Se hace pasar una mezcla de CH4 y H2 O sobre un catalizador de níquel a 1000 K. El gas saliente

step 1 Problem 71. In this problem, given that methane gas, react with H2O gas and it will form CO gas

Se hace pasar una mezcla de CH4 y H2 O sobre un catalizador...

Se hace pasar una mezcla de $\mathrm{CH}_4$ y $\mathrm{H}_2 \mathrm{O}$ sobre un catalizador de níquel a $1000 \mathrm{~K}$. El gas saliente se recoge en un matraz de $5.00 \mathrm{~L}$ y se encuentra que contiene $8.62 \mathrm{~g}$ de $\mathrm{CO}, 2.60 \mathrm{~g}$ de $\mathrm{H}_2, 43.0 \mathrm{~g}$ de $\mathrm{CH}_4$ y $48.4 \mathrm{~g}$ de $\mathrm{H}_2 \mathrm{O}$. Suponiendo que se ha alcanzado el equilibrio, calcule la $K_{\text {eq }}$ de la reacción.

Key Concepts

Mass-to-Mole Conversion

Mass-to-mole conversion is the process of converting a measured mass of a substance into moles using its molar mass. This conversion is a crucial step in stoichiometric calculations, as equilibrium expressions typically involve molar concentrations or pressures rather than masses.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to relate the amounts of reactants and products involved in a chemical reaction. It is critical in calculating the relationships between different species in the reaction, especially when converting measured quantities into moles and applying these ratios in equilibrium calculations.

Chemical Equilibrium

Chemical equilibrium refers to the state in which the concentrations of reactants and products remain constant over time because the forward and reverse reactions occur at the same rate. This concept is fundamental in understanding how reactions balance and how reaction conditions affect the amounts of substances present at equilibrium.

Equilibrium Constant

The equilibrium constant (K?q) is a numerical value that expresses the ratio of the concentrations (or partial pressures) of the products to the reactants, with each raised to the power of its stoichiometric coefficient. It quantifies the position of the equilibrium and helps predict the direction in which a reaction will proceed.

ICE Table Method

The ICE table (Initial, Change, Equilibrium) is a systematic way to organize the initial concentrations, the changes that occur as the system moves towards equilibrium, and the final concentrations at equilibrium. This method is essential for solving equilibrium problems by providing a clear visual framework to relate the reaction stoichiometry with concentration changes.

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