# 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%**