This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.

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Answer
N270.00
To solve this problem, we will use Faraday's laws of electrolysis, which relate the mass of a substance deposited to the quantity of electricity passed and its equivalent mass.
Given Information:
Assumptions for Valency:
Step 1: Calculate the equivalent mass for Aluminium and Copper. The equivalent mass () is given by the formula: .
For Aluminium:
For Copper:
Step 2: Determine the cost per equivalent for Aluminium. We are given that it costs N40 to deposit 1 g of Aluminium. First, find how many equivalents are in 1 g of Aluminium: Now, we can find the cost to deposit 1 equivalent of Aluminium:
Step 3: Calculate the cost to deposit 24 g of Copper. According to Faraday's second law, the same quantity of electricity (and thus the same cost) will deposit one equivalent of any substance. Therefore, the cost per equivalent for Copper will also be N360.
First, find how many equivalents are in 24 g of Copper: Now, calculate the total cost to deposit 24 g of Copper:
Comparing this to the given options, the correct answer is N270.00.
The final answer is .
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Given Information: Cost to deposit 1 g of Aluminium (Al) = N40 Molar mass of Al (M_Al) = 27 g/mol Molar mass of Copper (Cu) (M_Cu) = 64 g/mol Mass of Copper to be deposited (m_Cu) = 24 g Assumptions for Valency: Aluminium typically forms Al³⁺ ions, so…
This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.