, crit810CH12 So5dX Olis1O-Chapter 17 × CHI810-Chapter17 × Gilbert 4thCH1957 m/c

Question

, crit810CH12 So5dX Olis1O-Chapter 17 × CHI810-Chapter17 × Gilbert 4thCH1957 m/courses/wp-content/uploads/2017/11/CH1810-Pr-Ex-3-Fa2017-copy pdf c prof katz cnm + Automat Pb2+(aq) + Cu(s) Pb(s) + Cu2+(aq) 2. Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C Sn(s) I Sn2+(aq, 0.022 M) Il Agt(aq, 2.7 M) 1 Ag(s) 3. What mass of aluminum can be plated onto an object in 755 minutes at 5.80 A of current? 4. Aluminum crystallizes in a face centered cubic structure with an edge length of 2/2 r

Explanation / Answer

2) Nernest equation,

cell reaction = Sn(s) + 2Ag^+(aq) ----> Sn^2+(aq) + 2Ag(s)

Ecell = E0cell - 0.0591/nlog[Sn^2+]/[Ag^+]^2

E0cell = E0cathode - E0anode

        = 0.8 - (-0.13)

        = 0.93 v

Ecell = 0.93 - (0.0591/2)log(0.022/2.7^2)

        = 1 V

3)

faradays first law

equivalent weight of Al (Ewt)= atwt / charge = 27/3 = 9 g/equiv

W = Zit

Z= E/F

w = E/Fit

F = faraday = 96500 C

i = current = 5.8 A

t = time = 755 min = 755*60 = 45300 sec

w = weight of Al deposited = (9/96500)*5.8*45300 = 24.5 g

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