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

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: \[ \mathrm{NO}(g) + \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{NO}_{2}(g) \] It is stated that 57.1 kJ of energy is evolved for each mole of $\mathrm{NO}(g)$ that reacts. This indicates that the reaction is exothermic, and the enthalpy change $\Delta H$ should be negative.

Step 2: Determine the Enthalpy Change for the Reaction

Since the reaction involves 1 mole of $\mathrm{NO}(g)$ reacting, the enthalpy change $\Delta H$ 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: \[ \mathrm{NO}(g) + \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{NO}_{2}(g) \quad \Delta H = \boxed{-57.1 \, \text{kJ}} \]

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