Part A Silver can be plated out of a solution containing...

Part A Silver can be plated out of a solution containing Ag$^+$ according to the half-reaction Ag$^+$ (aq) + e$^-$ $\rightarrow$ Ag(s) How much time (in minutes) does it take to plate 12 g of silver using a current of 2.3 A? Express the time to two significant figures and include the appropriate units. t = 6.0 \cdot 10$^1$ min Incorrect; Try Again; 9 attempts remaining

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00:01 Silver can be plated out of a solution containing silver hyr and ag plus.

00:07 Okay.

00:09 According to the r -reaction, akers plus e minus to produce silver solid.

00:19 So this is the platin reaction.

00:22 The question says how much time in minutes does it take to plates 12 grams of silver? number, this is the mass, and the current, which is i, is 4 .9 hamper.

00:40 Okay, so we are looking for time here.

00:51 Okay, so from this equation, first thing we have to do is to convert this 12 gram to number of moles.

01:00 So number of mole, we know is mass divided by the molar mass.

01:05 And silver, if i'm correct, the atomic mass of that is 1 .08.

01:15 Yeah, 08.

01:22 So therefore, number of mole will be 12 grams, divided by 1 .0 .8 grams for more.

01:30 And that will be 12, however, 108.

01:35 So that will be 0 .111 .1.

01:40 1 mole.

01:44 So, from this equation up here, we know 1 mole of silver requires 1 more of electron, right? 1 more of silver higher requires 1 more of electron who produce 1 more of silver solid.

02:03 Okay.

02:06 So, we can say to produce 1 more of silver solid, we're going to need 1 more of electron.

02:20 So one more of electron will produce one more of a g solid, right? therefore, 0 .111 more of silver solid, we need 0 .111 .1...

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