Consider the reaction:
2Fe2O3⟶4Fe+3O2 ΔH∘rxn=+824.2 kJ

The formation of 83.0 g of O2 results in:
A. the absorption of 22800 kJ of heat.
B. the release of 2140 kJ of heat.
C. the absorption of 2140 kJ of heat.
D. the release of 713 kJ of heat.
E. the absorption of 713 kJ of heat.
F. the release of 22800 kJ of heat.

The formation of given amount of oxygen gas results in the absorption of 713 kJ of heat.

Explanation:

To calculate the number of moles, we use the equation:

Given mass of oxygen gas = 83 g

Molar mass of oxygen gas = 32 g/mol

Putting values in above equation, we get:

For the given chemical equation:

Sign convention of heat:

When heat is absorbed, the sign of heat is taken to be positive and when heat is released, the sign of heat is taken to be negative.

By Stoichiometry of the reaction:

When 3 moles of oxygen gas is formed, the amount of heat absorbed is 824.2 kJ

So, when 2.594 moles of oxygen gas is formed, the amount of heat absorbed will be =

Hence, the formation of given amount of oxygen gas results in the absorption of 713 kJ of heat.

0

explanation:

488479

rvmoo+478)9.68

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.