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Justify that the following reactions are...

Justify that the following reactions are redox reactions :
`Fe_(2)O_(3)(s)+3CO(g)to2Fe(s)+3CO_(2)(g)`

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`overset(+3)(Fe_(2)) overset(-2)O_(3)(s) + 3 overset(+2)(C ) overset(-2)(O)(g) rarr overset(0)(2Fe)(s) + 3 overset(+4)(C ) overset(-2)(O_(2))(g)` In this reaction, the oxidation state of Fe is decreasing from +3 (in `Fe_(2)O_(3)`) to 0 (in Fe), hence, `Fe_(2)O_(3)` is undergoing reduction. While the oxidation number of carbon is increasing from +2 (in CO) to +4 (in `CO_(2)`) hence CO is undergoing oxidation. Therefore, it is a redox reaction.
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Justify that the following reaction are redox reactions: a. CuO(s)+H_(2)(g)rarr Cu(s)+H_(2)O(g) b. Fe_(2)O_(3)(s)+3CO(g)rarr 2Fe(s)+3CO_(2)(g) c. 4BCl_(3)(g)+3LiAlH_(4)(s) rarr 2B_(2)H_(6)(g)+3LiCl(s)+3AlCl_(3)(s) d. 2K(s)+F_(2)(g)rarr 2K^(o+)F^(Θ)(s) e. 4NH_(3)(g)+5O_(2)(g)rarr 4NO(g)+6H_(2)O(g)

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The following reaction occurs in the Blast Furnace where ions ore is reduced to iron metal : Fe_(2)O_(3)(s)+3CO(g)hArr 2Fe(l)+3CO_(2)(g) Using the Le Chatelier's principle, predict which one of the following will not disturb the equilibrium?

The following teo reaction are known : Fe_(2)O_(3)(s)+3CO(g)rarr2Fe(s)+3CO_(2)(g) , Delta H= -26.8 kJ FeO(s)+CO(g)rarr Fe(s)+CO_(2)(g) , Delta H = - 16.5 kJ Correct target equation is Fe_(2)O_(3)(s)+CO(g)rarr 2FeO(s)+CO_(2)(g), Delta H = ?

The following two reaction are known : Fe_(2)O_(3)(s)+3CO(g)rarr2Fe(s)+3CO_(2)(g) , Delta H= -26.8 kJ FeO(s)+CO(g)rarr Fe(s)+CO_(2)(g) , Delta H = - 16.5 kJ Correct target equation is Fe_(2)O_(3)(s)+CO(g)rarr 2FeO(s)+CO_(2)(g), Delta H = ?

For the reaction Fe_2N(s)+(3)/(2)H_2(g)=2Fe(s)+NH_3(g)

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