We need a stoichiometrically balanced chemical equation to represent the redox reaction.....and I gets approx. 75% yield.
The metal is oxidized, and the halogen is reduced.....
And so we interrogate the molar quantities of the reactants....
And thus (finally)....
Note that in this scenario, i.e. limited quantities of the halogen, incomplete oxidation to
WARNING! Long answer! The percent yield is 96 %.
We are given the masses of two reactants, so this is a limiting reactant problem.
We know that we will need a balanced equation with masses, moles, and molar masses of the compounds involved.
1. Gather all the information in one place with molar masses above the formulas and everything else below them.
We start with the balanced equation.
(a) Calculate the moles of
(b) Calculate moles of
2. Identify the limiting reactant
An easy way to identify the limiting reactant is to calculate the "moles of reaction" each will give:
You divide the moles of each reactant by its corresponding coefficient in the balanced equation.
I did that for you in the table above.
3. Calculate the theoretical yield of
The theoretical yield of
4. Calculate the percent yield of
The formula for percentage yield is
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