Questions: When NO(g) reacts with O2(g) according to the following reaction, 57.1 kJ of energy are evolved for each mole of NO(g) that reacts. Complete the following thermochemical equation. ΔH=NJ(g)+O2(g) → 2 NO2(g) ΔH=?
? kJ
Transcript text: When $\mathrm{NO}(g)$ reacts with $\mathrm{O}_{2}(\mathrm{~g})$ according to the following reaction, 57.1 kJ of energy are evolved for each mole of $\mathrm{NO}(\mathrm{g})$ that reacts. Complete the following thermochemical equation. \[ \Delta H=\square \mathrm{NJ}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{NO}_{2}(g) \Delta H=? \] $\square$ kJ
Solution
Solution Steps
Step 1: Understand the Reaction and Given Information
The reaction given is:
NO(g)+O2(g)→2NO2(g)
It is stated that 57.1 kJ of energy is evolved for each mole of NO(g) that reacts. This indicates that the reaction is exothermic, and the enthalpy change ΔH should be negative.
Step 2: Determine the Enthalpy Change for the Reaction
Since the reaction involves 1 mole of NO(g) reacting, the enthalpy change ΔH for the reaction is simply the energy evolved, which is −57.1 kJ (negative because the reaction is exothermic).
Final Answer
The thermochemical equation with the enthalpy change is:
NO(g)+O2(g)→2NO2(g)ΔH=−57.1kJ