2Fe2O3 -> 4Fe+3O2 changeHrxn= +824.2 KJ
The decomposition of 57.0 g of Fe2O3 results in
The release of 23500 KJ of heat
The absorption of 147 KJ of heat
The absorption of 23500 KJ of heat
The absorption of 294 KJ of heat
The release of 294 KJ of heat
The release of 147 KJ of heat
This is done just like your last problem except this one is endothermic so energy is being absorbed (because of the + sign on delta H).
the release of 147 kj of heat
Its the absorption of 147kJ
Source:
Got it right on sapling
The decomposition of 89.0 g of Fe2O3 results in
To determine the heat released or absorbed during the decomposition of 57.0 g of Fe2O3, we can use the concept of heat of reaction (ΔHrxn) and stoichiometry.
Given:
ΔHrxn = +824.2 kJ (positive sign indicates the reaction is endothermic)
First, let's calculate the molar mass of Fe2O3:
Molar mass of Fe2O3 = (2 × atomic mass of Fe) + (3 × atomic mass of O)
= (2 × 55.845 g/mol) + (3 × 16.00 g/mol)
= 159.69 g/mol
Next, we need to find the number of moles of Fe2O3 using the given mass:
Number of moles = Mass / Molar mass
= 57.0 g / 159.69 g/mol
≈ 0.3574 mol
Now, according to the balanced chemical equation:
2Fe2O3 -> 4Fe + 3O2
We can see that for every 2 moles of Fe2O3 decomposed, 4 moles of Fe and 3 moles of O2 are produced.
Using stoichiometry, we can calculate the molar heat of reaction as follows:
Molar heat of reaction = ΔHrxn / Moles of Fe2O3
= 824.2 kJ / 0.3574 mol
≈ 2305 kJ/mol
Finally, to find the total heat released or absorbed during the decomposition of 57.0 g of Fe2O3, we multiply the molar heat of reaction by the number of moles:
Total heat released or absorbed = Molar heat of reaction × Moles of Fe2O3
≈ 2305 kJ/mol × 0.3574 mol
≈ 824.2 kJ
Therefore, the correct answer is:
The release of 824.2 kJ of heat.