The iron oxide can be reduced by the reaction: Fe2O3(s)+3C(graphite)--->2Fe(s)+3

Question

The iron oxide can be reduced  by the reaction:

                          

                                        Fe2O3(s)+3C(graphite)--->2Fe(s)+3CO(g)

Is the process spontaneous under standard conditions?How is it influenced by the rise of temperature?

Use the following standard values:

                                            

Substance

H^0 (kJ/mol)

S^0 (J/mol*K)

C (graphite)

0.0

5.7

Fe2O3(s)

-822.2

87.5

Fe(s.)

0.0

27.2

CO(g.)

-110.6

197.7

                                                                            

  

Substance

     

H^0 (kJ/mol)

     

S^0 (J/mol*K)

     

C (graphite)

     

0.0

     

5.7

     

Fe2O3(s)

     

-822.2

     

87.5

     

Fe(s.)

     

0.0

     

27.2

     

CO(g.)

     

-110.6

     

197.7

  

Explanation / Answer

G^0 = H^0 - TS^0

dG^0 (reaction) = G^0(products) - G^0(reactants)

G^0(products) = H^0 - TS^0 = 2x(0-(298x27.2)) + 3x(-110.6-298x197.7) = ?193286.8 kJ/mol

G^0(reactants) = H^0 - TS^0 = (-822.2 - 298x87.5) + 3x(0-298x5.7) = ?31993 kJ/mol

dG^0 (reaction) = G^0(products) - G^0(reactants)

   = ?193286.8 kJ/mol - (?31993 kJ/mol)

   = ?161293.8 kJ/mol

dG^0 = -ve => reaction is spontaneous

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