Reference no: EM13332436

Introduction to the Nernst Equation Learning Goal: To learn how to use the Nernst equation. The standard reduction potentials listed in any reference table are only valid at standard-state conditions of 25 circ C and 1 M. To calculate the cell potential at non-standard-state conditions, one uses the Nernst equation, E = E^\circ - \frac{2.303\,RT}{ nF}\log Q where E is the potential in volts, E^\circ is the standard potential in volts, R = 8.314 J/(K * mol) is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F= 96,500 C (mol ~e^-) is the Faraday constant, and Q is the reaction quotient. Consider the reaction Mg (s)+ Fe^2+(aq) \rightarrow Mg^2+(aq)+ Fe (s) at 83\;^\circ C , where [ Fe^2+]= 3.60 M and [ Mg 2+]= 0.310M . Part A What is the value for the reaction quotient, Q, for the cell?