Acetylene burns in air according to the following equation: C2H2(g)+2^5O2(g) ⟶ 2 CO2(g)+H2O

step 1 To calculate the delta H of formation of acetylene, we'll start with the delta H for this partic

Acetylene burns in air according to the following equation:...

Acetylene burns in air according to the following equation: $$\begin{array}{r}\mathrm{C}_{2} \mathrm{H}_{2}(g)+{ }_{2}^{5} \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) \\ \Delta H_{\mathrm{ru}}^{\circ}=-1255.8 \mathrm{~kJ}\end{array}$$Given $\Delta H_{\mathrm{f}}^{\circ}$ of $\mathrm{CO}_{2}(g)=-393.5 \mathrm{~kJ} / \mathrm{mol}$ and $\Delta H_{\mathrm{f}}^{\circ}$ of $\mathrm{H}_{2} \mathrm{O}(g)=$$-241.8 \mathrm{~kJ} / \mathrm{mol},$ find $\Delta H_{i}$ of $\mathrm{C}_{2} \mathrm{H}_{2}(g)$

Acetylene burns in air according to the following equation:
$$\begin{array}{r}\mathrm{C}_{2} \mathrm{H}_{2}(g)+{ }_{2}^{5} \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) \\
\Delta H_{\mathrm{ru}}^{\circ}=-1255.8 \mathrm{~kJ}\end{array}$$Given $\Delta H_{\mathrm{f}}^{\circ}$ of $\mathrm{CO}_{2}(g)=-393.5 \mathrm{~kJ} / \mathrm{mol}$ and $\Delta H_{\mathrm{f}}^{\circ}$ of $\mathrm{H}_{2} \mathrm{O}(g)=$$-241.8 \mathrm{~kJ} / \mathrm{mol},$ find $\Delta H_{i}$ of $\mathrm{C}_{2} \mathrm{H}_{2}(g)$

Key Concepts

Stoichiometry

Stoichiometry involves the quantitative relationships among reactants and products in a chemical reaction. It is essential for determining the proportional amounts of substances involved, ensuring that calculations of energy changes, like enthalpy, account accurately for the reaction's balanced nature.

Standard Enthalpy of Reaction

This concept refers to the overall heat change associated with a chemical reaction under standard conditions. It can be calculated from the standard enthalpies of formation of the reactants and products, taking into account the stoichiometry of the reaction, and reflects the energy absorbed or released during the process.

Standard Enthalpy of Formation

This is the enthalpy change when one mole of a compound is formed from its constituent elements in their standard states under standard conditions (usually 25°C and 1 atm pressure). It serves as a reference point for calculating enthalpy changes in chemical reactions and is fundamental to thermodynamics and calorimetry.

Hess's Law

Hess's Law states that the total enthalpy change of a chemical reaction is independent of the pathway taken, which means that the overall enthalpy change can be determined by summing the enthalpy changes of individual steps or related reactions. This principle is used to compute unknown enthalpy changes from known values.

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