO(g)...
Constants | Periodic Table Iron(III) oxide reacts with carbon to give iron and carbon monoxide. Fe2O3(s)+3C(s)→2Fe(s)+3CO(g) Part A How many grams of C are required to react with 78.2 g of Fe2O3? nothing   g   SubmitRequest Answer Part B How many grams of CO are produced when 38.0 g of C reacts? nothing   g   SubmitRequest Answer Part C How many grams of Fe can be produced when 6.40 g of Fe2O3 reacts? nothing   g   SubmitRequest Answer
Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide: Fe2O3 (s) +...
Iron (III) oxide reacts with carbon monoxide to produce iron and carbon dioxide: Fe2O3 (s) + 3CO(g)  2Fe (s) + 3 CO2 (g) 54.4 g of Fe2O3and 24.7 g of CO react to produce iron. Molar mass of Fe2O3 = 159.69 g/mol. Molar mass of CO = 28.01 g/mol. Determine the (a) limiting reactant, (b) theoretical yield, and (c) percent yield for the reaction if 29.1 g of iron are produced.
The following reaction is used to obtain iron from iron ore: Fe2O3(s)+3CO(g) ? 2Fe(s)+3CO2(g) The reaction...
The following reaction is used to obtain iron from iron ore: Fe2O3(s)+3CO(g) ? 2Fe(s)+3CO2(g) The reaction of 172 g of Fe2O3 with 84.2 g of CO produces 71.8 g of Fe. Calculate the theoretical yield of solid iron. Express the mass in grams to three significant figures.
Mining companies extract iron from iron ore according to the following balanced equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) In a...
Mining companies extract iron from iron ore according to the following balanced equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) In a reaction mixture containing 169 g Fe2O3 and 59.4 g CO, CO is the limiting reactant. Part A Calculate the mass of the reactant in excess (which is Fe2O3) that remains after the reaction has gone to completion. Express the mass with the appropriate units.
Mining companies extract iron from iron ore according to the following balanced equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) In a...
Mining companies extract iron from iron ore according to the following balanced equation: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) In a reaction mixture containing 179 g Fe2O3 and 61.8 g CO, CO is the limiting reactant. Part A Calculate the mass of the reactant in excess (which is Fe2O3) that remains after the reaction has gone to completion. Express the mass with the appropriate units.
Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH...
Calculate ΔHrxn for the following reaction: Fe2O3(s)+3CO(g)→2Fe(s)+3CO2(g) Use the following reactions and given ΔH′s. 2Fe(s)+3/2O2(g)→Fe2O3(s), ΔH = -824.2 kJ CO(g)+1/2O2(g)→CO2(g), ΔH = -282.7 kJ
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT