1. Balanced Chemical Equation:
The reaction you're describing is the fluorination of ethylene (C₂H₄) to produce 1,2-difluoroethane (C₂H₄F₂):
C₂H₄ + 2F₂ → C₂H₄F₂
2. Mole Calculations:
* Moles of C₂H₄F₂:
- Calculate the molar mass of C₂H₄F₂: (2 * 12.01 g/mol) + (4 * 1.01 g/mol) + (2 * 19.00 g/mol) = 66.06 g/mol
- Moles of C₂H₄F₂ = (100 g) / (66.06 g/mol) = 1.51 mol
* Moles of F₂:
- From the balanced equation, 2 moles of F₂ are required for every 1 mole of C₂H₄F₂.
- Moles of F₂ = (1.51 mol C₂H₄F₂) * (2 mol F₂ / 1 mol C₂H₄F₂) = 3.02 mol F₂
3. Volume Calculation:
* Ideal Gas Law:
- Assume standard temperature and pressure (STP): 0 °C (273.15 K) and 1 atm.
- Ideal Gas Law: PV = nRT, where:
- P = pressure (atm)
- V = volume (L)
- n = moles
- R = ideal gas constant (0.0821 L·atm/mol·K)
- T = temperature (K)
* Solving for Volume:
- V = (nRT) / P
- V = (3.02 mol * 0.0821 L·atm/mol·K * 273.15 K) / 1 atm
- V ≈ 67.5 L
Therefore, approximately 67.5 liters of fluorine gas (F₂) are required to convert 100 grams of C₂H₄ to C₂H₄F₂ at STP.
Important Note: Fluorine gas is extremely reactive and dangerous. This calculation is for theoretical understanding only and should not be attempted in a laboratory setting without proper safety precautions and expertise.
