Question

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 ∘C and 1 M . To calculate the cell potential at non-standard-state conditions, one uses the Nernst equation, E=E∘−2.303RTnFlog10Q where E is the potential in volts, E∘ is the standard potential in volts, R=8.314J/(K⋅mol) is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F=96,500C/(mol e−) is the Faraday constant, and Q is the reaction quotient. Substituting each constant into the equation the result is E=E∘−0.0592 Vnlog10Q Figure of 0

Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 85 ∘C , where [Fe2+]= 3.50 M and [Mg2+]= 0.310 M . Part A Part complete What is the value for the reaction quotient, Q , for the cell? Express your answer numerically. View Available Hint(s) -- SubmitPrevious AnswersRequest Answer Correct Part B Part complete What is the value for the temperature, T , in kelvins? Express your answer to three significant figures and include the appropriate units. View Available Hint(s) -- Q = 8.86×10−2 SubmitPrevious AnswersRequest Answer Incorrect; Try Again; 6 attempts remaining Part C Part complete 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) -- T T T = 317 Value K Units SubmitPrevious AnswersRequest Answer Part D Part complete Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) Express your answer to three significant figures and include the appropriate units. n n n = nothing Value nothing Units

Answer 1