At some temperature, the reaction N2( g)+3 H2( g) ⇌2 NH3( g) has an equilibrium constant Kc nume

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At some temperature, the reaction N2( g)+3 H2( g) ⇌2 NH3( g)...

At some temperature, the reaction $$\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})$$ has an equilibrium constant $K_{\mathrm{c}}$ numerically equal to 1 . State whether each of the following is true or false, and explain why. (a) An equilibrium mixture must have the $\mathrm{H}_{2}$ concentration three times that of $\mathrm{N}_{2}$ and the $\mathrm{NH}_{3}$ concentration twice that of $\mathrm{H}_{2}$. (b) An equilibrium mixture must have the $\mathrm{H}_{2}$ concentration three times that of $\mathrm{N}_{2}$. (c) A mixture in which the $\mathrm{H}_{2}$ concentration is three times that of $\mathrm{N}_{2}$ and the $\mathrm{NH}_{3}$ concentration is twice that of $\mathrm{N}_{2}$ could be an equilibrium mixture. (d) A mixture in which the concentration of each reactant and each product is $1 M$ is an equilibrium mixture. (e) Any mixture in which the concentrations of all reactants and products are equal is an equilibrium mixture. (f) An equilibrium mixture must have equal concentrations of all reactants and products.

At some temperature, the reaction
$$\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_{3}(\mathrm{~g})$$
has an equilibrium constant $K_{\mathrm{c}}$ numerically equal to 1 . State whether each of the following is true or false, and explain why. (a) An equilibrium mixture must have the $\mathrm{H}_{2}$ concentration three times that of $\mathrm{N}_{2}$ and the $\mathrm{NH}_{3}$ concentration twice that of $\mathrm{H}_{2}$. (b) An equilibrium mixture must have the $\mathrm{H}_{2}$ concentration three times that of $\mathrm{N}_{2}$. (c) A mixture in which the $\mathrm{H}_{2}$ concentration is three times that of $\mathrm{N}_{2}$ and the $\mathrm{NH}_{3}$ concentration is twice that of $\mathrm{N}_{2}$ could be an equilibrium mixture.
(d) A mixture in which the concentration of each reactant and each product is $1 M$ is an equilibrium mixture. (e) Any mixture in which the concentrations of all reactants and products are equal is an equilibrium mixture. (f) An equilibrium mixture must have equal concentrations of all reactants and products.

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, leading to constant concentrations of reactants and products. This concept is crucial for understanding how mixtures can have multiple sets of concentrations that satisfy the equilibrium condition, independent of the initial stoichiometric ratios given by the balanced equation.

Equilibrium Constant Expression

The equilibrium constant expression (Kc) relates the concentrations of the products and reactants at equilibrium according to their stoichiometric coefficients. It provides a quantitative measure of the position of equilibrium and is used to determine whether a given set of concentrations corresponds to an equilibrium state. It is important to note that the expression does not require the concentration ratios to directly reflect the stoichiometry of the balanced chemical equation.

Reaction Stoichiometry

Reaction stoichiometry involves the coefficients from a balanced chemical equation, which indicate the proportions in which reactants combine and products form. While the stoichiometric coefficients are used in the equilibrium constant expression, they do not dictate the actual concentrations at equilibrium; rather, they determine how the concentrations relate to each other when substituted into the equilibrium expression.

Reaction Quotient

The reaction quotient (Q) is calculated using the same form as the equilibrium constant expression but using initial or non-equilibrium concentrations. Comparing Q to Kc indicates the direction in which a reaction will shift to reach equilibrium. This concept is essential to understand that different sets of concentrations can eventually adjust to satisfy the equilibrium constant, even if they initially do not match simple stoichiometric ratios.

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