QUESTION 6 A voltaic cell is prepared using copper and silver. Its cell notation is shown below. Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s) Which of the following processes occurs at the cathode? Cu(s) → Cu2+(aq) + 2e¯ Cu2+(aq) + A) B) +2e → → Cu(s) C) Ag(s) Ag+(aq) + e¯ D) Ag+(aq) + e Ag(s) E) Cu(s) + 2Ag+(aq) → Cu²+(aq) + 2Ag(s) →

Consider a cell based on the following half-reactions: a. Draw this cell under standard conditions, labeling the anode, the cathode, the direction of electron flow, and the concentrations, as appropriate. b. When enough NaCl(s) is added to the compartment containing gold to make the [Cl] = 0.10 M, the cell potential is observed to be 0.31 V. Assume that Au3+ is reduced and assume that the reaction in the compartment containing gold is Au3+(aq)+4Cl(aq)AuCl4(aq) Calculate the value of K for this reaction at 25C.

A voltaic cell is constructed using the reaction of chromium metal and iron(II) ions. 2 Cr(s) + 3 Fe2+(aq) 2 Cr3+(aq) + 3 Fe(s) Complete the following sentences: Electrons in the external circuit flow from the ________ electrode to the ______ electrode. Negative ions move in the salt bridge from the ________ half-cell to the ______ half-cell. The half-reaction at the anode is _______ and that at the cathode is ________.

A voltaic cell is constructed in which one half-cell consists of a silver wire in an aqueous solution of AgNO3.The other half cell consists of an inert platinum wire in an aqueous solution containing Fe2+(aq) and Fe3+(aq). (a) Calculate the cell potential, assuming standard conditions. (b) Write the net ionic equation for the reaction occurring in the cell. (c) Which electrode is the anode and which is the cathode? (d) If [Ag+] is 0.10 M, and [Fe2+] and [Fe3+] are both 1.0 M, what is the cell potential? Is the net cell reaction still that used in part (a)? If not, what is the net reaction under the new conditions?