Calculate \\(\\Delta H_{{\ m{rxn}}}\\) for the following reaction: \\({\ m{Fe}}_

Question

Calculate (Delta H_{{ m{rxn}}}) for the following reaction:
({ m{Fe}}_2 { m{O}}_3 (s) + 3{ m{ CO(}}g) ightarrow 2{ m{ Fe(}}s) + 3{ m{ CO}}_2 (g))
Use the following reactions and given (Delta H{ m{'s}}).
(2{ m{ Fe(}}s); + ;3/2{ m{O}}_2 (g); ightarrow ;{ m{Fe}}_2 { m{O}}_3 (s){ m{ }}), (Delta H) = -824.2 ({ m{ kJ}})
({ m{CO(}}g); + ;{ aise0.5exhbox{$scriptstyle 1$} kern-0.1em/kern-0.15em lower0.25exhbox{$scriptstyle 2$}}{ m{O}}_2 (g); ightarrow ;{ m{CO}}_2 (g){ m{ }}), (Delta H) = -282.7 ({ m{ kJ}})

Explanation / Answer

Reversing the first reaction so that it formation entahlpy becomes = 824.2 kJ

and multiplying 3 in the second reaction i.e. 3* -282.7 kJ

and addidg both the reaction we get

Fe2O3 + (3 CO + 3/2 O2 )---> 2Fe + (3/2 O2 + 3CO2 )

we get 824.2 - 3*282.7

=- 23.9 kJ

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