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zmey [24]
3 years ago
8

Deduce the structure of an unknown compound using the data below: Molecular Formula: C6H12O IR: 1705 cm-1 1H NMR: no absorptions

greater than δ 3 ppm 13C NMR: δ 24.4, δ 26.4, δ 44.2, and δ 212.6 ppm. Resonances at δ 44.2 and 212.6 have very low intensity.

Chemistry
1 answer:
Novosadov [1.4K]3 years ago
7 0

Answer:

The compound elucidated from the spectral data is <u>4-methyl penta-2-none</u>

Explanation:

  • <u>1700 cm-1 from IR data</u> suspects aldehyde/ketone or carboxylic acid. However,since the peak is not a stretched vibration, it implies an aldehyde or ketone present.
  • <u>3 ppm H NMR</u> confirms O-CH3 bond
  • <u>24.4 13C NMR</u> confirms CH3-R bond
  • 26.4 13C NMR  confirms H3C-(R)C(H)-R
  • 44.2 13C NMR Confirms C=
  • 2126 13C NMR confirms aldehyde C=O bond

<u>The deduced structure is 4-methyl penta-2-one (see attached) </u>given multiple CH3 atoms.

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2.8 mg ≈ 0.12 mol

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When an atom of the unstable isotope Na-24 decays, it becomes an atom of Mg-24 because the Na-24 atom spontaneously releases:(1)
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The elements lithium and oxygen react explosively to from lithium oxide (Li2O). How much lithium oxide will form if 3.03 mol of
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The reaction equation:
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Consider the following reaction:C2H4(g) + F2(g) -----------&gt; C2H4F2(g) Delta H = -549 kJEstimate the carbon-fluorine bond ene
frutty [35]

Answer:

Bond energy of carbon-fluorine bond is 485 kJ/mol

Explanation:

Enthalpy change for a reaction,  is given as:

\Delta H_{rxn}=\sum [n_{i}\times (E_{bond})_{i}]-\sum [n_{j}\times (E_{bond})_{j}]

Where (E_{bond})_{i}  and (E_{bond})_{j} represents average bond energy in breaking "i" th bond and forming "j" th bond respectively.n_{i} and n_{j} are number of moles of bond break and form respectively.

In this reaction, one mol of C=C, four moles of C-H and one mol of F-F bonds are broken. One mol of C-C bond, four moles of C-H bonds and two moles of C-F bonds are formed

So, -549kJ=(1mol\times 614kJ/mo)+(4mol\times E_{C-H})+(1mol\times 154kJ/mol)-(1mol\times 347kJ/mol)-(4mol\times E_{C-H})-(2mol\times E_{C-F})

or, -549kJ=(1mol\times 614kJ/mo)+(1mol\times 154kJ/mol)-(1mol\times 347kJ/mol)-(2mol\times E_{C-F})

or, E_{C-F}=485kJ/mol

So bond energy of carbon-fluorine bond is 485 kJ/mol

8 0
3 years ago
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