Question

How many moles of mercury will be produced by electrolysing 1 M Hg(NO3)2 solution with a current of 2A for 3 hours.??? plzz answer urgently

Answer 1

Hey Friend, Here's your answer
Quantity of electricity passed = (2A) x (3 x 60 x 60s) = 21600 C Thus, 2F i.e. 2 x 96500 C deposit Hg = 1 mole 21600 C will deposit Hg
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Answer 2

Given:

Molarity = 1M

Current = 2A

Time = 3 hours

To find:

Number of moles of mercury produced by electrolysis.

Calculation:

During electrolysis, the fate of Hg is

$Hg^{2+}+2e^-\rightarrow Hg$

The above equation, represents that , $Hg^{2+}$ loses to electron and becomes stable Hg element.

With this concept, the amount of electron passing through the cathode is calculated as

Amount of electron passing = 2×3×3600        (current×time)

Amount of electron passing = 21600C

As 1 C of of electrons = $1.036\times 10^{-5}$ mol

21600 C of electron = $21600\times 1.036\times 10^ {-5}$ = 0.224 mol

As for formation of one mole of Hg, two electrons are released, the mole ratio of Hg and electron is 1:2

Thus the number of moles produced = $\frac{0.224}{2} = 0.112 moles$

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