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Posted by on Wednesday, July 16, 2008 at 7:15pm.

Heres the question:
"In determining the simplest formula of lead sulfide, 2.46 grams of lead are placed in a crucible with 2.00 grams of sulfur. When the reaction is complete, the product has a mass of 3.22 grams. What mass of sulfur should be used to in the simplest forumla calculation? Find the simplest formula of lead sulfide."

Could someone go through steps for me.

  • Chemistry - , Wednesday, July 16, 2008 at 7:35pm

    mass Pb = 2.46 g.
    mass lead sulfide = 3.22 g.
    mass S used = 3.22-2.46 = 0.76 g.

    mols Pb = 2.46/207.20 = 0.01187
    mols S = 0.76/32.066 = 0.02370

    ratio: Divide the smallest number by itself thereby assuring you that will be 1.0000.

    mols Pb = 0.01187/0.01187 = 1.000
    mols S = 0.02370/0.01187 = 1.9967

    rounded to whole numbers we have Pb = 1.0 and S = 2.0 so formula is PbS2.
    Note: I have carried out the numbers to far more places than is allowed so round down to two (since 0.76 has two places) at the most. Also, PbS is the formula for lead sulfide but these numbers don't reflect that.
    Check my work.

  • Chemistry - , Wednesday, July 16, 2008 at 8:19pm

    Thanks for the fast reply!

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