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.
ScanSolve AI Answer
This problem requires applying Faraday's First Law of Electrolysis. Given: Mass of metal M deposited (m) = 0.66 g Current (I) = 1.35 A Time (t) = 1500 s Metal M is divalent, meaning its valency (z) = 2. Faraday's constant (F) = 96500 C/mol (This is a standard constant you should know for electrolysis problems). Step 1: Calculate the total quantity of electricity (charge, Q) passed. The formula for charge is Q = I × t. Q = 1.35 A × 1500 s Q = 2025 C Step 2: Use Faraday's First Law to calculate the Relative Atomic Mass (RAM) of M. Faraday's First Law states that the mass deposited (m) is given by: m = RAM × Qz × F We need to find RAM (which is the molar mass, M). Rearrange the formula: RAM = (m × z × F)/(Q) Substitute the known values: RAM = 0.66 g × 2 × 96500 C/mol2025 C RAM = (127380)/(2025) g/mol RAM ≈ 62.9037 g/mol Rounding to three significant figures: RAM ≈ 62.9 g/mol The relative atomic mass (RAM) of M is 62.9.