metal rod of Pn, 200 mL of Pn(NO3)3 0.5 M solution. 1 metal rod of Ri, 200 mL of Ri(NO3)2 0.4 solution. KNO3 salt bridge. Pn3+ (aq) + 3e- --> Pn(s) Eo=-0.51 Ri2+(aq) + 2e- --> Ri(s) Eo= -0.59 Copy the template provided and draw the Galvanic Cell indicated as explained at the beginning of this problem. Label the cathode Label the anode Label the direction of the movement of electrons Label the direction of the movement of ions from the salt bridge Do not forget to draw the solution. Calculate the standard reduction potential. Calculate the voltage of the cell at 298 K. Write the shorthand notation for your constructed cell. Write the overall balanced redox reaction happening on this cell

1 metal rod of Pn, 200 mL of Pn(NO3)3 0.5 M solution. 1 metal rod of Ri, 200 mL of Ri(NO3)2 0.4 solution. KNO3 salt bridge.

Pn³⁺ (aq) + 3e^- --> Pn(s)   E^o=-0.51

Ri²⁺(aq) + 2e^- --> Ri(s)       E^o= -0.59

1. Copy the template provided and draw the Galvanic Cell indicated as explained at the beginning of this problem.
   1. Label the cathode
   2. Label the anode
   3. Label the direction of the movement of electrons
   4. Label the direction of the movement of ions from the salt bridge
   5. Do not forget to draw the solution.
2. Calculate the standard reduction potential.
3. Calculate the voltage of the cell at 298 K.
4. Write the shorthand notation for your constructed cell.
5. Write the overall balanced redox reaction happening on this cell