In a hydrogen-oxygen fuel cell, gaseous hydrogen serves as the
fuel, oxygen in the air as the oxidizer, and the reaction product
is water. Consider that flat plates of Pt are used as electrodes at
25°C and fuel and air are supplied at 1 atm. [20%] (a) Write the
Nernst expression for each half-cell reaction. (b) What is the
overall cell reaction? (c) Calculate the cell voltage, Ecell, given
the above conditions. (d) Suppose that the supply of hydrogen and...
A direct hydrogen fuel cell uses hydrogen and air (oxygen) to
produce electricity, as we showed in class.
If you wanted a voltage of 2.2 V for your fuel cell device
(which can be made of multiple cells), what mix of conversion
and/or number of cells would you want to use? Remember: the voltage
of cells in series adds up. There are a variety of possible
answers.
A hydrogen-oxygen fuel cell is used in the space program to
generate clean energy. Describe, in detail, the principle and
process of electrical energy generation from hydrogen-oxygen fuel
cell. Also include in the discussion major advantages and
limitations of such fuel cells.
a hydrogen-oxygen fuel cell is used in the space program to
generate clean energy. Describe, in detail, the principle and
process of electrical energy generation from hydrogen-oxygen fuel
cell. Also include in the discussion major advantages and
limitations of such fuel cells.
Hydrogen gas (a potential future fuel) can be formed by the
reaction of methane with water according to the following equation:
CH4(g)+H2O(g)→CO(g)+3H2(g)CH4(g)+H2O(g)→CO(g)+3H2(g) In a
particular reaction, 26.5 LL of methane gas (measured at a pressure
of 736 torr and a temperature of 25 ∘C) is mixed with 22.6 L of
water vapor (measured at a pressure of 702 torr and a temperature
of 125 ∘C). The reaction produces 26.2 L of hydrogen gas at STP.
Part A What is the...
The standard cell potential for the nickel–cadmium battery is
1.35 V, and the cell reaction can be written as
2NiO(OH)(s) + 2H2O(l) + Cd(s) ? 2Ni(OH)2(s) + Cd(OH)2(s)
Which one of the following statements do you expect to be true
based on the Nernst equation? Note Q =
reaction quotient, and K = equilibrium constant for the cell
reaction:
a. As the battery is used, the cell voltage approaches zero
because Q approaches K, in value.
b. When the battery...
Determine the overall reaction and its standard cell potential
at 25 °C for the reaction involving the galvanic cell made from a
half-cell consisting of a silver electrode in 1 M silver nitrate
solution and a half-cell consisting of a zinc electrode in 1 M zinc
nitrate. Is the reaction spontaneous at standard conditions?
For each reaction listed, determine its standard cell potential
at 25 °C and whether the reaction is spontaneous at standard
conditions.
Ag+(aq) + Cu(s)
àCu2+(aq)+ Ag(s)
Ag+ + e− ⟶ Ag +0.7996V
Cu2+ + 2e− ⟶ Cu +0.337V
a)
-1.117(nonspontaneous)
-0.4626V (nonspontaneous)
+0.4626V (spontaneous)
+1.117 (spontaneous)
Predict the standard cell potential and calculate the standard
reaction Gibbs free energy for galvanic cells having the following
cell reactions:
a) 3 Zn(s) +2Bi^3+(aq)--> 3 Zn^2+(aq) + 2Bi(s)
b) 2 H2(g) + O2(g)--> 2 H2O(l) in acidic solution
c)2 H2(g) +O2(g)--> 2 H2O(l) in basic solution
d) 3 Au+(aq) --> 2 Au(s) + Au^3+ (aq)
Write the cell reaction and electrode half-reactions and
calculate the standard potential of each of the following
cells:
a) Zn/ZnSO4(aq)//AgNO3(aq)/Ag
b) Pt/K3[Fe(CN)6](aq),
K4[Fe(CN)6](aq)//CrCl3 (aq)/Cr
Please show all steps and clear writing.
Thanks