108 g of silver (molar mass ) is deposited at cathode from solution by a certain quantity of electricity. The volume (in L) of oxygen gas produced at 273 K and 1 bar pressure from water by the same q

Question

108 g of silver (molar mass ) is deposited at cathode from  solution by a certain quantity of electricity. The volume (in L) of oxygen gas produced at 273 K and 1 bar pressure from water by the same quantity of electricity is .

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Strategy:
 Identify the relationship between the mass of a substance deposited at one electrode and the volume of gas produced at another using Faraday's Laws. Calculate the total charge passed and apply it to the stoichiometry of water electrolysis.

Step 1: Calculate moles of Ag and charge passed
The reduction of silver proceeds as: .
- Moles of Ag () .
- Since 1 mole of Ag requires 1 mole of electrons, charge passed .

Step 2: Determine moles of oxygen produced
The oxidation of water at the a

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