Question

What mass of CO2 is produced when 65.0 g of C2H4 reacts completely in the following equation:

C2H4 + 3O2 → 2CO2 + 2H2O

[Use 29.25 g/mol as the molar mass of CH4 and 45.5 g/mol as the molar mass of CO2]

Answer 1

The mass of CO2 produced from the reaction of 65.0 g of C2H4 is 203.9 g, calculated by converting the given mass of C2H4 to moles, using the mole ratio from the balanced chemical reaction, and then converting moles of CO2 to grams.

Step-by-step explanation:

To determine the mass of CO2 produced when 65.0 g of C2H4 reacts completely, we need to use stoichiometry based on the balanced chemical equation provided, C2H4 + 3O2 → 2CO2 + 2H2O. First, calculate the moles of C2H4 reacted by dividing the given mass by the molar mass of C2H4 (28.05 g/mol). Then, use the mole ratio from the balanced equation to convert moles of C2H4 to moles of CO2. Finally, multiply by the molar mass of CO2 (44.009 g/mol as given in the question) to find the mass of CO2 produced.

The calculation steps are as follows:

1. Calculate moles of C2H4: 65.0 g C2H4 ÷ 28.05 g/mol = 2.317 moles of C2H4.
2. Use the mole ratio (1 mol C2H4 : 2 mol CO2) to find moles of CO2: 2.317 moles C2H4 × 2 = 4.634 moles of CO2.
3. Calculate mass of CO2: 4.634 moles of CO2 × 44.009 g/mol = 203.9 g of CO2.

Therefore, the mass of CO2 produced is 203.9 g.