The balanced equation for the combustion of C3H8 (propane) is:
C3H8 + 5O2 → 3CO2 + 4H2O
However, the chemical equation provided in the question is for the combustion of C2H2 (acetylene) instead. So, we need to balance the given equation:
2C2H2 + 5O2 → 4CO2 + 2H2O
The molar mass of CO2 is 12 + 2(16) = 44 g/mol.
To calculate the mass of CO2 formed, we first need to determine the number of moles of C2H2 used in the reaction:
12.00 g C2H2 × (1 mol C2H2/26.038 g C2H2) = 0.4616 mol C2H2
According to the balanced equation, 2 moles of C2H2 produce 4 moles of CO2, so:
0.4616 mol C2H2 × (4 mol CO2/2 mol C2H2) = 0.9232 mol CO2
Finally, we can calculate the mass of CO2 formed:
0.9232 mol CO2 × 44 g/mol = 40.6 g CO2
Therefore, the mass of CO2 formed is approximately 40.6 grams if 12.00 grams of C2H2 are used in the reaction.