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The reaction of 5.0 g of fluorine with excess chlorine produced 5.6 g of chlorine trifluoride....

The reaction of 5.0 g of fluorine with excess chlorine produced 5.6 g of chlorine trifluoride. What is the percent yield of the reaction?

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Answer #1

Balenced chemical eq.

Cl2   +   3F2   -------->    2ClF3

71g (Cl2) react with    114g (F2) to obtain 184.9g of product (ClF3) formation.

Theoretical yield calculation (100%):

In gram if 5g of F2 taken: 5 x 184.9 / 114 = 8.1g (100%). It means we should get 8.1g of ClF3 from 5g of F2 after completion of reaction.

But from question it is only 5.6g.

So now, experimental yield % = 5.6 x 100 /8.1 = 69.13%.

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