Asked by MIRACLE IWUNZE

calculate the mass of silver deposited when a current of 2.6a is passed through a solution of a silver salt for 70mins ag=108,1 faraday 96500
Answered by DrBob222
Convert 70 min to seconds.
coulombs = C = Amps x seconds. C = approx 1E4 C but you need to do it more accurately than that.
Then 96,500 C will deposit 108.1 g (are you sure about the atomic mass Ag???. More like 107.9 I thought). So
108.1 x (1E4/96,500) = ? g Ag deposited.
Answered by Akinmutimi blessing
12.22
Answered by Friday Israel
calculate the Mass of silver deposited when a current of 2.6A is passed through a solution of a silver salt for 70 minutes (Ag =108 1 Faraday=96500)
Answered by Kayode
calculate the mass of silver deposited when a current of 2.6A is passed through solution of a silver salt for 70 minutes(Ag=108,IF=96500 c)
Answered by Anonymous
in this question Q=it. i=2.6A t=70min. Q=2.6*70*60=10920C
108g yield 96500F
Xg will yield 10920C
cross multiply you will have
10920*108/96500=12.22g
Answered by Judge Aboki
Calculated the mass of silver deposited when a current of 2.6A is passed through a solution of a silver for 70minutes (Ag=108;1 Faraday=96500c)

Answered by Peter
How will you calculate it after changing the minutes to second and finding your Coulombs which is current × time
Answered by Ponlir
You will cross multiply
Answered by Victor
M=Q * m.m / f * c
M=10920 * 108 / 96500 * 1
M= 12.22g
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