br asked in Science & MathematicsChemistry · 4 months ago

Fe(HSO3)3 + 3 HNO2 = Fe(NO2)3 + 3 H2(SO3) How many moles of the two products are obtained with 4.48L of ferrous hydrogen sulphite (gas)?

everything is in STP conditions

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  • 4 months ago
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    The coefficients in a balanced equation determine the ratio of the reactants to the moles of products. For the reaction, one mole of ferrous hydrogen sulfite reacts with three moles of ferrous nitrate to produce one mole ferrous nitrite and three moles of hydrogen sulfite. Since ferrous hydrogen sulfite is a gas at standard temperature and pressure, the volume of one mole is 22.4 liters. To determine the number

    n = 4.48 ÷ 22.4 = 0.2

    Since ferrous hydrogen sulfite and ferrous nitrate have the same coefficients, they have the same number of moles. (0.2). The ratio of moles of ferrous hydrogen sulfite to moles of hydrogen sulphite is 1:3. We can use the following proportion to calculate the number of moles of hydrogen sulfite.

    1 ÷ 3 = 0.2 ÷ n

    n = 0.6 mole

    I hope this is helpful for you.

  • 4 months ago

    No way.....

    "Ferrous hydrogen sulfite" is not "Fe(HSO3)3."

    Fe(HSO3)3 doesn't exist. (Nor does "ferrous hydrogen sulfite.") If iron(III) ions were added to a solution of bisulfite ions they would react to form iron(II) sulfate.

    .... 2Fe3+ + HSO3^- + H2O --> 2Fe2+ + SO4^2- + 3H+

    The entire premise of the question is flawed. Sure you could write what looks like a double replacement reaction, but it would be a work of fiction. Neither of the "products" are insoluble. Heck, molecules of H2SO3 don't even exist in solution. What is called "sulfurous acid" is actually sulfur dioxide dissolved in water in equilibrium with small amounts of H+ and HSO3^- ions. Your teacher should write questions dealing with chemistry which actually occurs.

    How about ....

    .... Fe(OH)3(s) + 3HNO3(aq) --> Fe(NO3)3(aq) + 3HOH(l)

    .... FeSO4(aq) + Ba(NO3)2(aq) --> BaSO4(s) + Fe(NO3)2(aq)

    .... FeCl3(aq) + 3AgNO3(aq) --> 3AgCl(s) + Fe(NO3)3(aq)

  • Dr W
    Lv 7
    4 months ago

    assuming the HNO2 is in XS

    .. 4.48L FHS.. . .1 mol FHS.. .... 1 Fe(NO2)3

    ------- ----- ---- x ----- ----- ----- x ---- --- ---- ---- = 0.200 mol Fe(NO2)3

    .. .. .. .1.. ... ... ... 22.41 L FHS.. ... 1 mol FHS

    .. 4.48L FHS.. . .1 mol FHS.. .... 3 mol H2SO3

    ------- ----- ---- x ----- ----- ----- x ---- ---- ---- ---- = 0.600 mol H2SO3

    .. .. .. .1.. ... ... ... 22.41 L FHS.. ... 1 mol FHS

    • pisgahchemist
      Lv 7
      4 months agoReport

      What am I missing? I can't find any references to "ferrous hydrogen sulfite", much less that it is a gas. There are multiple references to Fe(HSO4)3 as a catalyst, but it's not a gas.

  • 4 months ago

    At STP, the 4.48L will be 0.2 moles, so the products would be 0.2 moles of Fe(NO2)3 and 0.6 moles of H2(SO3).

    • pisgahchemist
      Lv 7
      4 months agoReport

      None of the species in this "equation" are gases. 22.414L for a mole of gas at STP is irrelevant.

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