Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 2 5°C.(The equation is balanced.)
$\quad$ $\quad$ Pb(s) + Br₂(l) → Pb²⁺(aq) + 2 Br⁻(aq)
Pb²⁺(aq) + 2 e^- → Pb(s) $\quad$ $\quad$ E° = -0.13 V
Br₂(l) + 2 e^- → 2 Br^- (aq) $\quad$ $\quad$ E° = +1.07 V

Question

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 2 5°C.(The equation is balanced.)

\quad

\quad

Pb(s) + Br₂(l) → Pb²⁺(aq) + 2 Br⁻(aq)
Pb²⁺(aq) + 2 e^- → Pb(s)

\quad

\quad

E° = -0.13 V
Br₂(l) + 2 e^- → 2 Br^- (aq)

\quad

\quad

E° = +1.07 V

Quizplus · Accepted Answer

To calculate the standard cell potential, we need to subtract the reduction potential of the anode (Pb) from the reduction potential of the cathode (Br-). We can see from the given half-cell reactions that the reduction potential of the anode is -0.13 V and the reduction potential of the cathode is +1.07 V. Therefore, the standard cell potential is:

E°cell = E°cathode - E°anode
E°cell = (+1.07 V) - (-0.13 V)
E°cell = +1.20 V

Therefore, the best choice is A) +1.20 V.

Use the Standard Half-Cell Potentials Listed Below to Calculate the Standard