Final answer:
The half-cell reaction for chlorine production is 2Cl⁻(aq) → Cl₂(g) + 2e⁻. To find the total current for worldwide chlorine production, use the annual production figure and adjust for plant operation time. Electrical power is then calculated by multiplying the total current by the operating voltage.
Step-by-step explanation:
The question is related to the electrolysis process for the production of chlorine gas (Cl₂) from chloride ions (Cl⁻).
Calculation of Mass of Chlorine Produced
To answer part (a), the half-cell reaction for the oxidation of chloride ions to form chlorine gas is:
2Cl⁻(aq) → Cl₂(g) + 2e⁻.
Total Current Calculation
In part (b), to determine the worldwide current needed to generate the annual supply of Cl₂, we need to use Faraday's laws of electrolysis and the annual production:
The electrochemical equivalent of Cl₂ can be calculated from the molar mass of Cl₂ and the charge carried by one mole of electrons (Faraday's constant).
Then, multiply the production value by the electrochemical equivalent to obtain the total charge required per year.
Since a typical plant is operational for 90% of the year, adjust the required charge for the actual operational time.
Divide the total annual charge by the operational seconds per year to get the total current.
Electrical Power Calculation
For part (c), the electrical power needed is obtained by multiplying the total current by the operating voltage:
Power (Watts) = Current (Amps) × Voltage (Volts)
Convert this power to kilowatt-hours to compare it to the power needed for the production of other chemicals or for domestic use.
Overall, these calculations require understanding of electrochemistry concepts such as Faraday's laws, the definition of current and power in an electrical circuit, and practical considerations for industrial electrolytic processes.