Consider the following reaction. 2Fe2O3 --> 4Fe + 3O2 deltaH = +824.2KJ The formation of 42.0 g of O2 results in? 1) the absorption of 361 kJ of heat. 2) the absorption of 11500 kJ of heat. 3) the absorption of 1080 kJ of heat.

If deltaH is positive, that means the reaction took heat from its environment (endothermic reaction).
The molar mass of O2 is 32 g/mol.
Therefore, 42g of O2 is equal to 1.3 moles O2.
The equation assumes 3 moles of O2. That means, only 1.3/3 = 43% of the delta H in the equation was formed.
824.2 kJ x 43% = 354 kJ. The closest answer is 1) the absorption of 361 kJ of heat.

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tutorareej tutorareej · Answer 2 · 2021-10-19T12:06:19+02:00

The formation of oxygen in the reaction, the absorption of 361 kJ of heat takes place.

The heat of formation of oxygen will be

[tex]\rm \Delta H[/tex] is +824.2 kJ.

The positive sign of H denotes that the reaction accepts energy from the surroundings. It is an endothermic reaction.

In the reaction the % formation of Oxygen is :

Total product formed = 7 moles

Oxygen formed = 3 moles

% Oxygen formed = [tex]\rm \frac{3}{7}\;\times\;100[/tex]

% oxygen formed = 42.85 %

The total enthalpy for the formation of product is +824.2 kJ.

The enthalpy for the formation of 42.85 % Oxygen = +824.2 [tex]\times[/tex] 42.85 / 100 kJ.

The enthalpy of the formation of oxygen in the reaction will be 353.22 kJ.

The closest is 361 kJ.

So, for the formation of oxygen in the reaction, the absorption of 361 kJ of heat takes place.

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