Calculate the the current that must be passed into a solution of aluminium salt for 1hour30minutes In order to deposite 1.5gram I aluminium (Al=27).
To determine the current that must be passed into the solution of aluminum salt, we must first calculate the number of moles of aluminum (Al) that needs to be deposited.
We are given that 1.5 grams of aluminum (Al) needs to be deposited and the molar mass of aluminum is 27 g/mol.
Number of moles of aluminum (Al) = Mass / Molar mass
Number of moles of aluminum (Al) = 1.5 g / 27 g/mol
Next, we will convert the time of 1 hour 30 minutes into seconds.
1 hour = 60 minutes
1 minute = 60 seconds
1 hour 30 minutes = 1 × 60 × 60 seconds + 30 × 60 seconds = 5400 + 1800 seconds = 7200 seconds
Now, we can calculate the current using Faraday's law of electrolysis.
Faraday's law of electrolysis states that the amount of substance deposited or liberated during electrolysis is directly proportional to the quantity of electricity passed.
Number of moles of aluminum (Al) deposited = Charge / (Faraday's constant × Charge of aluminum ion)
Number of moles of aluminum (Al) deposited = Charge / (96500 C × 3+ charge of aluminum ion)
Now, we can rearrange the equation to solve for the charge.
Charge = Number of moles of aluminum (Al) deposited × (96500 C × 3+ charge of aluminum ion)
Charge = (1.5 g / 27 g/mol) × (96500 C × 3)
Finally, we can calculate the current by dividing the charge by the time.
Current = Charge / Time
Current = [(1.5 g / 27 g/mol) × (96500 C × 3)] / 7200 seconds