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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?

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

Step-by-step explanation:

We are given:

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)=9.6352* 10^4C

To calculate the time required, we use the equation:


I=(q)/(t)

where,

I = current passed = 2.17 A

q = total charge =
9.6352* 10^4C

t = time required = ?

Putting values in above equation, we get:


2.17A=(9.6352* 10^4C)/(t)\\\\t=(9.6352* 10^4C)/(2.17A)=44402s

Converting this into hours, we use the conversion factor:

1 hr = 3600 seconds

So,
44402s* (1hr)/(3600s)=12.33hr

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

User Trenton Tyler
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