Calculate ΔH for the reaction N2 H4(l)+O2(g) ⟶N2(g)+2 H2 O(l) given the following data: 2 NH3(g

step 1 Let's calculate delta H for the given reaction. We're going to take reaction 1 as it is, which w

Calculate ΔH for the reaction N2 H4(l)+O2(g) ⟶N2(g)+2 H2...

Calculate $\Delta H$ for the reaction $$ \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) $$ given the following data: $$ \begin{aligned} 2 \mathrm{NH}_{3}(g)+3 \mathrm{~N}_{2} \mathrm{O}(g) & \longrightarrow 4 \mathrm{~N}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l) & \Delta H &=-1010 . \mathrm{kJ} \\ \mathrm{N}_{2} \mathrm{O}(g)+3 \mathrm{H}_{2}(g) & \longrightarrow \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{H}_{2} \mathrm{O}(l) & \Delta H &=-317 \mathrm{~kJ} \\ 2 \mathrm{NH}_{3}(g)+\frac{1}{2} \mathrm{O}_{2}(g) & \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{H}_{2} \mathrm{O}(l) & \Delta H &=-143 \mathrm{~kJ} \\ \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) & \Delta H &=-286 \mathrm{~kJ} \end{aligned} $$

Calculate $\Delta H$ for the reaction
$$
\mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{O}_{2}(g) \longrightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)
$$
given the following data:
$$
\begin{aligned}
2 \mathrm{NH}_{3}(g)+3 \mathrm{~N}_{2} \mathrm{O}(g) & \longrightarrow 4 \mathrm{~N}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l) & \Delta H &=-1010 . \mathrm{kJ} \\
\mathrm{N}_{2} \mathrm{O}(g)+3 \mathrm{H}_{2}(g) & \longrightarrow \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{H}_{2} \mathrm{O}(l) & \Delta H &=-317 \mathrm{~kJ} \\
2 \mathrm{NH}_{3}(g)+\frac{1}{2} \mathrm{O}_{2}(g) & \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{H}_{2} \mathrm{O}(l) & \Delta H &=-143 \mathrm{~kJ} \\
\mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) & \Delta H &=-286 \mathrm{~kJ}
\end{aligned}
$$

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Key Concepts

Hess's Law

Hess's Law states that the total enthalpy change for a chemical reaction is the same, regardless of the path taken from reactants to products. This principle allows for the combination, reversal, and scaling of individual chemical equations with known enthalpy changes to calculate the overall enthalpy change of a reaction.

Reaction Manipulation

Reaction manipulation involves the reversal, addition, or multiplication of given chemical equations so that, when they are summed, they yield the desired target reaction. During this process, the enthalpy values must be adjusted correspondingly; for example, reversing a reaction changes the sign of its enthalpy change and multiplying a reaction by a factor multiplies its enthalpy change by the same factor.

Stoichiometry

Stoichiometry in this context refers to the use of balanced coefficients in chemical reactions to ensure that the conservation of mass and atoms is maintained. Proper stoichiometric manipulation ensures that species cancel out or combine appropriately when applying Hess's Law, leading to the correct overall reaction and its enthalpy change.

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