Question

Acetylene gas (C2H2), is used in welding torches. When it reacts with oxygen, it produces carbon dioxide (CO2), and steam (H2O). The reaction can be described by the equation 2C2H2+5O2 -> 4CO,+2H2O. How much mass of C2H2 is needed to produce 75.0 grams of CO2?

Answer 1

22.1 g

Step-by-step explanation:

Step 1: Write the balanced equation for the combustion of acetylene

2 C₂H₂ + 5 O₂ ⇒ 4 CO₂ + 2 H₂O

Step 2: Calculate the moles corresponding to 75.0 g of CO₂

The molar mass of CO₂ is 44.01 g/mol.

75.0 g × 1 mol/44.01 g = 1.70 mol

Step 3: Calculate the moles of C₂H₂ required to produce 1.70 moles of CO₂

The molar ratio of C₂H₂ to CO₂ is 2:4. The moles of C₂H₂ required are 2/4 × 1.70 mol = 0.850 mol.

Step 4: Calculate the mass corresponding to 0.850 moles of C₂H₂

The molar mass of C₂H₂ is 26.04 g/mol.

0.850 mol × 26.04 g/mol = 22.1 g