Homework Answers
(a)(i) Volume of CO (g) = 16.2 L
Pressure of CO (g) = 1.50 atm
Temperature of CO (g) = 200.ºC
Convert the temperature to the absolute scale.
T = (273 + 200.)K = 473 K
Use the ideal gas to determine the number of moles of CO.
PV = nRT
where the symbols have their usual meanings.
Therefore,
n = PV/RT
Plug in values and get
n = (1.50 atm)*(16.2 L)/(0.082 L-atm/mol.K)(473 K)
= 0.6265 mol
≈ 0.626 mol (ans, correct to 3 sig, figs).
(ii) The balanced chemical reaction is given as
Fe2O3 (s) + 3 CO (g) ----------> 2 Fe (s) + 3 CO2 (g)
As per the stoichiometric equation,
1 mole Fe2O3 = 3 moles CO.
Mass of Fe2O3 taken = 15.39 g.
The atomic masses are
Fe: 55.845 g/mol
O: 15.999 g/mol
Gram molar mass of Fe2O3 = (2*55.845 + 3*15.999) g/mol
= 159.687 g/mol
Mol(s) Fe2O3 corresponding to 15.39 g = (15.39 g)/(159.687 g/mol)
= 0.09637 mol
≈ 0.0964 mol (correct to 3 sig. figs)
Determine the limiting reactant.
Fe2O3: (0.0964 mol Fe2O3)*(3 mols CO)/(1 mol Fe2O3) = 0.2892 mol CO
CO: (0.626 mol)*(1 mol Fe2O3)/(3 mols CO) = 0.20866 mol Fe2O3 ≈ 0.2087 mol Fe2O3.
We have only 0.0964 mol Fe2O3 and more than 0.2892 mol CO. Therefore, Fe2O3 is the limiting reactant.
(iii) As per the balanced stoichiometric equation,
1 mol Fe2O3 = 2 mols Fe.
Therefore,
Mols Fe corresponding to 0.0964 mol Fe2O3 = (0.0964 mol Fe2O3)*(2 mols Fe)/(1 mol Fe2O3)
= 0.1928 mol Fe.
≈ 0.193 mol Fe (correct to 3 sig, figs)
The moles of Fe formed = 0.193 mol (ans).
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Assume 117 grams of iron(III) oxide, Fe o reacts with excess hydrogen, H. The problem requires...
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all refer to the problem below
In the reaction of iron (III) sulfate and barium
hydroxide,
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If 20.0 g of Fe2(SO4)3 is mixed with 20.0 g of Ba(OH)2.
Molar masses
Fe2(SO4)3 = 399.91
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Fe(OH)3 = 106.88
39. If one of the chem 10 students ran the reaction as stated in
problem 35 and got 7.052 g of Ba(OH)2, what is the percentage yield
for the reaction...
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BACKGROUND: Synthesis of Potassium Iron
(III) Oxalate Hydrate Salt
The iron(II) ions from
Fe(NH4)2(SO4)2•6H2O
will be precipitated as iron(II) oxalate.
Fe^2+(aq) + C2O4^2-(aq) --> FeC2O4 (s)
The supernatant liquid, containing the ammonium and sulfate
ions, as well as excess oxalate ions and oxalic acid will be
decanted and discarded. The solid will then be re-dissolved and the
iron(II) ions will be oxidized to iron(III) ions by reaction with
hydrogen peroxide.
2Fe^2+(aq) + H2O2(aq) --> 2Fe^3+(aq) +2 OH^ - (aq)
The...
Iron ore is reduced to pure iron by smelting, during which the iron (III) oxide in...
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Assume 117 grams of iron(III) oxide, Fe o reacts with excess hydrogen, H. The problem requires that you determine the mass of iron, Fe, formed from this reaction. Fe, O (s) + 3 H (9) 2 Fe(s) + 3 H2O(1) 1 mol Fe 0, reus 159.70 g Fe,0, 55.85 g Fe --=81.8 g Fe Imol Fe
questions 35,36,37,38, and 39
all refer to the problem below
In the reaction of iron (III) sulfate and barium
hydroxide,
Fe2(SO4)3 + 3Ba(OH)2 -> 3BaSO4 + 2Fe(OH)3.
If 20.0 g of Fe2(SO4)3 is mixed with 20.0 g of Ba(OH)2.
Molar masses
Fe2(SO4)3 = 399.91
Ba(OH)2 = 171.35
Fe(OH)3 = 106.88
39. If one of the chem 10 students ran the reaction as stated in
problem 35 and got 7.052 g of Ba(OH)2, what is the percentage yield
for the reaction...
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BACKGROUND: Synthesis of Potassium Iron
(III) Oxalate Hydrate Salt
The iron(II) ions from
Fe(NH4)2(SO4)2•6H2O
will be precipitated as iron(II) oxalate.
Fe^2+(aq) + C2O4^2-(aq) --> FeC2O4 (s)
The supernatant liquid, containing the ammonium and sulfate
ions, as well as excess oxalate ions and oxalic acid will be
decanted and discarded. The solid will then be re-dissolved and the
iron(II) ions will be oxidized to iron(III) ions by reaction with
hydrogen peroxide.
2Fe^2+(aq) + H2O2(aq) --> 2Fe^3+(aq) +2 OH^ - (aq)
The...
Iron ore is reduced to pure iron by smelting, during which the iron (III) oxide in the ore reacts with carbon monoxide gas, like this: Fe2O3(s)+3CO(g) → 2Fe (s)+3CO2() Suppose an engineer decides to study the rate of this reaction. She prepares four reaction vessels with 93.4 g of solid iron (III) oxide and 29.8 g of carbon monoxide gas each. The volume and temperature of each vessel is shown in the table below. of reaction. In other words, select...
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