Dans un réacteur de 300 ml, on a introduit à 18 ^∘ C et sous une pression de 1 bar, 80 mL de mé

step 1 The number of moles of CH4 and O2 in the tank are N of CH4 equals M of CH4 over M of CH4 equals

Dans un réacteur de 300 ml, on a introduit à 18 ^∘ C et sous...

Dans un réacteur de $300 \mathrm{ml}$, on a introduit à $18{ }^{\circ} \mathrm{C}$ et sous une pression de 1 bar, $80 \mathrm{~mL}$ de méthane et $220 \mathrm{~mL}$ de dioxygène. On provoque par une étincelle la combustion du méthane $\left(\mathrm{CH}_4+2 \mathrm{O}_2=\mathrm{CO}_2+2 \mathrm{H}_2 \mathrm{O}\right)$, puis on laisse le réacteur se refroidir jusqu'à sa température initiale. Quelle est la pression à l'intérieur à cette température ?

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Key Concepts

Stoichiometry

This concept involves using the balanced chemical equation to determine the mole relationships between reactants and products. It is essential for identifying which reactant limits the reaction and for calculating the amounts of products produced from given initial quantities.

Ideal Gas Law

The ideal gas law describes the relationship between pressure, volume, temperature, and the number of moles of gas. It is used to predict how changes in the amount of gas (due to a reaction) impact the pressure in a closed container when the temperature and volume are held constant.

Limiting Reagent

The limiting reagent is the reactant that is completely consumed in a reaction, thereby governing the maximum amount of product that can be formed. Recognizing the limiting reagent is crucial for accurately determining the outcome of gas reactions.

Phase Changes

Considering phase changes is important in reactions involving gases because some products, such as water, may condense when cooled. This condensation removes the substance from the gaseous phase, significantly affecting the final pressure inside the reactor.

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