(1) () H) Define the terms voltaic and electrolytic cells Explaining your reasons, identify the sign of the free energy change for voltaic and electrolytic cells. Discuss the nature of the half-reaction at the anode for voltaic and electrolytic cells. Consider the potentials for the following cells: Cu(s) Cu (aq) + 2 e Ag (aq) e Ag(s) Zn+ (aq) + 2e Zn (s) Q 4(b) Determine the equilibrium constant for the following reaction: E-0.340 V E = +0.800 V E = -0.760 V [40 Marks] Cu(s)+2 AgNO (aq) + Cu(NO): (aq) + 2 Ag (s) and describe what will occur within the cell as the reaction proceeds. Determine the number of Faradays of electricity passed when 150.5 g of copper metal are consumed. Q4(c) [END OF EXAM] [30 Marks] Determine the voltage of the following cell that may not be in standard notation: Zn(s)/Zn(aq, 0.001 M) // Zn(aq. 1.0 M)/2n (s) describe what will occur within the cell and, explaining your reasons, state whether it is a voltaic or electrolytic cell. [End of Question 4]