For how long must a current of 1.5 ampares be passed through an aqueous solution of a copper salt .during electrolysis in order to deposited 2.50g of copper (cu 63.5)?
how many atoms in 2.50g?
How many electrons will be needed?
1.5A = 1.5 coulomb/second
time = quantity/rate
I need the solution
To find out the time required for the deposition of 2.50g of copper during electrolysis, we can use Faraday's law of electrolysis. The equation is as follows:
Mass of substance deposited = (Current × Time × Molar mass) / (Faraday's constant × Charge of the ion)
In this case, we want to find the time, so we rearrange the equation:
Time = (Mass of substance deposited × Faraday's constant × Charge of the ion) / (Current × Molar mass)
Now, let's break down the given information:
Current = 1.5 amperes
Mass of substance deposited = 2.50g
Molar mass of copper (Cu) = 63.5g/mol
Charge of the copper ion (Cu2+) = 2 (since copper usually forms a divalent ion)
Faraday's constant = 96500 C/mol (the charge of 1 mole of electrons)
Let's plug in the values into the equation:
Time = (2.50g × 96500 C/mol × 2) / (1.5 A × 63.5 g/mol)
Now we can calculate:
Time = (482500 C × 2) / 95.25 C ≈ 10,131 seconds
Therefore, a current of 1.5 amperes must be passed through the aqueous solution for approximately 10,131 seconds to deposit 2.50g of copper.