O hidrogénio eo dióxido de carbono reagem a alta temperatura...

O hidrogénio eo dióxido de carbono reagem a alta temperatura para dar água e monóxido de carbono. $$ \mathrm{H}_2(\mathrm{~g})+\mathrm{CO}_2(\mathrm{~g}) \rightleftarrows \mathrm{H}_2 \mathrm{O}(\mathrm{g})+\mathrm{CO}(\mathrm{g}) $$ (a) Experiências em laboratório, a $986^{\circ} \mathrm{C}$, mostram que, no equiIfbrio, num balão de $1,0 \mathrm{~L}$. existem 0,11 mol de $\mathrm{CO}, 0,11 \mathrm{~mol}$ de vapor de água, 0,087 mol de $\mathrm{H}_2$ e 0,087 mol de $\mathrm{CO}_2$. Calcule a constante de equilibrio da reação a $986^{\circ} \mathrm{C}$. (b) Se houver 0.050 mol de $\mathrm{H}_2$ e outro tanto de $\mathrm{CO}_2$ num vaso de $2,0 \mathrm{~L}$, em equilibrio a $986^{\circ} \mathrm{C}$, quantos moles de $\mathrm{CO}(\mathrm{g})$ e de $\mathrm{H}_2 \mathrm{O}(\mathrm{g})$ estarão presentes?

O hidrogénio eo dióxido de carbono reagem a alta temperatura para dar água e monóxido de carbono.
$$
\mathrm{H}_2(\mathrm{~g})+\mathrm{CO}_2(\mathrm{~g}) \rightleftarrows \mathrm{H}_2 \mathrm{O}(\mathrm{g})+\mathrm{CO}(\mathrm{g})
$$
(a) Experiências em laboratório, a $986^{\circ} \mathrm{C}$, mostram que, no equiIfbrio, num balão de $1,0 \mathrm{~L}$. existem 0,11 mol de $\mathrm{CO}, 0,11 \mathrm{~mol}$ de vapor de água, 0,087 mol de $\mathrm{H}_2$ e 0,087 mol de $\mathrm{CO}_2$. Calcule a constante de equilibrio da reação a $986^{\circ} \mathrm{C}$.
(b) Se houver 0.050 mol de $\mathrm{H}_2$ e outro tanto de $\mathrm{CO}_2$ num vaso de $2,0 \mathrm{~L}$, em equilibrio a $986^{\circ} \mathrm{C}$, quantos moles de $\mathrm{CO}(\mathrm{g})$ e de $\mathrm{H}_2 \mathrm{O}(\mathrm{g})$ estarão presentes?

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the rates of the forward and reverse reactions are equal, resulting in no net change in the concentrations of reactants and products over time. This fundamental concept is central to understanding how reactions behave under various conditions and is critical in the calculation and application of equilibrium constants.

Equilibrium Constant Expression (K)

The equilibrium constant is a dimensionless quantity that expresses the ratio of the concentrations (or pressures for gases) of products to reactants at equilibrium, each raised to the power of their stoichiometric coefficients. It provides a measure of the extent to which a reaction proceeds and is essential for predicting the composition of a reaction mixture at equilibrium.

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between the amounts of reactants and products in a chemical reaction. This concept is critical for determining how many moles of each substance participate in the reaction and is directly used in setting up and solving equilibrium problems, often through mole ratio relationships.

ICE Table Method

The ICE (Initial, Change, Equilibrium) table is a systematic tool used to organize and calculate the concentrations or moles of reactants and products in a chemical reaction as it proceeds to equilibrium. This method helps in visualizing the changes that occur from the start of the reaction to the point where equilibrium is established, making it easier to set up the equilibrium constant expression and solve for unknowns.

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