Gold is produced electrochemically from an aqueous solution of Au(CN)2^- containing an excess of

step 1 In this problem, we are told that gold is produced electrochemically from a solution in water of

Gold is produced electrochemically from an aqueous solution...

Gold is produced electrochemically from an aqueous solution of $\mathrm{Au}(\mathrm{CN})_{2}^{-}$ containing an excess of $\mathrm{CN}^{-}$. Gold metal and oxygen gas are produced at the electrodes. What amount (moles) of $\mathrm{O}_{2}$ will be produced during the production of $1.00 \mathrm{~mol}$ gold?

Key Concepts

Electrolysis

Electrolysis is the process of using electrical energy to drive chemical reactions that would not otherwise occur spontaneously. In the context of the problem, electrolysis is used to reduce gold ions to form gold metal at one electrode, while simultaneously oxidizing species to produce oxygen gas at the other electrode.

Electrode Reactions

Electrode reactions refer to the oxidation and reduction processes that occur at the anode and cathode, respectively, in an electrochemical cell. Understanding these half-reactions is essential for establishing the stoichiometric relationships between reactants and products, such as determining the ratio of electrons involved in the formation of oxygen compared to the reduction of gold ions.

Stoichiometry in Electrochemistry

Stoichiometry in electrochemistry involves calculating the mole relationships of substances involved in the half reactions of an electrochemical process. By balancing the number of electrons transferred in the oxidation and reduction reactions, one can determine how many moles of one product, like oxygen gas, are generated for a given amount of another product, such as gold metal.

Faraday's Laws of Electrolysis

Faraday's laws of electrolysis quantitatively relate the amount of substance produced at an electrode to the electric charge passed through the electrolyte. These laws serve as the foundation for calculating product quantities in electrochemical reactions by linking the number of moles of electrons transferred to the mass or moles of material deposited or evolved at an electrode.

Transcript

Please give Ace some feedback