What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 3.59×10-4 M and the Cr3+ concentration is 1.07 M ? 3Hg2+(aq) + 2Cr(s) →3Hg(l) + 2Cr3+(aq) Answer:  ____ V The cell reaction as written above is spontaneous for the concentrations given: _______ (true or false)

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What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Hg2+ concentration is 3.59×10-4 M and the Cr3+ concentration is 1.07 M ?

3Hg2+(aq) + 2Cr(s) →3Hg(l) + 2Cr3+(aq)

Answer:  ____ V

The cell reaction as written above is spontaneous for the concentrations given: _______ (true or false)
 
The Nernst Equation
A non-standard cell or half-cell potential can be calculated using the Nernst Equation:
RT
E = E° - .
In Q
nF
where
E = potential under non-standard conditions
standard potential
= ideal gas constant
T = kelvin temperature
n = number of moles of electrons for the reaction as written
F = charge carried by 1 mol of electrons
Q = reaction quotient
E°
R
It is customary to use the equation in a form where numerical values are substituted for R, T and F at a temperature of 25 °C.
For
R = 8.314 J mol'K!
T = 298.15 K
96,485 J V-l mol"
F =
(8.314 J mol! K(298.15 K)
RT
= 0.0257 V
F
96,485 J V-' mol-1
and the Nernst equation with the potentials in volts is:
Previous
0.0257
In 0
Hatural lagarithn.
Transcribed Image Text:The Nernst Equation A non-standard cell or half-cell potential can be calculated using the Nernst Equation: RT E = E° - . In Q nF where E = potential under non-standard conditions standard potential = ideal gas constant T = kelvin temperature n = number of moles of electrons for the reaction as written F = charge carried by 1 mol of electrons Q = reaction quotient E° R It is customary to use the equation in a form where numerical values are substituted for R, T and F at a temperature of 25 °C. For R = 8.314 J mol'K! T = 298.15 K 96,485 J V-l mol" F = (8.314 J mol! K(298.15 K) RT = 0.0257 V F 96,485 J V-' mol-1 and the Nernst equation with the potentials in volts is: Previous 0.0257 In 0 Hatural lagarithn.
and the Nernst equation with the potentials in volts is:
0.0257
E = E°
In Q
natural logarithm
Sometimes it is more convenient to use base-10 logarithms and the substitution of 2.303 log for In is made. (2.303 x 0.0257 = 0.0592)
Then, the Nernst equation for base-10 logs at 25 °C is:
0.0592
E = E°
log Q
base-10 logarithm
n
A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm.
Transcribed Image Text:and the Nernst equation with the potentials in volts is: 0.0257 E = E° In Q natural logarithm Sometimes it is more convenient to use base-10 logarithms and the substitution of 2.303 log for In is made. (2.303 x 0.0257 = 0.0592) Then, the Nernst equation for base-10 logs at 25 °C is: 0.0592 E = E° log Q base-10 logarithm n A common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm.
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