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Natali [406]
2 years ago
13

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

ll have been done when 0.487 mL of Br2(l) has been consumed
Chemistry
1 answer:
Yuri [45]2 years ago
8 0

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}

Read more about Work

brainly.com/question/756198

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Answer:

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PH7

Biochemical standard state:

Temperature is 25°

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Constant value of Mg2+

Both:

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g. Presurre is 1 atm.

Temperature is 25°

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