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2Fe2O3 (s) + 3C (s) –––> 4Fe (s) + 3CO2 (g)

Reaction 2Fe2O3 (s) 3C (s) –––> 4Fe (s) 3CO2 (g)

ΔH (KJ/mol)

 -824.2 0 0 -397.5

ΔS (J/molK)

 87.4 5.74 27.23 213.6

(A) Calculate ΔG° for this reaction

(B) How many electrons are transferred in the balanced reaction above?

(C) Calculate E° for the same reaction

(D) Using the Nernst Equation,what is the E value of the reaction if the partial pressure of CO2 drops to 0.0346 atm?

(E) Explain in a complete sentence why this reaction is or is not spontaneous using both ΔG and E found above

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Keith Leannon
Keith LeannonLv2
6 Jun 2022

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Related questions

The reaction shown below is involved in the refining of iron.
2Fe2O3(s) + 3C(s, graphite) ? 4Fe(s) + 3CO2(g)
Compound ?Hf° (kJ/mol) S° (J/mol/K) ?Gf° (kJ/mol)
Fe2O3(s) –824.2 ? –742.2
C(s, graphite) 0 5.740 0
Fe(s) 0 27.3 0
CO2(g) –393.5 213.6 –394.4
(6 pts) (a). Use data from the table above as needed to find ?H°for the reaction.
(6 pts) (b). ?S° for the reaction above is 557.98 J/K. Find S° forFe2O3(s).
c)Calculate ?G° for the reaction at the standard temperature of 298K. (There are at least 2
possible ways that you could do this.)
(7 pts) (d). At what temperatures would this reaction bethermodynamically spontaneous?

answers should be 9. (a). 467.9 kJ, (b). 87.4 J/K/mol, (c). 301.5kJ, (d). T > 839 K

1. Consider a voltaic (galvanic) cell with the following metal electrodes. Identify which metal is the cathode and which is the anode, and calculate the cell potential.

(a) Al and Co(II)
Cathode: ____

Anode: ______

Ecell =

(b) Cd(II) and Ag(I)

cathode: ___

anode: ___

Ecell= ____

(c) Cr(III) and Sc(III)

cathode: ___

Anode:_____

Ecell:____

2. A voltaic cell contains two half-cells. One half-cell contains a titanium electrode immersed in a 1.00 M Ti(NO3)3 solution. The second half-cell contains a zinc electrode immersed in a 1.00 M Zn(NO3)2 solution.

Ti3+(aq) + 3 e− → Ti(s)

E⁰red  = −1.370 V
Zn2+(aq) + 2 e− → Zn(s)

E⁰red  = −0.762 V

(a) Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell.

(b) Write the overall balanced equation for the voltaic cell. (Include states-of-matter under the given conditions in your answer.)

3. ΔG° and E° can be said to measure the same thing, and are convertible by the equation

ΔG° = −nFE⁰cell 

where n is the total number of moles of electrons being transferred, and F is the Faraday constant 9.64853415 ✕ 104 C/mol. The free energy (ΔG°) of a spontaneous reaction is always negative.

For each of the electrochemical cells below, calculate the free energy of the system and state whether the reaction is spontaneous or non-spontaneous as written based on the cathode and anode assignment given. (Use the table of Standard Electrode Potentials.)

(a) The cathode is Zn(II) and the anode is Co(II).

free energy: ____ kJ

spontaneity: _____

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