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The reaction of 9.3 grams of fluorine with
excess chlorine produced 4.1 grams of ClF3.
What percent yield of ClF3 was obtained?

  • chemistry -

    1. Write and balance the equation.
    2. Convert 9.3 g F2 to mols. mols = grams/molar mass.
    3. Using the coefficients in the balanced equation, convert mols F2 to mols of the product.l
    4. Now convert mols or the product to grams. g = mols x molar mass. This is the theoretical yield(TE). Actual yield is 4.1g.
    5. %yield = (actual yield/TE)*100 = ?

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