The mass of silver (Molar mass of Ag: ) displaced by a quantity of electricity which displaces 5600 mL of at S.T.P. will be g.

Question

The mass of silver (Molar mass of Ag: ) displaced by a quantity of electricity which displaces 5600 mL of  at S.T.P. will be  g.

Canvas Classes · Accepted Answer

Strategy:
 Use Faraday's Laws of Electrolysis to equate the charge required for gas production and metal deposition. Convert gas volume to Faradays and then to the mass of displaced silver.

Step 1: Calculate moles of oxygen at STP
Volume .
Molar volume at STP .

Step 2: Relate to Faradays
The oxidation of water is: .
Stoichiometry: 1 mole of  requires .
Total charge passed .

Step 3: Calculate mass of Silver
For Silver reduction: .
 deposits 1 mole of Silver.
Mass .

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