Question

When aqueous $AgN{O}_3$ is electrolyzed using Pt electrodes, if 3.2 g of $O_2$ is liberated at the anode, the Amount of Ag that will be deposited at the cathode in grams is (at wt. of Ag = 108)

• A. 32 g
• B. 1.6 g
• C. 4.32 g
• D. 43.2 g

Answer 1

The correct option is D

43.2 g

$A{g}^{+}+e\to Ag;$

$\text{Eq. wt of 'Ag'}{E}_{Ag}=\frac{108}{1}=108g(atomicmassofAg=108)$

$20H^{-}\to O_2+2H^{+}+4e;$

Eq. wt of ${}^{\prime }{O}_2^{\prime }$ $E_{o2}$ = $\frac{32}{4}=8g$ $(Molarmassof{O}_2=32)$

$\text{When same quantity of electricity is passes}$

$\text{no. of eqts of 'Ag' = no. of eqts of}{}^{\prime }{O}_2^{\prime }$

$\frac{W_{Ag}}{E_{Ag}}=\frac{W_{O_2}}{E_{O_2}};\frac{W_{Ag}}{108}=\frac{3.2}{8};W_{Ag}=43.2g$