At 500^∘ C, K for the formation of ammonia from nitrogen and...

At $500^{\circ} \mathrm{C}, K$ for the formation of ammonia from nitrogen and hydrogen gases is $1.5 \times 10^{-5}$. $$ \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) $$ Calculate the equilibrium partial pressure of hydrogen if the equilibrium partial pressures of ammonia and nitrogen are $0.015 \mathrm{~atm}$ and $1.2 \mathrm{~atm}$, respectively. 35. At a certain temperature, $K$ is 4.9 for the formation of one mole of bromine chloride gas (BrCl) from its elements. A mixture at equilibrium at this temperature contains all three gases. The partial pressures at equilibrium of bromine and chlorine gas is $0.19 \mathrm{~atm}$. What is the partial pressure of bromine chloride in this mixture at equilibrium?

At $500^{\circ} \mathrm{C}, K$ for the formation of ammonia from nitrogen and hydrogen gases is $1.5 \times 10^{-5}$.
$$
\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)
$$
Calculate the equilibrium partial pressure of hydrogen if the equilibrium partial pressures of ammonia and nitrogen are $0.015 \mathrm{~atm}$ and $1.2 \mathrm{~atm}$, respectively.
35. At a certain temperature, $K$ is 4.9 for the formation of one mole of bromine chloride gas (BrCl) from its elements. A mixture at equilibrium at this temperature contains all three gases. The partial pressures at equilibrium of bromine and chlorine gas is $0.19 \mathrm{~atm}$. What is the partial pressure of bromine chloride in this mixture at equilibrium?

Key Concepts

Chemical Equilibrium

Chemical equilibrium occurs when the rate of the forward reaction equals the rate of the reverse reaction. At this point, the concentrations (or partial pressures in gas systems) of all reactants and products remain constant over time, even though both reactions continue to occur. This concept is fundamental in understanding how reactions behave in closed systems.

Equilibrium Constant (Kp)

The equilibrium constant for gas-phase reactions, denoted as Kp, is defined as the ratio of the product of the partial pressures of the products to that of the reactants, each raised to the power of their stoichiometric coefficients. It quantifies the position of equilibrium and is temperature-dependent. Kp serves as a tool to predict the direction of the reaction and to calculate unknown partial pressures when the system is at equilibrium.

Partial Pressure

Partial pressure refers to the pressure that an individual gas in a mixture would exert if it occupied the entire volume by itself at the same temperature. It is used in the context of gas mixtures to apply the principles of the ideal gas law to each component separately. In chemical equilibrium problems involving gases, knowing the partial pressures of species is essential for setting up and solving the equilibrium expression.

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between reactants and products as dictated by the balanced chemical equation. In equilibrium problems, stoichiometry determines the exponents in the equilibrium constant expression and directly affects the calculations needed to find unknown quantities. It ensures that the conservation of mass is maintained throughout the reaction process.

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