If the cell is somehow operated under conditions in which it produces a constant voltage of 1.50 V , how much electrical work wi

Question

1 year ago

13

ll have been done when 0.487 mL of Br2(l) has been consumed

1 answer:

Yuri [45] · Answer 1 · 2023-08-27T12:13:08+03:00

For a cell operated to produce a constant voltage of 1.50 V, the electrical work done is mathematically given as

W=2.077*10^{-7}

<h3>What is the electrical work done?</h3>

Generally, the volume of Br2 is mathematically given as

$Vb=\frac{0.38*3.12}{159.809}$

Vb=7.18*10^-3ml

Therefore, the quantity of charge

q=(1.436*10^-2)*9.644*10^4

q=1.385^{-4}c

In conclusion, work done

W=Eq

W=1.50*1.385^{-4}

W=2.077*10^{-7}