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If the cell is somehow operated under conditions in which it produces a constant voltage of 1.50 V , how much electrical work will have been done when 0.487 mL of Br2(l) has been consumed

Sagot :

okpalawalter8

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}

What is the electrical work done?

Generally, the volume of Br2  is mathematically given as

[tex]Vb=\frac{0.38*3.12}{159.809}[/tex]

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}

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