Question

Nitrogen dioxide, NO2(g) (Delta. Hf = 33. 84 kJ/mol), is decomposed according to the following reaction: 2 upper N upper O subscript 2 (g) right arrow upper N subscript 2 (g) plus 2 upper O subscript 2 (g). What is the enthalpy change when 2. 50 mol of nitrogen dioxide decomposes? Use Delta H r x n equals the sum of delta H f of all the products minus the sum of delta H f of all the reactants. 13. 5 kJ of energy released 13. 5 kJ of energy absorbed 84. 6 kJ of energy released 84. 6 kJ of energy absorbed.

Answer 1

The heat of Reaction or Enthalpy is defined as the changes in the heat during a chemical reaction. The change in heat is calculated as the sum of all the heat change in products minus the sum of all the changes in the reactants.

How do you calculate the heat change in the reaction?

The chemical reaction between nitrogen and oxygen is given as:

$\rm 2 N O_2 \rightarrow N_2 + 2 O_2\\\\ \rm \Delta\; H_{f} &= 33.84 kJ/mol$

Now, we know:

• 1 mol Nitrogen dioxide requires = 33.84 kJ/mol
• 2.50 mol of nitrogen oxide will give  = $33.84 \times 2.50$
• Energy released = 84.6 energy released

Thus, the enthalpy change for the reaction will be 84.6 energy released.

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Answer 2

Answer:

C. 84.6 kJ of energy released

Explanation:

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