On réalise la réaction dont l'équation stœchiométrique s'écrit : PH3( g)=P(s)+3 / 2 H2( g) à vol

step 1 derive the KP expression here, products of a reactants. This would be the partial pressure of p2

On réalise la réaction dont l'équation stœchiométrique...

On réalise la réaction dont l'équation stœchiométrique s'écrit : $$ \mathrm{PH}_3(\mathrm{~g})=\mathrm{P}(\mathrm{s})+3 / 2 \mathrm{H}_2(\mathrm{~g}) $$ à volume constant et température constante, sous une pression initiale $p_0$. Quelle est l'expression littérale de la pression partielle du dihydrogène en fonction de la pression initiale $p_0$ et de la pression totale $p$ à chaque instant de la réaction?

On réalise la réaction dont l'équation stœchiométrique s'écrit :
$$
\mathrm{PH}_3(\mathrm{~g})=\mathrm{P}(\mathrm{s})+3 / 2 \mathrm{H}_2(\mathrm{~g})
$$
à volume constant et température constante, sous une pression initiale $p_0$. Quelle est l'expression littérale de la pression partielle du dihydrogène en fonction de la pression initiale $p_0$ et de la pression totale $p$ à chaque instant de la réaction?

Key Concepts

Partial Pressure

Partial pressure refers to the pressure exerted by a single gas component in a mixture and is directly proportional to its mole fraction in the mixture. When a chemical reaction produces or consumes a gaseous species, calculating its partial pressure is essential since it reflects the change in the number of moles of that particular gas in the mixture.

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. The stoichiometric coefficients, given in the balanced reaction, allow one to relate the change in the amount (or pressure, in the case of gases under constant conditions) of one species to the change in another, making it a key tool for analyzing reaction progress.

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, links the pressure, volume, temperature, and number of moles of a gas. In a reaction occurring at constant volume and temperature, changes in the number of moles of a gaseous species directly translate into changes in its pressure. This principle is used to relate variations in partial and total pressures throughout the reaction.

Reaction Extent (Progress of Reaction)

The extent of reaction quantifies how far a chemical reaction has proceeded. By introducing a variable (often denoted as x) to represent the change in the moles—or correspondingly, the pressure decrement or increment—of the reacting species, one can express the partial pressures of products and reactants in terms of the initial conditions and the progress of the reaction.

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