Understanding Electrolysis of Sodium Chloride
The electrolysis of molten sodium chloride (NaCl) involves the decomposition of NaCl into sodium (Na) and chlorine gas (Cl₂) when an electric current is passed through it.

Key Concepts
- **Faraday's Laws of Electrolysis**: The amount of substance produced at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the electrolyte.
- **Moles of Chlorine Gas**: One molecule of chlorine gas (Cl₂) corresponds to half a mole of Cl atoms. Thus, for 0.10 molecules of Cl₂, we need to calculate the moles:
- Moles of Cl₂ = 0.10 molecules × (1 mole / 6.022 × 10²³ molecules) = 1.66 × 10⁻²⁴ moles.
- **Charge Required**: Each mole of Cl₂ requires 2 moles of electrons for its production (based on the reaction: 2Cl⁻ → Cl₂ + 2e⁻). Hence, the total moles of electrons needed:
- Moles of electrons = 2 × 1.66 × 10⁻²⁴ = 3.32 × 10⁻²⁴ moles.

Calculating Charge
- **Total Charge (Q)**: Using Faraday's constant (F = 96500 C/mol), the charge required can be calculated:
- Q = Moles of electrons × Faraday's constant
- Q = 3.32 × 10⁻²⁴ moles × 96500 C/mol = 3.21 × 10⁻¹⁹ C.

Time Calculation
- **Using the formula**: \( t = \frac{Q}{I} \), where I is the current (3 A):
- \( t = \frac{3.21 × 10⁻¹⁹ C}{3 A} \)
- \( t = 1.07 × 10⁻¹⁹ \) seconds.
Thus, the time required to produce 0.10 molecules of chlorine gas using a current of 3 amperes is approximately \( 1.07 × 10⁻¹⁹ \) seconds.