An unknown metal M is electrolyzed. It took 74.1 s for a current of 2.00 A to plate out 0.107

step 1 So this is one of those unit conversions with the twist for electrolysis. If we knew the molar m

An unknown metal M is electrolyzed. It took 74.1 s for a...

An unknown metal $\mathrm{M}$ is electrolyzed. It took $74.1 \mathrm{~s}$ for a current of $2.00 \mathrm{~A}$ to plate out $0.107 \mathrm{~g}$ of the metal from a solution containing $\mathrm{M}\left(\mathrm{NO}_{3}\right)_{3}$. Identify the metal.

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Key Concepts

Stoichiometry of Electrochemical Reactions

This concept involves the interpretation of the reduction process in terms of electrons transferred. In cases where metal ions have a specific valence, the stoichiometry directly relates the number of electrons needed to reduce one ion to the metal. This helps in determining the molar relationships required to compute the atomic mass.

Determination of Atomic Weight

By combining the known mass of the deposited metal with the calculated moles of electrons (adjusted for the valence of the ion), the atomic weight of the unknown metal can be deduced. This process involves comparing the experimental molar mass with known values to identify the metal.

Faraday's Laws of Electrolysis

These laws state that the mass of a substance produced at an electrode during electrolysis is directly proportional to the amount of electric charge passed through the electrolyte. This concept is essential for relating the quantity of electricity (in coulombs) to the amount of metal deposited.

Coulomb's Law for Charge Transfer

This principle involves calculating the total charge transferred in an electrolytic process using the relationship Q = I × t, where I is the current and t is the time. It provides the necessary link between the electrical parameters and the chemical changes occurring during the electrolysis.

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