For the following half-reactions, answer the following questions below Co³*(aq) + e¯ –→ Co²*(aq) E° = +1.953 V Fe+(aq) + e¯ – Fe2+(aq) E° = +0.769 V I2(aq) + 2e¯· 21-(aq) E° = +0.534 V Pb²*(aq) + 2e¯ – Pb(s) E° = -0.127 V Cd²*(aq) + 2e¯· Cd(s) E° = -0.402 V Mn²+(aq) + 2e- · Mn(s) E° = -1.182 V a. Which is the weakest reducing agent? b. Which is the strongest reducing agent? c. Which is the strongest oxidizing agent?

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

A galvanic cell was constructed with a nickel electrode that was dipped into 1.1 M NiSO4 solution and a chromium electrode that was immersed into a solution containing Cr3+ at an unknown concentration. The potential of the cell was measured to be 0.557 V, with the chromium serving as the anode. The standard cell potential for this system was determined to be 0.487 V. What was the concentration of Cr3+ in the solution of unknown concentration?

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Explain the feasibility of the design of the galvanic cell in terms of a) standard cell potential generated and b) cost-effectiveness.

Use the following description of a galvanic cell to answer questions 4-7. One half-cell is prepared with a tin electrode submerged in 1.0 M Sn(NO,), and the other half-cell consists of a chromium electrode submerged in 1.o M Cr(NO), at standard temperature.

A cell consisting of two silver plates dipping in a 0.1 M and 0.01 M solution of silver nitrate AgNO3 respectively at 25 °C. 1- diagram the cell, 2- write the cell reaction 3- Calculate the cell potential

What mass of rhodium (Rh) metal will be deposited from a solution of Rh3+ ions by running electrical current through the solution at 0.500 A for 120.0 minutes?

+ 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…