0.45g of metal was deposited when a current of 1.8A is passed through a solution of its salt of 12.5m using appropriate electrode?
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To calculate the amount of metal deposited, you need to know the molar mass (M) of the metal. You also need to consider the Faraday's law of electrolysis, which states that the amount of metal deposited is directly proportional to the charge passed through the solution.
The formula to calculate the amount of metal deposited is:
Amount (in moles) = (Current x Time) / (Charge per mole of electrons)
Here's how you can calculate the amount of metal deposited:
1. Find the charge per mole of electrons (F):
- F is the Faraday's constant, which is approximately 96,485 Coulombs/mole.
2. Calculate the charge (Q) passed through the solution using the current (I) and time (t):
- Q = I x t
- In this case, I = 1.8 Amperes (A) and t = 12.5 seconds (s).
3. Calculate the amount of metal deposited (in moles) using the formula:
- Amount = (Current x Time) / Charge per mole of electrons
- Substitute the values: Amount = (1.8 A x 12.5 s) / 96,485 C/mol
4. Convert the amount of metal deposited from moles to grams:
- Multiply the amount (in moles) by the molar mass (M) of the metal.
Note: Make sure to use consistent units throughout the calculations.