Use cell potential to calculate an equilibrium constant.
Calculate the cell potential and the equilibrium constant for
the following reaction at 298 K:
Cu2+(aq) +
Hg(l) =
Cu(s) +
Hg2+(aq)
Hint: Carry at least 5 significant figures during intermediate
calculations to avoid round off error when taking the
antilogarithm.
Equilibrium constant: -------
Derive and explain the relationship between the Nernst equation,
the equilibrium constant and other thermodynamic quantities such as
enthalpy, Gibbs energy and entropy of reaction.
Derive an expression of the van Deemter equation that shows how
to calculate the minimum value of H based upon the values for A, B
and C and not flow rate. (Assume the C terms are combined into one
C term).
Using E° = .697 V and the Nernst equation, calculate the
concentration of Hg2+ in a sample of pond water if [Sn2+] = 0.500
M, [Sn4+] = 0.305 M and Ecell = 0.711 V.
(i) Use the information in the Resource section to calculate the
standard potential of the cell Ag(s)|AgNO3(aq)||Cu(NO3)2(aq)|Cu(s)
and the standard Gibbs energy and enthalpy of the cell reaction at
25°C.
(ii) Estimate the value of AG at 35 °C.
a. Show with the aid of a form of the Nernst equation that when
using a pH sensitive glass electrode and reference electrode that
the measured potential is proportional to pH.
b. Sketch a diagram of a pH sensitive glass electrode, label all
parts and indicate the function of each part.
(A) Derive Bernoulli's Equation from Pressure, Kinetic Energy and Potential Energy
(B) Express Bernoulli's equation:
- Per unit mass
-Per unit volume
- In terms of heads
Calculate the cell potential for a reaction in a electrolytic
cell with the following half-reactions if: [U 3+] = 0.10 M, [MnO4 -
] = 0.20M, [Mn2+], and [H+ ] = 0.20 M
U 3+ + 3e -> U o Ecell = - 1.642 V
MnO4 - + 8H+ + 5e- -> Mn2+ + 4H2O Ecell = +1.51 V
Use the current-voltage equation for the Na+ and K+ currents to
derive the GHK equation for the reversal potential for a channel
permeable to both Na+ and K+.