Asked by Loon
How long would it take in minutes to plate 1.00 gram of silver to a watch when 9.2 amps are passed through a silver (I) chloride solution? (atomic mass of silver is 107.8682 g/mol).
Answers
Answered by
DrBob222
I don't know why anyone would use AgCl instead of AgNO3 but that's not here nor there.
Coulombs = amperes x seconds
C = 9.2 A x seconds. So we need to fill in C and seconds.
We know that 96,485 C wil deposit 107.8682 grams of Ag. We want 1 g to be deposited; that will take how many C? That's
96,485 C x (1.0000 g/107.8682) = ? C
Substitute that value for C in
C = 9.2 x seconds and solve for seconds, then convert to min.
One note: the value of 9.2 give you two significant figures so all of those digits for the atomic mass of Ag aren't necessary. Post your work if you get stuck.
Coulombs = amperes x seconds
C = 9.2 A x seconds. So we need to fill in C and seconds.
We know that 96,485 C wil deposit 107.8682 grams of Ag. We want 1 g to be deposited; that will take how many C? That's
96,485 C x (1.0000 g/107.8682) = ? C
Substitute that value for C in
C = 9.2 x seconds and solve for seconds, then convert to min.
One note: the value of 9.2 give you two significant figures so all of those digits for the atomic mass of Ag aren't necessary. Post your work if you get stuck.
Answered by
Loon
Okay, so I did that and I got 97.225 secs or 1.62 minutes
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