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During the electrolysis of aqueous silver nitrate, a current of 5.0 A was passed through the electrolyte for 3 hours.

      

During the electrolysis of aqueous silver nitrate, a current of 5.0 A was passed through the electrolyte for 3 hours.
a) Write the equation for the reaction which took place at the anode
b) Calculate the mass of silver deposited. (Ag = 108; IF = 96500 C)

  

Answers


John
a) 4OH-(aq) $\rightarrow$ 4e + 2H2O(l) + O2(g)

b) Q = It

= 5 x 3 x 60 x 60 = 54000 C

Mass of silver deposited = $\frac{108\times 54000}{96500}$

= 60.44 g
johnmulu answered the question on February 16, 2017 at 06:55


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