Question

How many hours are required to produce 1.00 x

103kgof sodium by the electrolysis of molten NaCl with a
constantcurrent of 3.00 x 104 A?

Answer 1

Answer: 42 hours

Step-by-step explanation:

Moles of electron = 1 mole

According to mole concept:

1 mole of an atom contains
`6.022* 10^(23)` number of particles.

We know that:

Charge on 1 electron =
`1.6* 10^(-19)C`

Charge on 1 mole of electrons =
`1.6* 10^(-19)* 6.022* 10^(23)=96500C`

`NaCl\rightarrow Na^++Cl^-`

`Na^++e^-\rightarrow Na`

According to stoichiometry:

1 mole of electrons deposit = 23 g of sodium

i.e 96500 C of electricity deposit = 23 g of sodium

Thus 23 g of sodium is deposited by = 96500 C of electricity

`1.00* 10^3kg=1.00* 10^6g` of sodium is deposited by =
`(96500)/(23)* 1.00* 10^6=4.20* 10^9` C of electricity

To calculate the time required, we use the equation:

`I=(q)/(t)`

where,

I = current passed =
`3.00* 10^4A`

q = total charge =
`4.20* 10^9`

t = time in secods = ?

Putting values in above equation, we get:

`3.00* 10^4A=(4.20* 10^9)/(t)`

`t=1.4* 10^5sec=42hr`
`(1sec= 0.0003hr`

Thus 42 hours are required.