When same quantity of electricity is passed through aqueous AgNO3 and H2SO4 solutions connected in series, 5.04 × 10-2 g of H2 is liberated. What is the mass of silver (in grams) deposited? (Eq. wts. of hydrogen = 1.008, silver = 108)

Question

When same quantity of electricity is passed through aqueous AgNO3 and H2SO4 solutions connected in series, 5.04 × 10-2 g of H2 is liberated. What is the mass of silver (in grams) deposited? (Eq. wts. of hydrogen = 1.008, silver = 108) (A) 54 (B) 0.54 (C) 5.4 (D) 10.8

Tardigrade Admin · Accepted Answer

Given, weight of hydrogen liberated =5.04 × 10-2 g Eq. wt. of hydrogen =1.008 Eq. wt. of silver =108 Weight of silver deposited, w =? According to Faraday's second law of electrolysis ( text weight of silver deposited / text weight of hydrogen liberated ) =( text eq. wt .of silver / text eq. wt. of hydrogeon ) (w/5.04 × 10-2)=(108/1.008) W=(108 × 5.04 × 10-2/1.008) =5.4 g

Q. When same quantity of electricity is passed through aqueous AgNO3​ and H2​SO4​ solutions connected in series, 5.04×10−2g of H2​ is liberated. What is the mass of silver (in grams) deposited? (Eq. wts. of hydrogen = 1.008, silver = 108)

54

0.54

5.4

10.8

Q. When same quantity of electricity is passed through aqueous $A g N O_{3}$ and $H_{2} S O_{4}$ solutions connected in series, $5.04 \times 1 0^{- 2} g$ of $H_{2}$ is liberated. What is the mass of silver (in grams) deposited? (Eq. wts. of hydrogen = $1.008,$ silver = $108$ )