91Ó°ÊÓ

This problem is related to Faraday's Law of electrolysis, states as "mass of substance deposited or discharged is directly proportional to the electricity passed through the cell".

Mathematically given by, $m∞Q$

Relative uncertainty = ( absolute uncertainty $÷$best estimate )$×100\%$

According to faraday 1 Faraday (96500C) of current is required to deposit or discharge 1 Equivalent weight of the substance.

Given that

Atomic mass of Ag is 107.868, is also the equivalent weight of silver.

Determination of Faraday Constant

1F = charge on electron $×$Avogadro number

$$\begin{gathered} 1\mathrm{F}=1.6×{10}^{-19}\mathrm{C}×6.023×{10}^{23} \\ =96368\mathrm{C} \end{gathered}$$

Therefore 1F = 96368C is the calculated value of the Faraday constant.

Relative uncertainty = ( absolute uncertainty$÷$best estimate )$×100\%$

So from the above:

Relative uncertainty $$\begin{gathered} =\frac{132×100}{96368} \\ =0.1369\% \end{gathered}$$

The value can therefore be quoted as role="math" localid="1654772237672" $96368CÂ\pm 0.1369\%$.is the uncertainty. And the Uncertainty value is

$\frac{96368×0.1369}{100}×132$

And the real Faraday constant will be$96368CÂ\pm 132=96500C$