Advanced Organic Chemistry
Q 1: Explain how you would separate
K4[Fe(CN)6] from K3[Fe(CN)6]
?
Q 2: Determine the mole fraction of
CrCl2(OH2)4+ and
CrCl(OH2)5+ if 5mL of it was
collected had an absorbance of 0.534 and 0.257. Assume that the
extinction coefficients of the two coplexes are the same
What is the mass of potassium oxalate monohydrate and
iron (III) chloride required to synthesize 3g of potassium tris
(oxalato)iron (III). water should not be included in
equation.
Please include equation and explain in detail. thank you!
1 mole of K4[Fe(CN)6] contains carbon = 6g atoms. 0.5 mole of K4[Fe(CN)6] contain carbon = 3g atoms. The mass of carbon present in 0.5 mole of K4[Fe(CN)6] is:
Potassium tris(oxalato) ferrate (III), also known as potassium
ferrioxalate, is a green crystalline- compound of octahedral
geometry. It is a metal complex of iron with three oxalate (C2O42-)
ligands bonded to the central metal atom (Fe). These ligands are
bidentate, meaning that each of them binds to the metal atom at 2
different places.
Potassium ferrioxalate is a very interesting photosensitive
material. In solution, it reacts with
2− light photons and undergoes a reduction reaction and
decomposes to give Fe(C2O4)2...
An inorganic chemist isolates a compound which she thinks is
potassium ferrocyanide: K4Fe(CN)6-3(H2O). she carries out a redox
determination for iron yielding the following results: 13.3%,
13.5%, 13.4%, 13.3%, 13.5% Fe by weight. At 95% confidence, has she
proven that the compound is not potassium ferrocyanide?
Identify the most likely transition metal
M:
a)
K3[M(CN)6], in which M is a
first-series transition metal and the complex has 3 unpaired
electrons.
b)
[M(H2O)6]3+, in which M is a
second-series transition metal and LFSE = –2.4 Do.
c) Tetrahedral
[MCl4]–, which has 5 unpaired electrons and
M is a first-series transition metal.
d) Square planar
[MCl2(NH3)2], in which M is a d8
third-series transition metal.
when 1.6038 g of an organic iron compound Fe, C, H and O was
burned in O2, 2.9998 g of CO2 and 0.85850 g of H2O were produced.
In a separate experiment to determine the mass percent of iron,
0.2726 g of the compound yielded 0.06159 g of Fe2O3. What is the
empirical formula of the compound?
In the lab, you mixed 3.8 g of iron(III) chloride
hexahydrate, with 9g of potassium oxalate monohydrate and produced
5.2g of a green crystalline product [K3Fe(C2O4)3·3H2O], along with
aqueous potassium chloride and water. What is the percent yield of
the green crystalline product?