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1.00 g zinc and 0.80 g sulfur are allowed to react all the zinc is used up 1.50 g of zinc sulfide is formed and some unreacted sulfur remains what is the mass of unreacted sulfur

  • chemistry -

    Zn + S ==> ZnS
    mols Zn = 1.00/65.39 = 0.016 but you need to do it more accurately.
    Convert mols Zn to mols S. That's 0.016 mols Zn x (1 mol S/1 mol Zn) = 0.016 mols Zn x 1/1 = 0.016 mols S.
    grams S used = mols x atomic mass S; then
    g S initially - g S used = g S remaining after the reaction.

  • chemistry -


  • chemistry -

    .30 g

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