The equilibrium constant for the gaseous reaction H2+I2 ⇋2 HI at a temperature of 720 kelvin is

step 1 We're given a reaction with all gaseous species. And we're given that the equilibrium constant f

The equilibrium constant for the gaseous reaction H2+I2 ⇋2...

The equilibrium constant for the gaseous reaction $$ \mathrm{H}_2+\mathrm{I}_2 \leftrightharpoons 2 \mathrm{HI} $$ at a temperature of 720 kelvin is $K=46.8$. A flask initially containing only $\mathrm{HI}$ is prepared and maintained at 720 kelvin. What is the concentration of $\mathrm{HI}$ in the flask when chemical equilibrium is attained? [Ans. $77 \%$ by volume]

The equilibrium constant for the gaseous reaction
$$
\mathrm{H}_2+\mathrm{I}_2 \leftrightharpoons 2 \mathrm{HI}
$$
at a temperature of 720 kelvin is $K=46.8$. A flask initially containing only $\mathrm{HI}$ is prepared and maintained at 720 kelvin. What is the concentration of $\mathrm{HI}$ in the flask when chemical equilibrium is attained? [Ans. $77 \%$ by volume]

Key Concepts

Chemical Equilibrium

Chemical equilibrium is the state in a reversible reaction where the rates of the forward and reverse reactions become equal, leading to constant concentrations of all species over time. This concept is fundamental in understanding how reactions settle into a stable configuration where observable changes cease, even though the individual molecular processes continue to occur.

Equilibrium Constant

The equilibrium constant (K) is a dimensionless value that quantifies the ratio of the concentrations (or partial pressures) of products to reactants at equilibrium, each raised to the power of their stoichiometric coefficients. It provides insight into the position of equilibrium, indicating whether a reaction favors products or reactants under a given set of conditions.

Reaction Quotient

The reaction quotient (Q) is calculated in the same way as the equilibrium constant but using the initial or non-equilibrium concentrations of reactants and products. Comparing Q to K helps determine the direction in which a reaction will proceed to reach equilibrium.

Stoichiometry in Equilibrium Reactions

Stoichiometry in equilibrium reactions involves using the balanced chemical equation to relate the changes in proportions of reactants and products as the system moves toward equilibrium. This concept is crucial for setting up relationships between species concentrations and for solving equilibrium problems accurately.

ICE Tables

ICE tables (Initial, Change, Equilibrium) are a systematic method used to organize and compute the concentrations of reactants and products as a reaction approaches equilibrium. They help clearly outline the initial amounts, the changes that occur during the reaction, and the final equilibrium concentrations, making complex equilibrium problems more manageable.

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