The heat cvolved during the combustion of 112 litre of water...

The heat cvolved during the combustion of 112 litre of water gas (mixture of equal volumes of $\mathrm{II}_{2}$ and $(\mathrm{CO})$ is (i) $\mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) ; \Delta / l=-241.8 \mathrm{k} \mathrm{J}$ (ii) $\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g}) ; \Delta H=283 \mathrm{~kJ}$ (1) $241.8 \mathrm{~kJ}$ (2) $283.3 \mathrm{~kJ}$ (3) $1312 \mathrm{~kJ}$ (4) $1586 \mathrm{~kJ}$

The heat cvolved during the combustion of 112 litre of water gas (mixture of equal volumes of $\mathrm{II}_{2}$ and $(\mathrm{CO})$ is
(i) $\mathrm{H}_{2}(\mathrm{~g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) ; \Delta / l=-241.8 \mathrm{k} \mathrm{J}$
(ii) $\mathrm{CO}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g}) \rightarrow \mathrm{CO}_{2}(\mathrm{~g}) ; \Delta H=283 \mathrm{~kJ}$
(1) $241.8 \mathrm{~kJ}$
(2) $283.3 \mathrm{~kJ}$
(3) $1312 \mathrm{~kJ}$
(4) $1586 \mathrm{~kJ}$

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Key Concepts

Combustion Reaction

This concept involves the oxidation of a substance (fuel) in the presence of oxygen to produce combustion products (such as water and carbon dioxide) along with the release of energy. The process is exothermic, meaning it releases heat, and understanding the reaction’s stoichiometry is critical to calculating the overall energy change in the reaction.

Reaction Enthalpy

Reaction enthalpy (?H) is the measure of the total heat absorbed or released during a chemical reaction at constant pressure. It is expressed on a per mole basis and can be summed for multiple reactions to compute the total heat change involved in a process such as complete combustion.

Gas Stoichiometry

Gas stoichiometry uses the concept of equal volumes of gases corresponding to equal numbers of moles under the same conditions of temperature and pressure, according to Avogadro’s law. This principle is essential when calculating the amounts of reactants and products in gaseous reactions, thereby allowing the determination of energy changes for a given volume of a gas mixture.

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