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kit 發問於 科學及數學化學 · 1 十年前

F4 calculation

ammonium nitrate is manufactured from ammonia by a two-stage process

1. NH3+2O2 -> HNO3+H2O

2.HNO3+ NH3 -> NH4NO3

what is the max. mass of fertilizer that can be made if only17 tonnes of ammonia is available?

2 個解答

評分
  • 1 十年前
    最愛解答

    1. NH3 + 2O2 → HNO3 + H2O

    2. HNO3 + NH3 → NH4NO3

    According to the equations, we should use 8.5 tonnes of ammonia in state one and the other 8.5 tonnes in state 2. (By mole ratio, NH3 : HNO3 = 1:1)

    Molar mass of ammonia, NH3

    = 14.0 + 1.0 X 3

    = 17.0 g/mol

    No. of mole of NH3

    = mass / molar mass

    = 1.7 X 10^7 / 17.0

    = 1.0 X 10^6 mol

    From equation 2, mole ratio of NH3 : NH4NO3 = 1:1

    So, no. of mole of NH4NO3 = 1.0 X 10^6 mol

    Molar mass of NH4NO3

    = 14.0 X 2 + 1.0 X 4 + 16.0 X 3

    = 80.0 g/mol

    By mass = molar mass X no. of mole

    Mass of NH4NO3 = 80.0 X 1.0 X 10^6

    = 8.0 X 10^7 g

    = 80 tonnes

    So, the maximum mass of fertilizer that can be made is 80 tonnes.

    (P.S. relative atomic mass of H = 1.0 , N = 14.0 , O = 16.0)

    資料來源: Myself~~~
  • 1 十年前

    Overall reaction:

    2 NH3 + 2 O2 --> NH4NO3 + H2O

    i.e. 2 mole of NH3 (mw = 17) yield 1 mole of NH4NO3 (mw = 80)

    Thus, assuming 100 % conversion,

    max. mass of NH4NO3 = 17 tonnes / 17 / 2 * 80 = 40 tonnes

    資料來源: Stoichiometry calculation
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