He cell potential of a redox reaction occurring in an electrochemical cell under any set of temperature and concentration conditions can be determined from the standard cell potential of the cell using the nernst equation e = e° − rt nf ln q where e is the cell potential of the cell, e° is the standard cell potential of the cell, r is the gas constant, t is the temperature in kelvin, n is the moles of electrons transferred in the reaction, and q is the reaction quotient. use this relationship to answer the problem below. for the following oxidation-reduction reaction 2 al3+(aq) + 3 cu(s) → 2 al(s) + 3 cu2+(aq) the standard cell potential is −2.00 v. what is the actual cell potential of the cell if the temperature is 320 k, the initial al3+ concentration is 0.00114 m, and the initial cu2+ concentration is 0.0291 m? (note that the reaction involves the transfer of 6 moles of electrons, and the reaction quotient is 19.0.) v