Use standard reduction potentials to calculate the equilibrium constant for the reaction:2Ag+(aq) + Pb(s) → 2Ag(s) + Pb2+(aq)Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.Equilibrium constant: _____G° for this reaction would be _________ (greater or less) than zero. Sometimes the base-10 logarithm is used and the substitution of 2.303 log for In is made. (2.303 × 0.0257 = 0.0592) Then, the equationfor base-10 logs at 25 °C is:0.0592E°celllog Kbase-10 logarithmnA common student error is to use the wrong kind of logarithm. Be sure, when you choose an equation, to use the correct logarithm. Relationship between E°cell and KThe equilibrium constant for a cell reaction can be calculated from the standard cell voltage. The relationship between them is:RTE°.cell- In KnFwherestandard cell potentialideal gas constantT = kelvin temperaturen = number of moles of electrons for the reaction as writtenF = charge carried by 1 mol of electronsK = equilibrium constantE°R%3DIt 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.ForR = 8.314 J molr'K!T =298.15 KF96,485 J V' mol"1(8.314 J moll K)(298.15 K)RT= 0.0257 VF96,485 J V' mol"and the equation with the potential in volts is:0.0257E° cellIn Knatural logarithmPreviousNext

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Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 105QAP: Consider a voltaic cell in which the following reaction occurs. Zn(s)+Sn2+(aq)Zn2+(aq)+Sn(s) (a)...

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Use standard reduction potentials to calculate the equilibrium constant for the reaction:

2Ag⁺(aq) + Pb(s) → 2Ag(s) + Pb²⁺(aq)

Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm.

Equilibrium constant: _____

G° for this reaction would be _________ (greater or less) than zero.

Sometimes the base-10 logarithm is used and the substitution of 2.303 log for In is made. (2.303 × 0.0257 = 0.0592) Then, the equation
for base-10 logs at 25 °C is:
0.0592
E°
cell
log K
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.

Relationship between E°cell and K
The equilibrium constant for a cell reaction can be calculated from the standard cell voltage. The relationship between them is:
RT
E°.
cell
- In K
nF
where
standard cell 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
K = equilibrium constant
E°
R
%3D
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 molr'K!
T =
298.15 K
F
96,485 J V' mol"1
(8.314 J moll K)(298.15 K)
RT
= 0.0257 V
F
96,485 J V' mol"
and the equation with the potential in volts is:
0.0257
E° cell
In K
natural logarithm
Previous
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