Question

The mass of silver (Molar mass of Ag : 108 gmol–1 ) displaced by a quantity of electricity which displaces 5600 mL of O2 at S.T.P. will be _____ g.

Answer 1

The equation for the equivalent of Ag is:

$\text{Eq. of Ag} = \text{Eq. of } O_2$

Let x grams of silver be displaced.

$\frac{x}{108} = \frac{5.6}{22.7} \times 4$

Using the molar volume of gas at STP (22.7 L), we get:

$x = 106.57 \, \text{g}$

Thus, the answer is approximately 107 g.

Alternatively, using 22.4 L as the molar volume at STP:

$\frac{x}{108} = \frac{5.6}{22.4} \times 4$

which gives $x = 108 \, \text{g}$.

Answer 2

The equation for the equivalent of Ag is:

$\text{Eq. of Ag} = \text{Eq. of } O_2$

Let x grams of silver be displaced.

$\frac{x}{108} = \frac{5.6}{22.7} \times 4$

Using the molar volume of gas at STP (22.7 L), we get:

$x = 106.57 \, \text{g}$

Thus, the answer is approximately 107 g.

Alternatively, using 22.4 L as the molar volume at STP:

$\frac{x}{108} = \frac{5.6}{22.4} \times 4$

which gives $x = 108 \, \text{g}$.