Question

How many seconds are required to deposit 0.277 grams of silver metal from a solution that contains Ag⁺ ions, if a current of 0.655 A is applied.
_____ s

How many seconds are required to deposit 0.223 grams of silver metal from a solution that contains Ag⁺ ions, if a current of 0.856 A is applied.
____ s

Answer 1

1)

the electrolysis expression is:

Ag1+ + 1e- ------> Ag

1 mol of Ag requires 1 mol of electron

1 mol of electron = 96485 C

So,1 mol of Ag requires 96485 C

let us calculate mol of element deposited:

we have below equation to be used:

number of mol, n = mass/molar mass

= 0.277/107.9

= 0.00257 mol

total charge = mol of element deposited * charge required for 1 mol

= 0.00257*96485

= 247.6955 C

we have below equation to be used:

time = Q/i

= 247.6955/0.655

= 378 s

Answer: 378 s

2)

the electrolysis expression is:

Ag1+ + 1e- ------> Ag

1 mol of Ag requires 1 mol of electron

1 mol of electron = 96485 C

So,1 mol of Ag requires 96485 C

let us calculate mol of element deposited:

we have below equation to be used:

number of mol, n = mass/molar mass

= 0.223/107.9

= 0.00207 mol

total charge = mol of element deposited * charge required for 1 mol

= 0.00207*96485

= 199.4083 C

we have below equation to be used:

time = Q/i

= 199.4083/0.856

= 233 s

Answer:233 s