A. The reaction produces 165E3 kJ for 2 mols; therefore, delta H = -165E3 kJ for 2 mols. My thermodynamic tables don't give this value. Look to see that you have posted the right number. I'm thinking you meant 1650. I will use your value to answer A and C.
B. This site does not support us drawing diagrams. Sorry.
C. So you have 165E3 kJ for 159.7 x 2 or 319.4 g Fe2O3. For 23.6 you will have 165E3 kJ x (23.6/319.4) = ? kJ.
The reaction of iron with oxygen is very familiar. You can see the resulting rust on buildings, vehicles and bridges. You may be surprised, however at the large amount of heat that is produced by this reaction.
4Fe(g) + 3O2(g) 2Fe2O3(g) + 165 x 103 kJ
(a) What is the enthalpy change for this reaction?
(b) Draw the enthalpy diagram that corresponds to the thermochemical equation.
(c) What is the enthalpy change for the formation of 23.6 g iron (III) oxide?
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