A 1.0 L solution of CaF2 was electrolyzed for 14.7 h to give 99.47 g of calcium. Assuming the minimum voltage needed was avalible, what amperage would be needed to complete the electrolysis in the given time

The amperage needed to complete the electrolysis in the given time is 9.08 A

Explanation:

We are given:

Moles of electron = 1 mole

According to mole concept:

1 mole of an atom contains number of particles.

We know that:

Charge on 1 electron =

Charge on 1 mole of electrons =

moles of calcium =

is required to deposit = 1 mole

Thus 1 mole is deposited by = 193000 C

2.49 moles will be deposited by =

To calculate the time required, we use the equation:

where,

I = current passed = ?

q = total charge =

t = time required = 14.7 hours =52920 s  ( 1hour=3600s)

Putting values in above equation, we get:

Hence, the amperage needed to complete the electrolysis in the given time is 9.08 A

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