Question #92579
Metallocene are metals sandwiched by two cyclopentadienyl ions, (C5H5)–. A metallocene sample of unknown metal, MC5H5 (all 5 are subscripts) was burned in air. Products of combustion found to contain 46.08488% carbon dioxide, 9.42644% water vapour and the rest are metal (I) oxide. All products are in mass percent. The mass ratio of stoichiometric amount of oxygen to the burned metallocene is 1:1.295. What is the name of the metal in the metallocene sample? Prove by showing your complete solution.
1
Expert's answer
2019-08-14T02:43:41-0400

The reaction of combustion of the given metallocene (MeCp) is following:

2 MeC5H5+13O2=10CO2+5H2O+Me2O2 \ MeC_5H_5 + 13O_2=10CO_2+5H_2O+Me_2O

The stoichiometric ratio between MeCp and O2 is:

n(MeCp)n(O2)=213\frac{n(MeCp)}{n(O_2)}=\frac{2}{13}

As n(MeCp)=m(MeCp)M(MeCp)n(MeCp)=\frac{m(MeCp)}{M(MeCp)} and n(O2)=m(O2)M(O2)n(O_2)=\frac{m(O_2)}{M(O_2)} ,the above equation transforms to the following:

m(MeCp)m(O2)M(O2)M(MeCp)=213\frac{m(MeCp)}{m(O_2)}\cdot \frac{M(O_2)}{M(MeCp)}=\frac{2}{13}

From the given conditions the mass ratio of stoichiometric amount of oxygen to the burned metallocene is 1:1.295, i.e. m(O2)m(MeCp)=11.295\frac{m(O_2)}{m(MeCp)}=\frac{1}{1.295}

Thus two equations above transform to the following:

1.2951M(O2)M(MeCp)=213\frac{1.295}{1}\cdot \frac{M(O_2)}{M(MeCp)}=\frac{2}{13}

from which we can find molar mass of metallocene:

M(MeCp)=1.2951332gmol2=269.36gmolM(MeCp)=\frac{1.295\cdot 13 \cdot 32\frac{g}{mol}}{2}=269.36\frac{g}{mol}

Taking into account that M(MeCp)=M(Me)+M(Cp)=M(Me)+M(C5H5)=M(Me)+65 (gmol)M(MeCp)=M(Me)+M(Cp)=M(Me)+M(C_5H_5)=M(Me)+65 \ (\frac{g}{mol}) it is easy to find the molar mass of metal:

M(Me)+65=269.36M(Me)+65=269.36

M(Me)=204.36gmolM(Me)=204.36 \frac{g}{mol}

This molar mass of metal corresponds to thallium, that is known to form a metallocene that adopts a sandwich-like polymeric structure:


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