A galvanic (voltaic) cell is made using the 2 half cells: Zn2+ (aq) + 2e → Zn(s) E =-.763 V Mg2+ (aq) + 2e - → Mg(s) with Zn(s) and Mg(s) as the electrodes. Answer the questions A. It is the anode. [Select ] B. It is the cathode. [Select] C. Electrons in the wire flow toward it. [Select]. D. Anions from the salt bridge flow toward it. [Select] E. Gains mass. [Select] E = -2.37 V F. Losses mass. [Select]

The diagram below is an electrochemical cell based on a redox reaction that needs to be completed by a student in the laboratory. Zn(s) + Br₂(1)→ Zn²+ (aq) + 2 Br¯(aq) C electron flow? B A H G Salt Bridge Zn E F D Which of the following is true for the cell? O a. The cathode is A, the anode is B and the electrons travel from left to right O b. The cathode is A, the anode is B, however there is no current Oc. The cathode is A, the anode is B and the electrons travel from left to right O d. The anode is A, the cathode is B and the electrons travel from left to right O e. The anode is A, the cathode is B and the electrons travel from right to left

3. Consider the HCN-KCN buffer system, which species would react if a dilute aqueous HBr solution were added to the buffer? O CN O CN O HCN O KCN

11