Question

The oxidation of nitrogen in the hot exhaust of jet engines and automobiles occurs by the reaction n2(g) o2(g) −→ 2 no(g) ∆h ◦ = 180.6 kj how much heat is absorbed in the formation of 1.54 mol no? answer in units of kj.

Answer 1

To calculate the heat absorbed in the formation of 1.54 mol NO, you use the given enthalpy change of 180.6 kJ for 2 moles and find that 139.23 kJ of heat is absorbed for the formation of 1.54 mol NO.

Step-by-step explanation:

The oxidation of nitrogen in the hot exhaust of jet engines and automobiles is represented by the reaction N2(g) + O2(g) → 2 NO(g), with an enthalpy change (ΔH°) of 180.6 kJ for the formation of 2 moles of NO. To find out how much heat is absorbed in the formation of 1.54 mol NO, we need to use the concept of stoichiometry and proportionality.

Since the given ΔH° corresponds to 2 moles of NO, for 1 mole of NO, the heat absorbed would be half of 180.6 kJ. Therefore, for 1.54 moles the calculation is as follows:

Heat absorbed = 180.6 kJ/2 × 1.54

= 139.23 kJ

This calculation shows that 139.23 kJ of heat is absorbed during the formation of 1.54 mol NO in the reaction between nitrogen and oxygen.