Hydrogen is prepared from natural gas (mainly methane, CH4 ) by partial oxidation. CH4(g)+(1)/(2

step 1 Thermodynamics is the study of the relationship between heat, work, temperature and energy. And

Hydrogen is prepared from natural gas (mainly methane, CH4 )...

Hydrogen is prepared from natural gas (mainly methane, $\mathrm{CH}_{4}$ ) by partial oxidation. $$ \mathrm{CH}_{4}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}(g)+2 \mathrm{H}_{2}(g) $$ Calculate the enthalpy change $\Delta H^{\circ}$ for this reaction, using standard enthalpies of formation.

Hydrogen is prepared from natural gas (mainly methane, $\mathrm{CH}_{4}$ ) by partial oxidation.
$$
\mathrm{CH}_{4}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}(g)+2 \mathrm{H}_{2}(g)
$$
Calculate the enthalpy change $\Delta H^{\circ}$ for this reaction, using standard enthalpies of formation.

Key Concepts

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It ensures that the energy calculations correctly account for the number of moles of each substance reacting or forming, enabling accurate determination of the overall enthalpy change using standard enthalpy values.

Hess's Law

Hess's Law states that the total enthalpy change for a reaction is independent of the pathway by which the reaction occurs. It allows the calculation of reaction enthalpies by summing known enthalpy changes for related reaction steps, such as standard enthalpies of formation, regardless of the number of steps involved.

Enthalpy Change of Reaction

The enthalpy change of a reaction is the total heat absorbed or released during the process, calculated as the difference between the sum of the enthalpies of formation of the products and that of the reactants. This value indicates whether a reaction is exothermic (releases heat) or endothermic (absorbs heat).

Standard Enthalpy of Formation

This concept refers to the change in enthalpy when one mole of a compound is formed from its elements in their standard states under standard conditions (usually 1 atm pressure and 25°C). In thermochemical calculations, these values are used as fundamental building blocks to determine the overall energy change in a reaction.

Transcript

Please give Ace some feedback