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A gaseous compound consists of 86% carbon and 14% hydrogen by mass. At s.t.p, 3.2dm3 of the compound has a mass of 6g. (C = 12 H = 1 molar gas volume at s.t.p = 22.4dm3)

  1. Calculate its empirical formula  
  2. Calculate its molecular formula   

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  1.  
    Elements  C  H 
     % Mass 86  14 
     RAM 12  1
     Moles 86/12 =7.166  14/1=14 
     


    Mole ratio
     7.166
     7.166
      1
      1
       14  
     7.166
     1.95
      2

    E.F =CH2

  2. If 3.2dm3   → 6g
     22.4dm3 → ?
    22.4 × 6   =42 
        3.2
    MF=(EF)n
    n=R.M.M
         E.F.M
     =42/14=3 
    MF =(CH2)3
     =C3H6 

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