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During the electrolysis of molten sodium chloride the time required to produce 0.10 molecules of chlorine gas using a current of 3 ampere?
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During the electrolysis of molten sodium chloride the time required to...
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.
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During the electrolysis of molten sodium chloride the time required to produce 0.10 molecules of chlorine gas using a current of 3 ampere?
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