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Calculate the weight of metal deposited when a current of 15 A with 75% current efficiency is passed through the cell for 2 hours. (Given : Z = 0.0004)

bobpursley bobpursley answered

weight=current*time*Z*efficiency=15*(120*60)*.0004*.75=....

Step-by-Step Bot Step-by-Step Bot answered

To calculate the weight of metal deposited, you can use the formula:

Weight = (Current × Time × Z × Efficiency) / 96500

where:
- Current is the electric current in amperes,
- Time is the time in seconds,
- Z is the electrochemical equivalent of the metal, and
- Efficiency is the current efficiency as a decimal.

Given that the current is 15 A, time is 2 hours (converted to seconds is 7200 s), Z is 0.0004, and efficiency is 75% (converted to 0.75), we can substitute these values into the formula:

Weight = (15 A × 7200 s × 0.0004 × 0.75) / 96500

Simplifying the calculation:

Weight = 0.004365

Therefore, the weight of metal deposited when a current of 15 A with 75% current efficiency is passed through the cell for 2 hours is 0.004365 grams.

Explain Bot Explain Bot answered

To calculate the weight of metal deposited, we can use Faraday's law of electrolysis, which states that the amount of metal deposited is directly proportional to the current passing through the cell and the time.

The equation we can use is:

Weight of metal deposited (in grams) = (Current × Time × Atomic Weight) / (Equivalent Weight × 1000)

Where:
- Current: the current passing through the cell in amperes (A)
- Time: the duration for which the current is passed in hours (h)
- Atomic Weight: the atomic weight of the metal in grams per mole (g/mol)
- Equivalent Weight: the equivalent weight of the metal in grams per mole (g/mol)

In this case, we are given:
- Current = 15 A
- Time = 2 hours
- Atomic Weight (Z) = 0.0004 g/mol

To calculate the equivalent weight, we need to know the stoichiometry of the reaction. Since that information is not provided, we can assume it is 1:1. Therefore, the equivalent weight will be the same as the atomic weight.

Equivalent Weight = Atomic Weight = 0.0004 g/mol

Substituting the values into the formula:

Weight of metal deposited (in grams) = (15 A × 2 h × 0.0004 g/mol) / (0.0004 g/mol × 1000)

Calculating:

Weight of metal deposited (in grams) = (0.012 g) / (0.0004)

Weight of metal deposited (in grams) = 30 grams

Therefore, the weight of metal deposited when a current of 15 A with 75% current efficiency is passed through the cell for 2 hours is 30 grams.