An aqueous solution of an unknown salt of ruthenium is...

An aqueous solution of an unknown salt of ruthenium is electrolyzed by a current of $2.50$ A passing for $50.0 \mathrm{~min}$. If $2.618 \mathrm{~g}$ Ru is produced at the cathode, what is the charge on the ruthenium ions in solution?

Key Concepts

Ionic Charge and Oxidation States

Determining the charge on a metal ion involves understanding its oxidation state in the reaction. In electrolysis, the number of electrons used to deposit the metal correlates directly with the ionic charge. By comparing the moles of electrons transferred (calculated from the charge passed) to the moles of metal deposited, one can deduce the charge (or oxidation state) of the metal ion in solution.

Redox Reactions and Electron Transfer

Electrochemical reactions involve the gain or loss of electrons in oxidation-reduction (redox) processes. In an electrolytic cell, the ion at the cathode is reduced by gaining electrons, and the number of electrons required to reduce one ion determines its charge and oxidation state.

Current, Time, and Charge Relationship

The total charge passed in an electrolysis experiment is determined by multiplying the current (measured in amperes) by the time (in seconds). This basic principle is crucial because the charge directly influences the moles of electrons available for the reduction of ions at the electrode.

Faraday's Laws of Electrolysis

Faraday's laws establish the quantitative relationship between the amount of substance altered at an electrode and the total electric charge passed through the electrolyte. This concept allows us to compute the number of moles of electrons transferred during electrolysis using the relationship Q = I × t and then relate this to the mass of the substance deposited.

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