Question
In: Chemistry
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.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
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.
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 use this reaction to obtain iron from iron ore : Fe2O3(s) + 3CO(g) =...
Mining companies use this reaction to obtain iron from
iron ore : Fe2O3(s) + 3CO(g) = 2Fe(s) + 3CO2(g). The reaction of
167g Fe2O3 with 84.7g CO produces 76.5g Fe. Determine the
theoretical yield. Determine the percent yield.
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 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?
(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...
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...
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
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
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