The Percentage Yield of ClF3 in a Chemical Reaction
Calculation of Percentage Yield of ClF3
The reaction of 9.2 grams of fluorine with excess chlorine produced 6.3 grams of ClF3. We need to calculate the percentage yield of ClF3 obtained in this chemical reaction.
Solution:
The Balanced Chemical Reaction is as follows:
Cl₂ + 3 F₂ → 2 ClF₃
According to the equation,
114 g (3 moles) F₂ produces 184.88 g (2 moles) of ClF₃
Therefore, 19.2 g of F₂ will produce X grams of ClF₃.
Solving for X,
X = (19.2 g × 184.88 g) ÷ 114 g
X = 31.13 g of ClF₃ (Theoretical Yield)
After the reaction, the actual yield obtained is 6.3 grams of ClF3. Now, we can calculate the percentage yield.
Percentage Yield = (Actual Yield ÷ Theoretical Yield) × 100
Percentage Yield = (6.3 g ÷ 31.3 g) × 100
Percentage Yield = 20.12%
What is the percentage yield of ClF3 in the given chemical reaction? Answer: Percentage Yield = 20.12%