When current of 15A was passed through electrolyte solution for fifteen minutes determine in coulomb the quantity of charge flowed What mass of copper will be deposited when a mass of copper will be deposited when s current of 5C passes through an electrolytic cell for 15 minutes 33 seconds

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2 parts
1

13500 C\text{13500 C}

2

1.536 g\text{1.536 g}

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Part 1· 2 steps

Determine the quantity of charge flowed.

  1. Convert the time from minutes to seconds.

    t=15 minutes×60 seconds1 minute=900 secondst = 15 \text{ minutes} \times \frac{60 \text{ seconds}}{1 \text{ minute}} = 900 \text{ seconds}

  2. Calculate the quantity of charge (QQ) using the formula Q=I×tQ = I \times t.

    Q=15 A×900 sQ = 15 \text{ A} \times 900 \text{ s} Q=13500 CQ = 13500 \text{ C}

    The quantity of charge flowed is 13500 C\boxed{\text{13500 C}}.

Part 2

1.536 g\text{1.536 g}

Determine the mass of copper deposited.

Assumption: The phrase "current of 5C" is interpreted as "current of 5A", as current is measured in Amperes (A) and charge in Coulombs (C).

  1. Convert the time from minutes and seconds to total seconds.

    t=15 minutes 33 secondst = 15 \text{ minutes } 33 \text{ seconds} t=(15×60) s+33 st = (15 \times 60) \text{ s} + 33 \text{ s} t=900 s+33 st = 900 \text{ s} + 33 \text{ s} t=933 st = 933 \text{ s}

  2. Calculate the total charge (QQ) passed using the formula Q=I×tQ = I \times t.

    Q=5 A×933 sQ = 5 \text{ A} \times 933 \text{ s} Q=4665 CQ = 4665 \text{ C}

  3. Identify the necessary constants for copper deposition.

    • Molar mass of copper (MM) = 63.55 g/mol63.55 \text{ g/mol}
    • Valency of copper (nn) = 2 (for Cu2+\text{Cu}^{2+} ions)
    • Faraday's constant (FF) = 96485 C/mol96485 \text{ C/mol}

  4. Apply Faraday's First Law of Electrolysis to find the mass (mm) of copper deposited.

    m=Q×Mn×Fm = \frac{Q \times M}{n \times F} m=4665 C×63.55 g/mol2×96485 C/molm = \frac{4665 \text{ C} \times 63.55 \text{ g/mol}}{2 \times 96485 \text{ C/mol}} m=296400.75 g192970m = \frac{296400.75 \text{ g}}{192970} m≈1.536 gm \approx 1.536 \text{ g}

    The mass of copper deposited is 1.536 g\boxed{\text{1.536 g}}.

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