CHEISTRY | MOLE CONCEPT | Question 17


A reaction container holds 5.77g of P4 and 5.77g of O2. The following reaction occur

P4 + O2 → P4O6

If there were enough Oxygen were available, then the P4O6 reacts further;
P4O6 + O2 → P4O10

Calculate;
i. Mode of P4O10 produced
ii. Mass of P4O10 produced.


  • DATA


    Mass of P4 = 5.77g
    Mass of 02 = 5.77g

    Equations PO4 + 302 → P4O6
    P4O6 + 202 → P4O10
    Asked
    i. Mole of P4O10 produced
    ii. Mass of P4O10 produced

    To find the mole of P4,
    Mole of P4 = mass of P4 / Molar mass of P4
    = 5.77g / 124g/mole
    = 0.0465 mole

    Mole of 02 = mass of 02 / Mole of 02
    = 5.77g / 32g/mole
    = 0.1803125 mole

    Mole ratios for P4 = 0.0465 / 1
    = 0.0465
    For 02 = 0.803125 / 3
    = 0.060104
    The limiting reagent was oxygen
  • i/ To find mole of P4O10


    mole equivalent between O2 and P4O10
    2 miles of O2 Ξ 1 mole of P4O10 0.1803 mole Ξ?
    Mole of O2 = (0.1803 mole × 1 mole) / 2 mole
    = 0.09015 mole
    0.09015 mole of P4O10 produced
  • ii/ To find the mass of P4O10


    From;
    Mole of P4O10 = 0.09015 mole
    Molar mass of P4O10 = 284
    Mass = mole × molar mass
    = 0.0915 mole × 284g/mole
    = 256.026g
    256.026g of P4O10 produced

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