A concentration cell similar to the one shown is composed of two Mn electrodes and solutions of different Mn2+concentrations. The left compartment contains 1.38 M Mn2+ , and the right compartment contains 1.31 M Mn2+ . Calculate the cell potential for this reaction at 298 K.

In a cell with an aluminum electrode in a solution of aluminum nitrate and a zinc electrode in a solution of zinc nitrate:  Al|Al3+ || Zn2+|Zn.  If you increase the concentration of Zn2+, which of the following is true about the cell potential?

A particular voltaic cell operates on the reaction Zn(s) + Cl, (9) → Zn+ (aq) + 2C1 (aq) giving a cell potential of 0.763 V. Calculate the maximum electrical work generated when 17.0 g of zinc metal is consumed. Maximum electrical work-

A galvanic cell whose cell reaction is 2Fe3+(aq) + Zn(s) → 2Fe2+(aq) + Zn2+(aq) has acell potential of 0.72V. What is the maximum electrical work that can be obtained fromthis cell per mole of iron(III) ion?

The anode compartment of a galvanic cell consists of a Zn anode immersed in 0.05M ZnCl2 The cathode compartment consists of a Cu cathode immersed in an 0.10M CuCl2 solution. Using the cell potentials found on page 815 of your textbook, calculate the cell potential for this reaction. Assume T = 298K.

You make a voltaic cell with copper and aluminum. If the cell potential is measured to be +2.50 V at room temperature, then what is the reaction quotient?

Calculate the cell potential of a cell composed of a cathode consisting of a Co wire immersed in a 1.44 M Co²+ solution and an anode consisting of a Co wire immersed in a 5.60×10-5 M Co²+ solution. Assume the temperature of the solutions is 298 K. Cell potential: V

Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions. Identify the reactions with K > 1 among the following redox reactions. Write the line representations for the Galvanic cells, indicating the anode and 1. cathode. a. Cl2 + Br → Ct + Br2 b. Mnoa + H* + Ce → Cet + Mn2 + H20

+ The Nernst Equation The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation i E=E 2.303 RT log10 Q where E is the potential in volts, Eo is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, 12 is the number of moles of electrons transferred, Fis the Faraday constant, and is the reaction quotient. Using the common reference temperature, 25 °C or 298 K, the equation has the form E = ED (0.0592) log Q The reaction quotient has the usual form Q [products [reactants A table of standard reduction potentials gives the voltage at standard conditions, 1.00 M for all solutions and 1.00 atm for all gases. The Nernst equation allows for the calculation of the cell potential E at other conditions of concentration and pressure. Part A For the reaction 2Co²+ (aq) + 2Cl(aq) +2Co²+ (aq) + Ch₂(g). E 0.483 V what is the cell potential at 25°C if the…