8. Z(s) KNO3(aq) salt bridge V 1.0 MZ(NO3)₂ (aq) Half-Reaction X²+ (aq) + 2e → X(s) Z² (aq) + 2 e → Z(s) X(s) 1.0 MX(NO3)₂(aq) Standard Reduction Potential (V) -1.25 V 0.45 V Consider the voltaic cell, half-reactions, and standard reduction potentials shown above. Which reaction occurs at the anode?

Calculate the standard cell potential, ?∘cellEcell°, for the reaction shown. Use these standard reduction potentials.   Cu(s)+Ag+(aq)⟶Cu+(aq)+Ag(s)

4. A cell uses the following reaction: a. Zn (s) + 2 H* (aq) → Zn²* (aq) + H2 (g) (a) Determine the emf of the cell under standard conditions. (b) When PH,=1.0 atm and [Zn²*] = 1.0 M, the cell potential is 0.560 V. Determine the concentration of H* in the cathode compartment. Zn2“(aq) + 2e¯ → Zn(s) -0.763 2H*(aq) + 2e¯ –→ H2(g) b.

What will be the products of the electrolysis of an 1-M aqueous aluminum chloride (AICI3) solution at 25 °C? (The electrodes themselves are platinum.) (Use the standard electrode potentials table in your online textbook's Appendix to help you answer the question.) No products will be produced. H₂(8) +20H (aq) + Cl₂(g) 4Al(s) + 30₂(g) + 12H*(aq) O 2H₂(g) + 4H₂O(l) + O₂(g) O2Al(s) + 3Cl2(g)

. Consider the oxidation-reduction reaction Mg (s) + Cu2+ (aq) → Mg2+ (aq) + Cu (s)           Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?

Consider the following reduction potentials. Ag*(aq) + e → Ag(s) E° = + 0.80 V Sn2*(aq) + 2 e -→Sn(s) E° = - 0.14 V Mg2 (aq) + 2 e - → Mg(s) E° = - 2.37 V a.) Calculate the cell potential at standard conditions (E°cell) for a voltaic cell of Mg2+/Mg and Ag*/Ag, in Volts. E° cell = v b.) Calculate Ecel in V at 298 K if [Mg2*] = 0.100 M and [Ag*] = 0.100 M. %3D Ecell = V

O ELECTROCHEMISTRY = Understanding concentration cells ODDOD 3/5 A certain metal M forms a soluble nitrate salt MNO3. Suppose the left half cell of a galvanic cell apparatus is filled with a 1.50 M solution of MNO3 and the right half cell with a 150. mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 30.0 °C. Which electrode will be positive? Oleft right ? What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.

Gibbs free energy= -434250 J/mol for a galvanic cell whose two half-reactions: Mt3+ (aq) + 3 e1- → Mt (s), and R2+ (aq) + 2 e1- → R (s), have standard reduction potentials of 1.09 V and 0.34 V respectively