Part A earning Goal: o learn how to use the Nernst equation What is the value fo
ID: 1045286 • Letter: P
Question
Part A earning Goal: o learn how to use the Nernst equation What is the value for the reaction quotient, Q, for the cell? Express your answer numerically. View Available Hint(s) he standard reduction potentials listed in any eference table are only valid at standard-state onditions of 25 C and 1 M To calculate the cell otential at non-standard-state conditions, one ses the Nernst equation 2303 RT logo Q n F where E is the potential in volts, E" is the standard potential in volts R = 8314 J/(K-mol) is the gas constant, Tis the temperature in kelvins, n is the number of moles of electrons transferred F96,500 C/(mol e ) is the Faraday constant, and Q is the reaction quotient Submit Previous Answers X Incorrect: Try Again: 3 attempts remaining Substituting each constant into the equation the result is EE002 y log,pQ Y Part EBExplanation / Answer
A.
Q = [Mg2+] / [Fe2+]
Substitute the given concentrations of Mg2+ and Fe2+ to get Q value.
If [Mg2+] =0.310 M and [Fe2+] = 3.20 M at standard condition
Q = 0.310 / 3.20
Q = 0.0969
B.
To convert the degree celcius to kelvin add 273.15
T = 273.15 + 0C
T = 273.15 + 41
T = 314.15 K
C.
n = number of electrons transferred = 2
D.
E0Mg2+/Mg = - 2.38 V
E0Fe2+/Fe = - 0.41 V
E0cell = E0Fe2+/Fe - E0Mg2+/Mg = - 0.41 - ( - 2.38 ) = + 1.97 V