Question

Asked Oct 21, 2019

Given the following:

2 Fe_{(s)} + 3/2 O_{2(g)} → Fe_{2}O_{3(s)} ΔH^{o}_{rxn} = -824.2 kJ/mol

3 Fe_{(s)} + 2 O_{2(g)} → Fe_{3}O_{4(s)} ΔH^{o}_{rxn} = -1118.4 kJ/mol

Calculate the ΔH^{o}_{rxn} for the following equation:

3 Fe_{2}O_{3(s)} → 2 Fe_{3}O_{4(s)} + 1/2 O_{2(g)}

Your answer should be to one place past the decimal point.

Step 1

Thermodynamic is the branch of chemistry that mainly deals with the heat transfer between system and surroundings. Here system is the substance for which the heat content is studied and remaining part of universe is consider as the surroundings.

Step 2

The heat content of any substance or reaction system can be expressed in terms of enthalpy whereas the randomness in the system is associated with the entropy of system.

Hess law states that the enthalpy change for multistep chemical reaction is the sum of all enthalpy changes. It can be written as;

Step 3

Given:

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