A Steel Spoon Is To Be Electroplated With Silver ,how Long Should A Current Of 1.5A Be passed though a silver nitrate solution in order to deposit 54g of silver metal on the spoon?
moles Silver=54/107.9=.5 moles
electrons in .5 moles=.5*avagnumber.
current*time=totalcharge=.5*avagnumber*chargeperelectron
time= .5*avanumber*1.6e-19/1.5 seconds
What mass of copper will be deposited froma solution of copper (2)sulphate when a current of 7.5A is passed through for 1 minute and 40 second
To determine how long a current should be passed through a silver nitrate solution to deposit 54g of silver metal on a steel spoon, we need to use a concept called Faraday's Law of Electrolysis.
Faraday's Law states that the amount of substance produced (or consumed) during electrolysis is directly proportional to the number of moles of electrons that pass through the circuit. The equation relating these quantities is:
mass (g) = (current (A) × time (s) × molar mass (g/mol)) / (charge of 1 electron (C))
In this case, we want to deposit 54g of silver (Ag) on the spoon. The molar mass of silver is approximately 107.87 g/mol. The charge of one electron is 1.602 × 10^-19 C.
We can rearrange the equation to solve for time:
time (s) = (mass (g) × charge of 1 electron (C)) / (current (A) × molar mass (g/mol))
Plugging in the given values, we have:
time (s) = (54g × 1.602 × 10^-19 C) / (1.5A × 107.87 g/mol)
Calculating this expression will give us the time required to deposit 54g of silver on the spoon when a current of 1.5A is passed through the silver nitrate solution.