Final answer:
To calculate the mass of carbon dioxide produced by the complete combustion of 2.0 L of C2H2 at STP, we need to use the balanced equation and stoichiometry. The correct mass of CO2 produced is 7.88 grams. The balanced equation for the combustion of C2H2 is 2C2H2 + 5O2 → 4CO2 + 2H2O.
Step-by-step explanation:
To calculate the mass of carbon dioxide produced by the complete combustion of 2.0 L of C2H2 at STP, we need to use the balanced equation and stoichiometry. The balanced equation for the combustion of C2H2 is 2C2H2 + 5O2 → 4CO2 + 2H2O. From the equation, we can see that for every 2 moles of C2H2, 4 moles of CO2 are produced. Therefore, to calculate the mass of CO2, we need to convert 2.0 L of C2H2 to moles using the ideal gas law, then use the stoichiometric ratio to find the moles of CO2, and finally convert the moles of CO2 to grams by multiplying with the molar mass of CO2. First, let's convert 2.0 L of C2H2 to moles. At STP (Standard Temperature and Pressure), 1 mole of any ideal gas occupies a volume of 22.4 L.
Therefore, 2.0 L of C2H2 is equal to 2.0/22.4 = 0.0893 moles of C2H2. Next, using the stoichiometric ratio from the balanced equation, we can find the moles of CO2 produced. For every 2 moles of C2H2, 4 moles of CO2 are produced. Therefore, 0.0893 moles of C2H2 will produce (0.0893/2) * 4 = 0.179 moles of CO2. Finally, to convert moles of CO2 to grams, we multiply by the molar mass of CO2 which is approximately 44.01 g/mol. Therefore, the mass of CO2 produced by the complete combustion of 2.0 L of C2H2 at STP is 0.179 * 44.01 = 7.88 grams. Hence, the correct answer is 7.88 grams of CO2.