Given that 4 NH3(g)+5 O2(g) →4 NO(g)+6 H2 O(l) ΔHrxn^∘=-1166 kJ ·mol^-1 4 NH3(g)+3 O2(g) →2 N2

step 1 In this question we want to determine the end of the change associated with the reaction of nitr

Given that 4 NH3(g)+5 O2(g) →4 NO(g)+6 H2 O(l) ΔHrxn^∘=-1166...

Given that $4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \rightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)$ $$ \Delta H_{\mathrm{rxn}}^{\circ}=-1166 \mathrm{~kJ} \cdot \mathrm{mol}^{-1} $$ $4 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{~N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)$ $$ \Delta H_{\mathrm{rxn}}^{\circ}=-1531 \mathrm{~kJ} \cdot \mathrm{mol}^{-1} $$ calculate the value of $\Delta H_{\mathrm{rxn}}^{\circ}$ for the equation $$ \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{NO}(g) $$

Given that
$4 \mathrm{NH}_{3}(g)+5 \mathrm{O}_{2}(g) \rightarrow 4 \mathrm{NO}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)$
$$
\Delta H_{\mathrm{rxn}}^{\circ}=-1166 \mathrm{~kJ} \cdot \mathrm{mol}^{-1}
$$
$4 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \rightarrow 2 \mathrm{~N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l)$
$$
\Delta H_{\mathrm{rxn}}^{\circ}=-1531 \mathrm{~kJ} \cdot \mathrm{mol}^{-1}
$$
calculate the value of $\Delta H_{\mathrm{rxn}}^{\circ}$ for the equation
$$
\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{NO}(g)
$$

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Key Concepts

Thermochemical Equation Manipulation

Manipulating thermochemical equations involves reversing, scaling, and adding chemical equations to cancel out intermediate species and obtain a target reaction. When these equations are combined, their corresponding enthalpy changes are added algebraically, taking into account any changes in coefficients or directions of the reactions, which is fundamental to applying Hess's Law.

Hess's Law

Hess's Law states that the total enthalpy change for a chemical reaction is the same regardless of the pathway taken, since enthalpy is a state function. This principle allows one to calculate the enthalpy change of a reaction by algebraically adding, subtracting, or scaling the enthalpy changes of other reactions that, when combined, yield the overall reaction.

Enthalpy as a State Function

Because enthalpy is a state function, its change depends only on the initial and final states of a process and not on the pathway. This means that by properly manipulating and combining reactions, the overall enthalpy change of a desired reaction can be determined, irrespective of the intermediate steps involved.

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