How many seconds are required to produce 1.0 g of silver metal by the electrolysis of a AgNO₃ solution using a current of 5.0 amps?

Question

Quizplus · Accepted Answer

The correct answer is C because the amount of substance produced by electrolysis is directly proportional to the current and the time. The time required to produce 1.0 g of silver metal can be calculated using the formula:```t = (m * z * F) / (I * A)```where:* t is the time in seconds* m is the mass of the substance produced in grams* z is the number of electrons transferred per mole of the substance* F is the Faraday constant (96,485 C/mol)* I is the current in amps* A is the atomic mass of the substanceFor silver, z = 1 and A = 107.87 g/mol. Substituting these values into the formula, we get:```t = (1.0 g * 1 * 96,485 C/mol) / (5.0 A * 107.87 g/mol) = 180 s```

How Many Seconds Are Required to Produce 1