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I Learning Goal: To learn how to use the Nernst equation. The standard reduction potentials listed in any reference table are only valid at the common reference temperature of 25 °C and standard conditions of 1 M for solutions and 1 atm for gases. To calculate the cell potential at nonstandard conditions, one uses the Nernst equation, E=Eº – 2.303 RT Elogio a nF where E is the potential in volts, Eº is the standard potential at 25°C 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/(mole") is the Faraday constant, and Q is the reaction quotient. At the common reference temperture of 298 K substituting each constant into the equation the result is E=E° 2 Vlog10 @ 0.0592 V Part A What is the value for the reaction quotient for the call Express your answer numerically View Available Hints) ΡΑ ΑΣΦ English (United States) IN @ 15 A
Part B What is the value for the temperature, Tin kelvins ? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) DO HÅ ? T= Value Units Part What is the value for n? Express your answer as an integer and include the appropriate units (i.e. enter mol for moles). View Available Hint(s) ? HA n = Value Units Focus (United States) MA E
Part D o Calculate the standard cell potential at 25°C for Mg(s) + Fe2+ (aq) →Mg2+ (aq) + Fe(s) Express your answer to three significant figures and include the appropriate units. View Available Hint(s) НА 1 ? Eº = Value Units IE