[r-soy]

Hi all

Q1 : when a run down battery is recharged 22600C of charge is required comput the time in hour needed to recharge the battery to 8A current ?

my answer is : t = Q / I = 22600 / 8 = 2825

Q2 : calculate the number of Faraday required depositing 1 X 10^-5moles of cu from cu^2 ?

my answer is
Cu ----- > cu^2+

the charge of cu = 3
the number of Faraday needed to deposit 1 mole will be = 3F
the number of Faraday needed to deposit 1 X 10^-5 mole will be = 3F X  1 X 10^-5
= 3 X 10^-5 F

I want check my solving

thanks

[MrTeo]

The first answer seems OK but I don't really understand the second one: first of all the reducing reaction isn't Cu→Cu²⁺, but the inverse one (even if this doesn't change your answer, it's pretty important to write clearly and correctly the reactions). And why does Cu have a charge of 3?

Just a note, try to use superscripts and subscripts next time, to make the text more readable, thanks  

[sjb]

Hi all

Q1 : when a run down battery is recharged 22600C of charge is required comput the time in hour needed to recharge the battery to 8A current ?

my answer is : t = Q / I = 22600 / 8 = 2825

What are your units?