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Pb + S yield FeS
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5.6g of iron metal Fe are heated strong and mixed with 8g of sulfur S to form 4.4g of iron(ll) sulfide FeS. a, identify the
Top answer:
Fe + S --> FeS a. moles Fe = g/atomic mass = 5.6/56 = 0.1 mol moles S = 8/32 = 0.25 0.1 mole Fe will
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Hi, please check my work:
In an experiment, 23.4 g of FES are added to excess oxygen and 16.5 g of FE2O3 are produced. The
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you should get half the moles you started with. expected yield=.133 moles or .133*molmassFe2O3
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Hi, please check my work:
In an experiment, 23.4 g of FES are added to excess oxygen and 16.5 g of FE2O3 are produced. The
Top answer:
That equation does not look balanced to me. Check the oxygen on both sides.
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Hi, please check my work:
In an experiment, 23.4 g of FES are added to excess oxygen and 16.5 g of FE2O3 are produced. The
Top answer:
You started with .266 mol you should have ended with .133 mole of product. Actual product moles:
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Hi, please check my work:
In an experiment, 23.4 g of FES are added to excess oxygen and 16.5 g of FE2O3 are produced. The
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Your calculations are correct, but there seems to be a mistake in your final calculation for the
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How much HCO2H is obtained by reacting 3.0g of FeS, 1.60g H2S, and 1.60g CO2 if the reaction results in a 47.0% yield?
I know
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Well, now that you've calculated the molar masses of each compound, you can use them to calculate
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Given the following standard reduction potentials,
Fe^2+(aq) + 2e^- ==> Fe(s) E naught = -o.440V FeS(s) + 2e^- ==> Fe(s) +
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To determine the Ksp for FeS(s) at 25 degrees Celsius using the given standard reduction potentials,
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4 FeS(s) + 7 O2(g) ==> 2 Fe2O3(s) + 4 SO2(g)
7.82 moles of FeS are required to produce 3.91 moles of Fe2O3 What is the maximum
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The problem here is "liters" of Fe2O3? and Liters of FeS? These are not gases, and something is
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Can Fe2+ and Mn2+ be separated by precipitating FeS(s) and not MnS(s)? Assume [Fe2+]=[Mn2+]=[H2S]=0.10 M. Choose a [H3O+] that
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What does Kspa mean? It can't be Ksp because neither Ksp for FeS nor Ksp for MnS are anywhere close
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Sb2S3(s) + 3 Fe(s) 2 Sb(s) + 3 FeS(s)
When 14.7 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the percent
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Follow the steps in this example stoichiometry problem. This will give you the theoretical yield.
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