nt 16 (Chapter 18) Mozila Firefox ViewlassignmentProblemiD 956350328koffsets pre

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nt 16 (Chapter 18) Mozila Firefox ViewlassignmentProblemiD 956350328koffsets prev https//session masteringchemistry. Assignment 16 (Chapter 18) Introduction to the Nernst Equation Consider the reaction Mg(s) + Fe2+ (aq) Mg2+ (aq) + Fe(s) 0.110 M ConstantsPeriodic Table at 41-c , where Fe, 1-2 90 Mand [Mg2+] Learning Goal: To lean howr to use the Nenst equation Part A The standard reduction potentials listed in any reference table are orly valid at standard-state conditions of 25 C and 1 M. To calculate the cell potential at non-standard-state conditions, one uses the Nenst equation, What is the value for the reaction quotient, Q for the cell? Express your answer numerically. View Available Hint(s) 2.303 RT where E is the potential in vots, B is the standard potental in volts R=8.314J/(K-mo) rs the gas constant, T is the temperature in kelins, n is the number of moles of electrons transfered F = 96,500 C/(mol e ) is the Faraday constant, and Q is the reaction quotient Substituting each constant into the equation the result is Submit x Incorrect; Try Again; 5 attempts remaining Part B What is the value for the temperature, T, in kevins? Express your answer to three significant figures and include the approp units. View Available Hints) T- Value Units Submit Incorrect; Try Again: 4 attempts remaining

Explanation / Answer

Part A:

Value of reaction quotient, Q = [Mg2+]/ [Fe2+]

= [0.110]/ [2.90]

= 0.0379

Part B:

Value of temperature T in Kelvins = 41 + 273 = 314 Kelvin

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