A sample of C2 H2(g) has a pressure of 7.8 kPa . After some time a portion of it reacts to form

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A sample of C2 H2(g) has a pressure of 7.8 kPa . After some...

A sample of $\mathrm{C}_{2} \mathrm{H}_{2}(g)$ has a pressure of 7.8 $\mathrm{kPa}$ . After some time a portion of it reacts to form $\mathrm{C}_{6} \mathrm{H}_{6}(g) .$ The total pressure of the mixture of gases is then 3.9 $\mathrm{kP}$ . Assume the volume and the temperature do not change. What fraction of $\mathrm{C}_{2} \mathrm{H}_{2}(g)$ has undergone reaction?

Key Concepts

Ideal Gas Law

The ideal gas law states that the pressure of a gas is directly proportional to the number of moles when the temperature and volume are held constant. This principle is crucial for interpreting how changes in pressure reflect changes in the number of gas moles, providing a bridge between measurable pressure changes and the extent of a chemical reaction.

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction according to a balanced chemical equation. Understanding stoichiometry allows one to relate the amount of reactant consumed to the amount of product formed, which is key when determining the fraction of a reactant that reacted based on changes in total moles.

Fractional Reaction Conversion

Fractional reaction conversion is the measure of the proportion of the initial reactant that has undergone reaction. By using the relationship between the initial and final moles (or pressures) deduced from the ideal gas law and stoichiometric ratios, one can calculate the fraction of the reactant that has been converted into products during the reaction.

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