Question

The weight of silver (at. $wt.=108$ ) displaced by a quantity of electricity which displaces $5600mL$ of $O_2$ at $STP$ will be

• A. 5.4 g
• B. 10.8 g
• C. 54 .0 g
• D. 108.0 g
  

Answer 1

Answer: (D)

At STP, $1$ mole of oxygen occupies $22400mL$.
Hence, the number of moles of oxygen corresponding to $5600ml$ is
$n_{O_2}=\frac{5600}{22400}=\frac{1}{4}=\frac{W_{O_2}}{M_{O_2}}$.
$1$ mole of oxygen produces $4$ moles of lectrons and $1$ mole of silver requires 1 mole of electrons.
$\frac{W_{Ag}}{M_{Ag}}\times 1=\frac{W_{O_2}}{M_{O_2}}\times 4$
$\frac{W_{Ag}}{M_{Ag}}\times 1=\frac{1}{4}\times 4$
$\frac{W_{Ag}}{108}=\frac{1}{4}\times 4$
$W_{Ag}=108g$
Thus, the weight of silver displaced by a quantity of electricity which displaces $5600m{l}_2{O}_2$ at STP will be $108.0g$.