Question

In a galvanic cell, one half-cell consists of a lead strip dipped into a 1.00 M solution of Pb(NO₃)₂. In the second half-cell, solid uranium is in contact with a 1.00 M solution of U(NO₃)₃. Pb is observed to plate out as the galvanic cell operates, and the initial cell voltage is measured to be 1.672 V at 25°C.


(a) Write balanced equations for the half-reactions at the anode and the cathode. Show electrons as e^-. Use the smallest integer coefficients possible and indicate states.

Half-reaction at anode (do not multiply by factor):

Half-reaction at cathode (do not multiply by factor):

(b) Calculate the standard reduction potential of a U³⁺|U half-cell. The standard reduction potential of the Pb²⁺|Pb electrode is -0.126 V.

______________V

Answer 1

- Ans . It is given that Pb is observed to plate out, which - means Pb will get Onidised 2 Andde half Cell Reaction - PBL) — Methan the (Ouidation) Cathodic half cell Reaction or y té — Voy (Reduction) Balanced Overall Chemical Equation 3Pb(s) + 2 U2 - 31% tap) +20 (6) 999 Cell Voltage = 1.672 v = Full Elan: E cathede - E made El & B - E PRE 1.672 - E3% - (-0.126) 1.672 – 0.126 = EU3t/u E02% 1.546V