On the basis of the thermochemical equations H2 O(g)+C(s) ⟶CO(g) Δ=13 l kJ CO(g)+(1)/(2) O2( g)

step 1 On the basis of thermochemical equation, as written, you can see the equation. Delta H, which is

On the basis of the thermochemical equations H2 O(g)+C(s)...

On the basis of the thermochemical equations $\mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{C}(\mathrm{s}) \longrightarrow \mathrm{CO}(\mathrm{g}) \Delta \|=13 \mathrm{l} \mathrm{kJ}$ $\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CO}_{2}(\mathrm{~g}) \Delta H=282 \mathrm{~kJ}$ $\mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \Delta / I=-242 \mathrm{~kJ}$ $\mathrm{C}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CO}_{2}(\mathrm{~g}) \Delta / /=\mathrm{X} \mathrm{kJ}$ The valuc of $\mathrm{X}$ will be (1) $393 \mathrm{~kJ}$ (2) $655 \mathrm{~kJ}$ (3) $393 \mathrm{~kJ}$ (4) $655 \mathrm{~kJ}$

On the basis of the thermochemical equations $\mathrm{H}_{2} \mathrm{O}(\mathrm{g})+\mathrm{C}(\mathrm{s}) \longrightarrow \mathrm{CO}(\mathrm{g}) \Delta \|=13 \mathrm{l} \mathrm{kJ}$
$\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CO}_{2}(\mathrm{~g}) \Delta H=282 \mathrm{~kJ}$
$\mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \Delta / I=-242 \mathrm{~kJ}$
$\mathrm{C}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{~g}) \longrightarrow \mathrm{CO}_{2}(\mathrm{~g}) \Delta / /=\mathrm{X} \mathrm{kJ}$
The valuc of $\mathrm{X}$ will be
(1) $393 \mathrm{~kJ}$
(2) $655 \mathrm{~kJ}$
(3) $393 \mathrm{~kJ}$
(4) $655 \mathrm{~kJ}$

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Key Concepts

Thermochemical Equations

Thermochemical equations are balanced chemical equations that also include the enthalpy change (?H) associated with the reaction. They provide a way to represent not only the reactants and products in a reaction but also the energy absorbed or released, which is essential for understanding the thermodynamics of the reaction.

Hess's Law

Hess's Law is a principle in thermochemistry stating that the total enthalpy change of a chemical reaction is independent of the pathway taken. It means that if a reaction can be expressed as a series of steps, the sum of the enthalpy changes for each step will equal the enthalpy change for the overall reaction, allowing calculation of unknown enthalpy changes from known ones.

Enthalpy Change

Enthalpy change (?H) represents the heat content change in a reaction at constant pressure. It indicates whether a reaction is exothermic (releases heat) or endothermic (absorbs heat) and is a key parameter in determining the energy profile of chemical processes. Understanding ?H is vital for analyzing reaction energetics and energy balance.

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