Determine the % yield when 7.80 grams of benzene (c6h6) burns in oxygen gas to form 3.00 grams of co2 gas and water vapor.

Benzene reacts with O₂ to produce CO₂ and H₂O, i. e.

C₆H₆ + 7.5 O₂ → 6 CO₂ + 3 H₂O

According to equation,

78.11 g (1 mole) C₆H₆ reacts to produce = 264 g (6 moles) of CO₂

Hence,

7.80 g C₆H₆ when reacted will produce = X g of CO₂

Solving for X,

X = (7.80 g * 264 g) : 78.11 g

X = 26.36 g of CO₂

Theoretical Yield:

26.36 g of CO₂ produced is theoretical yield which shows 100% reaction between benzene and oxygen.

Actual Yield:

According to statement the actual amount of CO₂ produced is 3.0 g of CO₂.

%age Yield:

%age Yield = (Actual Yield : Theoretical Yield) * 100

Putting Values,

%age Yield = (3.00 g : 26.36 g) * 100

%age Yield = 11.38 %