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

step 1 explanation for the osculture here we have given chemical reaction so here chemical reaction is

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 $\mathrm{C}_{6} \mathrm{H}_{6}(\mathrm{~g})$. The total pressure of the mixture of gases is then $3.9 \mathrm{kPa}$. Assume the volume and the temperature do not change. What fraction of $\mathrm{C}_{2} \mathrm{H}_{2}(g)$ has undergone reaction?

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Key Concepts

Ideal Gas Law

The ideal gas law relates the pressure, volume, temperature, and number of moles of a gas. When temperature and volume are constant, the pressure of a gas is directly proportional to the number of moles. This principle allows us to interpret changes in pressure as changes in the number of gas molecules, which is particularly useful when analyzing reactions involving gases.

Reaction Stoichiometry

Reaction stoichiometry involves using the balanced chemical equation to relate the amounts (in moles) of reactants and products. The mole ratios provided by the coefficients in the chemical equation allow for the determination of how much product is formed from a given amount of reactant, and how the consumption of reactants affects the overall quantity of gas present.

Extent of Reaction Calculation

The extent of reaction, or percent conversion, is a measure of how much of a reactant has been converted into products. By comparing the initial and final amounts (or pressures) of gases and applying the stoichiometric relationships, one can calculate the fraction or percentage of the reactant that has undergone reaction. This concept is key to analyzing reactions where the change in the number of moles directly affects observable properties like pressure.

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