If 25 grams of propane burns and the percent yield is 75% how many grams of carbon dioxide is produced? C3H3 + 5O2 —> 4H2O + 3CO2

57 g

Explanation:

Step 1: Write the balanced equation

C₃H₈ + 5 O₂ ⇒ 4 H₂O + 3 CO₂

Step 2: Calculate the mass corresponding to 25 g of propane

The molar mass of C₃H₈ is 44.1 g/mol.

25 g × 1 mol/44.1 g = 0.57 mol

Step 3: Calculate the theoretical yield of CO₂ from 0.57 moles of C₃H₈

The molar ratio of C₃H₈ to CO₂ is 1:3. The theoretical yield of CO₂ is 3/1 × 0.57 mol = 1.7 mol

Step 4: Calculate the real yield of CO₂

We will use the following expression.

real yield = theoretical yield × percent yield

real yield = 1.7 mol × 75%

real yield = 1.3 mol

Step 5: Calculate the mass corresponding to 1.3 moles of carbon dioxide

The molar mass of CO₂ is 44.01 g/mol.

1.3 mol × 44.01 g/mol = 57 g

it means there are 3 atoms of oxygen