chemistry

A mixture contained zinc sulfide, ZnS, and lead sulfide, PbS. A sample of the mixture weighing 6.12 g was reacted with an excess of hydrochloric acid. The reactions are given below.
ZnS(s) + 2 HCl(aq) → ZnCl2(aq) + H2S(g)

PbS(s) + 2 HCl(aq) → PbCl2(aq) + H2S(g)
If the sample reacted completely and produced 1.038 L of hydrogen sulfide, H2S, at 23°C and 745 mmHg, what were the percentages of ZnS and PbS in the mixture?
ZnS

  1. 0
  2. 3
asked by caroline
  1. Let X = mass ZnS
    Let Y = mass PbS
    MM = molar mass
    =====================
    You need two equations.
    X + Y = 6.12 is one. The second is
    X(MM H2S/MM ZnS) + Y(MMH2S/MMPbS) = grams H2S.
    The g H2S must be calculated from PV = nRT and solve for n=number of moles H2S, then convert to grams, knowing 22.4 L H2S at STP will have a mass of 34.08 grams.

    Solve the two equation simultaneously which will give you grams ZnS and grams PbS. Then percent ZnS = (mass ZnS/mass sample)*100 = ?? and
    %PbS = (mass PbS/mass sample)*100 = ??

    1. 0
    posted by DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    The following equilibrium was studied by analyzing the equilibrium mixture for the amount of H2S produced. Sb2S3(solid)+3H2(gas)2Sb(solid)+3H2S(solid) A vessel whose volume is 2.5L is filled with 0.0100 mole of
  2. chemistry

    The first step in the process used to recover zinc metal from zinc sulfide ore is the reaction of zinc sulfide with oxygen gas to produce zinc oxide and sulfur dioxide. 2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2(g) When the external
  3. chemistry 106

    The first step in the industrial recovery of zinc from the zinc sulfide ore is roasting, that is, the conversion of ZnS to ZnO by heating. 2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2 SO2(g) ΔH = -879 kJ/mol Calculate the heat evolved (in
  4. chemistry help

    An amount of 414.27 g of zinc sulfide (ZnS, MM=97.44 g/mol) reacts with 99.58 g of oxygen gas (O2, MM=31.999 g/mol) at a constant temperature of 298.0 K and constant pressure of 1.00 atm. The reaction: 2 ZnS(s) + 3 O2(g) --> 2
  5. chemistry help

    An amount of 414.27 g of zinc sulfide (ZnS, MM=97.44 g/mol) reacts with 99.58 g of oxygen gas (O2, MM=31.999 g/mol) at a constant temperature of 298.0 K and constant pressure of 1.00 atm. The reaction: 2 ZnS(s) + 3 O2(g) --> 2
  6. Chemistry

    Zinc and sulfur react to form zinc sulfide according to the equation Zn+S=>ZnS a) How many grams of ZnS will be formed? b) How many grams of the excess reactant will remain after the reaction is over?
  7. Chemistry

    Lead can be extracted from lead(II) sulfide, PbS, in two stages. Stage 1: Lead(II) sulfide is heated in air. It reacts with oxygen to produce lead(II) oxide and sulfur dioxide. Stage 2: The Lead(II) oxide is then heated in a blast
  8. Chemistry College

    A 79.1 g mixture of the compounds calcium chloride and sodium sulfide is 80.9 % by mass sodium sulfide. The compound sodium sulfide is 58.9 % by mass sodium. Calculate the mass (g) of sulfur in the mixture. thanks.
  9. chemistry

    what is the concentration of lead ions and sulfide ions in a saturated solution of lead sulfide (PbS) solution at 25 degrees celsius.
  10. chemistry

    what is the concentration of lead ions and sulfide ions in a saturated solution of lead sulfide (PbS) solution at 25 degrees celsius.

More Similar Questions