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Given: 

(i) \; 2Fe_{2}O_{3}_{(s)} \rightarrow 4Fe_{(s)} + 3O_{2(g)}\; ; \;\Delta\:_{r}G^{o} = + 1487.0\:kJ\;mol^{-1}

(ii) \; 2CO_{(g)} + O_{2(g)}\rightarrow 2CO_{2(g)}\; ; \;\Delta\:_{r}G^{o} = -514.4\:kJ\;mol^{-1}

Free energy change, \Delta\:_{r}G^{o} for the reaction   2Fe_{2}O_{3(s)} + 6CO_{g} \rightarrow 4Fe_{(s)} + 6 CO_{2(g)}  will be :

  • Option 1)

    −112.4 kJ mol −1

  • Option 2)

    −56.2 kJ mol −1

  • Option 3)

    −168.2 kJ mol −1

  • Option 4)

    −208.0 kJ mol −1

 

Answers (2)

best_answer

As we have learnt,

 

ΔG{reaction} -

\Delta G _{reaction }= \sum \Delta G_{product}- \sum \Delta G_{reactant}
 

- wherein

\sum \Delta G_{product}=Sum of   \Delta G of all product

\sum \Delta G_{reactant}=Sum of   \Delta G of all reactant

 

 \Delta G_{Reaction} = \Delta G_{1} + 3\times \Delta G_{2} \\*\Rightarrow \Delta G_{Reaction} = 1487 + (3\times -514.4) = -56.2\;kJ\:mol^{-1}

 


Option 1)

−112.4 kJ mol −1

Option 2)

−56.2 kJ mol −1

Option 3)

−168.2 kJ mol −1

Option 4)

−208.0 kJ mol −1

Posted by

prateek

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