Final answer:
To find the mass of C2H4O2 needed to produce 1.75 L of CO2, we calculate the molar mass of C2H4O2 and use stoichiometry to determine that 0.002344 kg or 2.344 g of C2H4O2 is required.
Step-by-step explanation:
To calculate the mass of compound C2H4O2 (acetic acid) required to produce 1.75 L of carbon dioxide upon combustion, we must first write the balanced equation for the reaction:
C2H4O2 (l) + O2 (g) → 2CO2 (g) + 2H2O (l)
From the balanced equation, we can see that 1 mole of C2H4O2 produces 2 moles of CO2. Using the ideal gas law, we can assume that at standard temperature and pressure (STP), 1 mole of a gas occupies 22.4 L.
Hence, to get 1.75 L of CO2, we would need 1.75 L / 22.4 L/mol = 0.078125 moles of CO2.
Since 1 mole of C2H4O2 yields 2 moles of CO2, we would need half this amount of C2H4O2, which is 0.0390625 moles.
Next, we find the molar mass of C2H4O2 by summing the atomic masses of its constituent atoms (2 C, 4 H, and 2 O).
Molar mass of C2H4O2 = 2(12.01) + 4(1.01) + 2(16.00)
= 60.05 g/mol.
Therefore, the mass of the C2H4O2 needed is 0.0390625 moles * 60.05 g/mol = 2.344 g or 0.002344 kg.