Chapter 19, Problem 19.159MP

Consider a galvanic cell that utilizes the following half reactions:
Anode: $Zn(s)+H_{2}O(l)\to ZnO(s)+2H^{+}(aq)+2e^{-}$
Cathodae: $A{g}^{+}(aq)+e^{-}\to Ag(s)$
(a) Write a balanced equation for the cell reaction, and use the thermodynamic data in Appendix B to calculate the values of $\Delta H^o,$
$\Delta S^o,$ and $\Delta G^o$ for the reaction.
(b) What are the values of P and the equilibrium constant K for the cell reaction at 25 °C?
(c) What happens to the cell voltage if aqueous ammonia is added to the cathode compartment? Calculate the cell voltage assuming that the solution in the cathode cornpartment was prepared by mixing 50.0 mL of 0.100 s1 AgNO₃ and 50.0 mL of 4.00 M NH₃.
(d) Will AgCI precipitate if 10.0 ml. of 0.200 M NaCI is added to the solution in part (c)? Will AgBr precipitate if 10.0 ml. of 0.200 M KBr is added to the resulting solution?