QUESTION 11 The more negative the EO value for a given reaction, the greater the tendency for the reaction to occur as written. O True O False QUESTION 12 The Nernst equation is used to calculate electrode potentials of Galvanic cells at concentrations other than 1 M O True O False

A1.0-L sample of 1.0 M HCI solution has a 13.5 A current applied for 41 minutes. What is the pH of the solution after the electricity has been turned off?

A current of 5.55 A is passed through a Cu(NO3)₂ solution for 1.90 h. How much copper is plated out of the solution? mass of copper: g

Consider the following standard reduction potentials in acid solution:                                E°(V) Al⁺³ + 3e− → Al(s) −1.66 Ag⁺¹ + e− → Ag(s) +0.80 Sn⁺⁴ + 2e− → Sn⁺² +0.14 Fe⁺³ + e− → Fe⁺² +0.77   The strongest reducing agent among those shown above is A) Al⁰ B) Fe⁺³ C) Br⁻ D) Al⁺³

Calculate Ecel (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.793 M and the concentration of the ion at the cathode is 1.90 M. Use the standard reduction potentials from Appendix L in our textbook. Np + Lu³* » Lu + Np3*

A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. E° V 'cell * TOOLS х10

Cell Potential For a given galvanic cell, the standard cell potential can be calculated by subtracting the standard half-cell potential of the reaction that occurs at the cathode from the standard half-cell potential of the reaction that occurs at the anode: Ecell Ered (cathode) - Ed (anode) ▼ Tarnish on copper is the compound CuO. A tarnished copper plate i placed in an aluminum pan of boiling water. When enough salt is added so that the solution conducts electricity, the tarnish disappears. Imagine that the two halves of this redox reaction were separated and connected with a wire and a salt bridge. Part A Calculate the standard cell potential given the following standard reduction potentials: A²+ +3e Cu²+ + 20 Express your answer to two decimal places and include the appropriate units. ▸ View Available Hint(s) Ecell = li Value 4 → Units ? Al; E Cu; E 19 of 42 -1.66 V 0.340 V Review | Constants | Periodic Table

below. questions 8 for the electrolysis of molten lead(II) chloride (PbCl₂) as seen in the diagram Anode + Voltage source Porous screen Molten PbCl₂ e Cathode

A certain metal M forms a soluble sulfate salt M₂SO4. Suppose the left half cell of a galvanic cell apparatus is filled with a 3.00 M solution of M₂SO4 and the right half cell with a 30.0 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 35.0 °C. Which electrode will be positive? 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. left right x10 X Ś

The electrode potential for the following two half reactions are as follows: Al+3 + 3 e- = Al(s) E = (-)1.66 V  Fe+2 + 2e- = Fe(s) E = (-) 0.44 V. An electrochemical cell has an Al anode immersed in aluminum sulfate solution and a Fe cathode immersed in an iron (II) sulfate solution. The voltage generated by this cell would be:  a) -2.10 V   b)  + 2.10 V  c)  -1.22 V  d)  + 1.22 V The number of electrons transferred in the reaction A) 2 b)  3  C0  5  d)  6