Aircraft accident report mole airlines flight 1023 dc 6 02 o hare airport chicago october 23 2010
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Aircraft Accident Report Mole Airlines Flight 1023 DC 6-02 O’Hare Airport, Chicago October 23, 2010. National Transportation Safety Board. SHS Task Force Report Number:60-21-023-AA. Mole Airlines Flight 1023. SHS Task Forces October 2011. Flight leaving O’Hare headed for Boston

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Aircraft accident report mole airlines flight 1023 dc 6 02 o hare airport chicago october 23 2010

Aircraft Accident ReportMole AirlinesFlight 1023 DC 6-02 O’Hare Airport, ChicagoOctober 23, 2010

National Transportation Safety Board

SHS Task Force

Report Number:60-21-023-AA


Mole airlines flight 1023

Mole Airlines Flight 1023

SHS Task Forces

October 2011


National transportation safety board

  • Flight leaving O’Hare headed for Boston

  • 6:02 pm EST plane crashed outside of Detroit, MI

  • Evidence of a Pre-Crash Explosion Found

  • At the site of the explosion a material has been found.

    • Subsequent chemical analysis of the material shows it to be:

      Carbon 37.01%Hydrogen 2.22%

      Nitrogen 18.5%Oxygen 42.27%


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  • Mangled passengers are found in and around the crash.

  • They are not recognizable and their dental records are not available.

  • They must be identified by the substances found in their belongings or in their bodies.

  • Upon further investigation one passenger showed a time of death approximated at one hour prior to the crash. Perhaps they were murdered?


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  • Split into 12 task forces (2 chemist teams)

  • Work on analysis chemical substances from each Toe Tag.

  • You should be able to determine the EMPIRICAL FORMULA from the % compositions that were found.

  • Compare the formulas to known compounds on the data table to name the chemical.

  • Use passenger list to make a tentative identification.

  • Submit reports to your supervisor.


C 37 01 h 2 22 n 18 5 o 42 27

C:37.01% H: 2.22% N: 18.5% O: 42.27%

  • How to find the Empirical Formula….

    • Assume 100g & Divide % composition by molecular mass

      • 37.01g C / 12.01 g/mol = 3.083 mol C

      • 2.22g H / 1.01 g/mol = 2.20 mol H

      • 18.5g N / 14.0 g/mol = 1.32 mol N

      • 42.27g O / 16.00 g/mol = 2.642 mol O

Atomic Mass of Carbon


How to find the empirical formula

How to find the Empirical Formula….

  • Divide all answers by the smallest answer (1.32 mol)

    • 3.083 mol C / 1.32 mol = 2.33

    • 2.20 mol H / 1.32 mol = 1.67

    • 1.32 mol N / 1.32 mol = 1.00

    • 2.642 mol O / 1.32 mol = 2.00


Write the number of moles as a subscript in a chemical formula

Write the number of moles as a subscript in a chemical formula

3.083 mol C / 1.32 mol = 2.33 Carbon

2.20 mol H / 1.32 mol = 1.67 Hydrogen

1.32 mol N / 1.32 mol = 1.00 Nitrogen

2.642 mol O / 1.32 mol = 2.00 Oxygen

  • C2.33H1.67N1.00O2.00

  • Need to get whole numbers as subscripts


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  • Multiply these answers by 2, 3, or 4 to get whole numbers

    • 2 x 2.33 = 4.66 Not close enough

    • 3 x 2.33 = 6.99 Very close to the WHOLE NUMBER 7

    • 4 x 2.33 = 9.32 Not close enough

  • USE 3

    • 3 x 2.33 = 7There are 7 C

    • 3 x 1.67 = 5There are 5 H

    • 3 x 1.00 = 3There are 3 N

    • 3 x 2.00 = 6There are 6 O

  • Write out the Empirical Formula using the whole numbers calculated.

    • Formula= C7H5N3O6


  • National transportation safety board

    Formula= C7H5N3O6

    • Look up Formula on Table to Identify

      • Trinitrotoluene

      • Description: Explosive (TNT=dynamite)

    • What conclusions can be draw from the evidence?


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