Question

4. Consider the electrochemical cell described below: Zn(s)|Zn$^{2+}$(aq)||Cu$^{2+}$(aq)|Cu(s) a. Sketch a picture of the cell. Label the anode, cathode, and salt bridge. b. Indicate the direction that electrons travel through the circuit in the diagram you drew for part a. c. Indicate the direction that the positive and negative ions flow in the salt bridge in the diagram you drew for part a. d. Write the equation for the half reaction that occurs at the anode. e. Write the equation for the half reaction that occurs at the cathode. f. Which species is oxidized? g. Which species is reduced? h. How will the mass of the electrodes change as the electrochemical cell operates? 5. Calculate $\Delta G^\circ$ and K for the reaction described below at 298 K. Is the reaction spontaneous? Mg(s)|Mg$^{2+}$(aq)||Pb$^{2+}$(aq)|Pb(s) Pb$^{2+}$(aq) +2e$^-$ $\rightarrow$Pb(s) Mg$^{2+}$(aq) +2e$^-$ $\rightarrow$Mg(s) E$^\circ$=-0.1262 V E$^\circ$=-2.372 V

          4. Consider the electrochemical cell described below:
Zn(s)|Zn$^{2+}$(aq)||Cu$^{2+}$(aq)|Cu(s)
a. Sketch a picture of the cell. Label the anode, cathode, and salt bridge.
b. Indicate the direction that electrons travel through the circuit in the diagram you drew for part a.
c. Indicate the direction that the positive and negative ions flow in the salt bridge in the diagram you
drew for part a.
d. Write the equation for the half reaction that occurs at the anode.
e. Write the equation for the half reaction that occurs at the cathode.
f. Which species is oxidized?
g. Which species is reduced?
h. How will the mass of the electrodes change as the electrochemical cell operates?
5. Calculate $\Delta G^\circ$ and K for the reaction described below at 298 K. Is the reaction spontaneous?
Mg(s)|Mg$^{2+}$(aq)||Pb$^{2+}$(aq)|Pb(s)
Pb$^{2+}$(aq) +2e$^-$ $\rightarrow$Pb(s)
Mg$^{2+}$(aq) +2e$^-$ $\rightarrow$Mg(s)
E$^\circ$=-0.1262 V
E$^\circ$=-2.372 V

4. Consider the electrochemical cell described below:
Zn(s)|Zn^2+(aq)||Cu^2+(aq)|Cu(s)
a. Sketch a picture of the cell. Label the anode, cathode, and salt bridge.
b. Indicate the direction that electrons travel through the circuit in the diagram you drew for part a.
c. Indicate the direction that the positive and negative ions flow in the salt bridge in the diagram you
drew for part a.
d. Write the equation for the half reaction that occurs at the anode.
e. Write the equation for the half reaction that occurs at the cathode.
f. Which species is oxidized?
g. Which species is reduced?
h. How will the mass of the electrodes change as the electrochemical cell operates?
5. Calculate Δ G^∘ and K for the reaction described below at 298 K. Is the reaction spontaneous?
Mg(s)|Mg^2+(aq)||Pb^2+(aq)|Pb(s)
Pb^2+(aq) +2e^- →Pb(s)
Mg^2+(aq) +2e^- →Mg(s)
E^∘=-0.1262 V
E^∘=-2.372 V

Added by Michael G.

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