What total volume of gas derived from oxalyl chloride could be produced based on the 3
mL of oxalyl chloride solution used in your experiment. Assume complete reaction and
that oxalyl chloride is the limiting reagent
The molar mass of oxalyl chloride (C2Cl2O2) is calculated as follows:
Carbon (C): 2 atoms x 12.01 g/mol = 24.02 g/mol
Chlorine (Cl): 2 atoms x 35.45 g/mol = 70.9 g/mol
Oxygen (O): 2 atoms x 16.00 g/mol = 32.00 g/mol
Molar mass of oxalyl chloride = 24.02 + 70.9 + 32 = 126.92 g/mol
Now, we need to convert the volume of the oxalyl chloride solution to moles. Since the molarity is not provided, we cannot calculate the exact number of moles. However, we can estimate it assuming a typical molarity range for oxalyl chloride solutions used in experiments (e.g., 0.1 - 1.0 M).
If we assume a 0.1 M oxalyl chloride solution, then the number of moles in 3 mL (0.003 L) of solution can be calculated as follows:
Moles = Molarity x Volume = 0.1 mol/L x 0.003 L = 0.0003 mol
Since oxalyl chloride is the limiting reagent, this amount of oxalyl chloride will react completely to produce carbon dioxide (CO2) and phosgene (COCl2) gases. The balanced chemical equation for the reaction is as follows:
C2Cl2O2 + 2H2O -> 2COCl2 + CO2
From the balanced equation, we can see that 1 mole of oxalyl chloride produces 1 mole of CO2 gas. Therefore, the number of moles of CO2 gas produced will also be 0.0003 mol.
Now, we can calculate the total volume of CO2 gas produced at STP (standard temperature and pressure, 0°C and 1 atm) using the ideal gas law:
PV = nRT
Assuming the ideal gas constant R = 0.0821 L.atm/mol.K, the temperature T = 273 K, and the pressure P = 1 atm, we can rearrange the equation to solve for the volume V:
V = nRT/P = (0.0003 mol) x (0.0821 L.atm/mol.K) x (273 K) / 1 atm = 0.0069 L or 6.9 mL
Therefore, approximately 6.9 mL of CO2 gas could be produced from the 3 mL of oxalyl chloride solution in your experiment.