If current of 4.5A is used to find time taken for 5.5g of gold deposited. Given Au is 197 and 1 Faraday = 96500C
To find the time taken for gold to be deposited, we can use Faraday's law of electrolysis, which states that the amount of substance deposited is directly proportional to the current and the time.
The formula to calculate the time taken is as follows:
Time (t) = (Mass of Substance (m) * Atomic Mass (M)) / (Current (I) * Faraday's Constant (F))
Given:
Current (I) = 4.5 A
Mass of gold (m) = 5.5 g
Atomic mass of gold (M) = 197 g/mol
Faraday's Constant (F) = 96500 C/mol
Plugging in the given values into the formula:
Time (t) = (5.5 g * 197 g/mol) / (4.5 A * 96500 C/mol)
Simplifying the expression:
Time (t) = (5.5 g * 197) / (4.5 * 96500)
Time (t) = 1.204 / 433.5
Time (t) ≈ 0.265 seconds
Therefore, the time taken for 5.5g of gold to be deposited with a current of 4.5A is approximately 0.265 seconds.
To find the time taken for the deposition of gold using a current of 4.5A, we can use the formula:
Time (t) = (Amount of Substance (n) * Atomic Mass (M)) / (Current (I) * Faraday's Constant (F))
Given:
Current (I) = 4.5 A
Amount of Substance (n) = 5.5 g / Atomic Mass (M) of Gold (Au) = 5.5 g / 197 g/mol
Faraday's Constant (F) = 96500 C/mol
First, let's calculate the amount of substance using the given mass and atomic mass:
Amount of Substance (n) = 5.5 g / 197 g/mol ≈ 0.0279 mol
Now let's substitute the values into the formula and calculate the time:
Time (t) = (0.0279 mol * 197 g/mol) / (4.5 A * 96500 C/mol)
Simplifying the equation:
Time (t) ≈ (5.4863 g) / (435750 C)
Time (t) ≈ 1.26 * 10^-5 s
Therefore, the time taken for the deposition of 5.5g of gold using a current of 4.5A is approximately 1.26 * 10^-5 seconds.