Fuel cells with molten alkali metal carbonates as electrolytes can use methane as a fuel. The methane is first converted into hydrogen in a two-step process: CH4(g) + H₂O(g) →CO(g) + 3 H₂(g) CO(g) + H₂O(g) → H₂(g) + CO₂(g) a. Assign oxidation numbers to carbon and hydrogen in the reactants and products. b. Using the standard free energy of formation values in Table A4.3 in Appendix 4, calculate the standard free-energy changes in the two reactions and the overall AG for the formation of H₂ + CO₂ from methane and steam.
Fuel cells with molten alkali metal carbonates as electrolytes can use methane as a fuel. The methane is first converted into hydrogen in a two-step process: CH4(g) + H₂O(g) →CO(g) + 3 H₂(g) CO(g) + H₂O(g) → H₂(g) + CO₂(g) a. Assign oxidation numbers to carbon and hydrogen in the reactants and products. b. Using the standard free energy of formation values in Table A4.3 in Appendix 4, calculate the standard free-energy changes in the two reactions and the overall AG for the formation of H₂ + CO₂ from methane and steam.
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 83E: Consider a concentration cell that has both electrodes made of some metal M. Solution A in one...
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I’m stuck with part 18:89 can you please help me to understand
![benefits.
Problems
18.89. Fuel cells with molten alkali metal carbonates as
electrolytes can use methane as a fuel. The methane is first
converted into hydrogen in a two-step process:
CH4(g) + H₂O(g) →CO(g) + 3 H₂(g)
CO(g) + H₂O(g) → H₂(g) + CO₂(g)
a. Assign oxidation numbers to carbon and hydrogen in
the reactants and products.
b. Using the standard free energy of formation values
in Table A4.3 in Appendix 4, calculate the standard
free-energy changes in the two reactions and the overall
AG for the formation of H₂ + CO₂ from methane and
steam.
*18.90. A direct methanol fuel cell uses the oxidation of methanol
by oxygen to generate electrical energy. The overall
reaction, which is given below, has a AG value of -702.4
kJ/mol of methanol oxidized. What is the standard cell
potential for this fuel cell?
CH₂OH() + O₂(g) →CO₂(g) + 2 H₂O(l)
Additional Problems
18.91. Calculate the Ecell value at 298 K for the cell based on the
reaction
Fe³+ (aq) + Cut (aq) → Fe²+ (aq) + Cu²+ (aq)
when [Fe³+] = [Cut] = 1.50 x 10-³ M and [Fe²+] =
[Cu²+] = 2.5 x 10-4 M.
18.92. Calculate the Ecell value at 298 K for the cell based on the
reaction
Cu(s) + 2 Ag+ (aq) → Cu²+ (aq) + 2 Ag(s)
when [Ag] = 2.56 x 10-3 M and [Cu2+] = 8.25 x 10-4 M.
18.9
18.98
*18.99.
*18.100.
C
r
t
a](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fca02d504-5e24-41f0-ab73-e50e96514c35%2F8cb9aadc-dba1-4c72-9ddf-02a3129f22ce%2F64pp6ou_processed.jpeg&w=3840&q=75)
Transcribed Image Text:benefits.
Problems
18.89. Fuel cells with molten alkali metal carbonates as
electrolytes can use methane as a fuel. The methane is first
converted into hydrogen in a two-step process:
CH4(g) + H₂O(g) →CO(g) + 3 H₂(g)
CO(g) + H₂O(g) → H₂(g) + CO₂(g)
a. Assign oxidation numbers to carbon and hydrogen in
the reactants and products.
b. Using the standard free energy of formation values
in Table A4.3 in Appendix 4, calculate the standard
free-energy changes in the two reactions and the overall
AG for the formation of H₂ + CO₂ from methane and
steam.
*18.90. A direct methanol fuel cell uses the oxidation of methanol
by oxygen to generate electrical energy. The overall
reaction, which is given below, has a AG value of -702.4
kJ/mol of methanol oxidized. What is the standard cell
potential for this fuel cell?
CH₂OH() + O₂(g) →CO₂(g) + 2 H₂O(l)
Additional Problems
18.91. Calculate the Ecell value at 298 K for the cell based on the
reaction
Fe³+ (aq) + Cut (aq) → Fe²+ (aq) + Cu²+ (aq)
when [Fe³+] = [Cut] = 1.50 x 10-³ M and [Fe²+] =
[Cu²+] = 2.5 x 10-4 M.
18.92. Calculate the Ecell value at 298 K for the cell based on the
reaction
Cu(s) + 2 Ag+ (aq) → Cu²+ (aq) + 2 Ag(s)
when [Ag] = 2.56 x 10-3 M and [Cu2+] = 8.25 x 10-4 M.
18.9
18.98
*18.99.
*18.100.
C
r
t
a
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