Question

A lamp has a current of 2.17 A. In hours, how long does it take for 1 mole of electrons to pass through the lamp?

Answer 1

Answer: The amount of time needed for 1 mole of electrons to pass through the lamp is 12.33 hrs.

Explanation:

We are given:

Moles of electron = 1 mole

According to mole concept:

1 mole of an atom contains $6.022\times 10^{23}$ number of particles.

We know that:

Charge on 1 electron = $1.6\times 10^{-19}C$

Charge on 1 mole of electrons = $1.6\times 10^{-19}\times 6.022\times 10^{23}=9.6352\times 10^4C$

To calculate the time required, we use the equation:

$I=\frac{q}{t}$

where,

I = current passed = 2.17 A

q = total charge = $9.6352\times 10^4C$

t = time required = ?

Putting values in above equation, we get:

$2.17A=\frac{9.6352\times 10^4C}{t}\\\\t=\frac{9.6352\times 10^4C}{2.17A}=44402s$

Converting this into hours, we use the conversion factor:

1 hr = 3600 seconds

So, $44402s\times \frac{1hr}{3600s}=12.33hr$

Hence, the amount of time needed for 1 mole of electrons to pass through the lamp is 12.33 hrs.