chemistry

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disulfur dichloride is used to vulcanize rubber. it can be made by treating molten sulfur with gaseous chlorine: S8(1)+Cl2(g) -----> S2Cl2(1) starting with a mixture of 32.0g of sulfur and 71.0g of Cl2,
a.) which is the limiting reactant?
b.) what is the theoretical yield of S2Cl2?
c.) what mass of the excess reactant remains when the reaction is completed?

  • chemistry -

    1. Balance the equation.
    2. Convert 32.0 g S8 to moles. moles = grams/molar mass.
    3. Convert 71.0 g Cl2 to moles.
    4a. Convert moles S8 to moles S2Cl2 using the coefficients in the balanced equation.
    4b. Same for moles Cl2 to moles S2Cl2.
    4c. The SMALLER number of moles S2Cl2 will be the moles S2Cl2 formed and the reagent from which the smaller amount arises will be the limiting reagent.
    5. Theoretical yield is found by converting moles S2Cl2 to grams. Grams = moles x molar mass.
    6. Go through the same kind of procedure to determine the grams of the excess reagent used to form the theoretical yield of S2Cl2, then subtract from the amount with which you started. Post your work if you get stuck.

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