Question

Study the reaction. NO(g) ⇌ 12N2(g) + 12O2(g) ΔH = −90.3 kJ Which statement about the reaction is correct? A) The reverse reaction releases 90.3 kJ/mol of energy. B) If one mole of O2 is formed, then 180.6 kJ energy is absorbed. C) The products have higher energy than the reactants. D) The forward reaction is an exothermic reaction.

Answer 1

D) The reaction is an exothermic reaction.

Step-by-step explanation:

I just took the test and got it right.

Hope this helps :)

Answer 2

The forward reaction is an exothermic reaction.

Step-by-step explanation:

An exothermic reaction is one in which energy is released, usually in the form of heat hence the enthalpy of the reaction is negative. When a reaction exothermic, the energy of the reactants is greater than the energy of the products hence the excess energy is given out as heat. The reactants lie at a higher energy level in the reaction profile compared to the products.

When we look at the reaction given in the question, NO(g) ⇌ 12N2(g) + 12O2(g) ΔH = −90.3 kJ , we can easily see from the thermochemical reaction that the forward reaction is exothermic, energy is released by the reaction system as evidenced by the negative enthalpy of reaction.