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Leviafan [203]
2 years ago
5

he thermite reaction, in which powdered aluminum reacts with iron(III) oxide, is highly exothermic. 2 Al(s) + Fe2O3(s) Al2O3(s)

+ 2 Fe(s) Use standard enthalpies of formation to find for the thermite reaction
Chemistry
1 answer:
Afina-wow [57]2 years ago
4 0

The given question is incomplete. The complete question is

The thermite reaction, in which powdered aluminum reacts with iron oxide, is highly exothermic: 2Al(s)+Fe_2O_3(s)\rightarrow Al_2O_3(s)+2Fe(s). Use standard enthalpies of formation to find ΔH∘rxn for the thermite reaction. Express the heat of the reaction in kilojoules to four significant figures.

Answer: ΔH∘rxn for the thermite reaction is -851.5 kJ

Explanation:

The balanced chemical reaction is :

2Al(s)+Fe_2O_3(s)\rightarrow Al_2O_3(s)+2Fe(s)

We have to calculate the enthalpy of reaction (\Delta H^o).

\Delta H^o=H_f_{product}-H_f_{reactant}

\Delta H^o=[n_{Fe}\times \Delta H_f^0_{(Fe)}+n_{Al_2O_3}\times \Delta H_f^0_{(Al_2O_3)}]-[n_{Al}\times \Delta H_f^0_(Al)+n_{Fe_2O_3}\times \Delta H_f^0_{(Fe_2O_3)}]

where,

We are given:

\Delta H^o_f_{(Fe_2O_3(s))}=-824.2kJ/mol\\\Delta H^o_f_{(Al_2O_3(s))}=-1675.7kJ/mol\\\Delta H^o_f_{(Fe(s))}=0kJ/mol\\\Delta H^o_f_{(Al(s)}=0kJ/mol

Putting values in above equation, we get:

\Delta H^o_{rxn}=[(2\times 0)+(1\times -1675.5)]-[(2\times 0)+(1\times -824.2)]=-851.5kJ

ΔH∘rxn for the thermite reaction is -851.5 kJ

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Percentage Yield is Calculated as,

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Explanation:

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