Ammonia is added to a gaseous reaction mixture containing H2, Cl2, and HCl that is at chemical e

step 1 We start with equation 2, HCL gas plus NH3 gas will produce an H4 CL solid. And if we increase t

Ammonia is added to a gaseous reaction mixture containing...

Ammonia is added to a gaseous reaction mixture containing $\mathrm{H}_{2}, \mathrm{Cl}_{2},$ and $\mathrm{HCl}$ that is at chemical equilibrium. How will the addition of ammonia affect the relative concentrations of $\mathrm{H}_{2}, \mathrm{Cl}_{2},$ and $\mathrm{HCl}$ if the equilibrium constant of reaction 2 is much greater than the equilibrium constant of reaction $1 ?$ (1) $\quad \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{HCl}(g)$ (2) $\quad \mathrm{HCl}(g)+\mathrm{NH}_{3}(g) \rightleftharpoons \mathrm{NH}_{4} \mathrm{Cl}(s)$

Ammonia is added to a gaseous reaction mixture containing $\mathrm{H}_{2}, \mathrm{Cl}_{2},$ and $\mathrm{HCl}$ that is at chemical equilibrium. How will the addition of ammonia affect the relative concentrations of $\mathrm{H}_{2}, \mathrm{Cl}_{2},$ and $\mathrm{HCl}$ if the equilibrium constant of reaction 2 is much greater than the equilibrium constant of reaction $1 ?$
(1) $\quad \mathrm{H}_{2}(g)+\mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{HCl}(g)$
(2) $\quad \mathrm{HCl}(g)+\mathrm{NH}_{3}(g) \rightleftharpoons \mathrm{NH}_{4} \mathrm{Cl}(s)$

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Key Concepts

Chemical Equilibrium

This concept refers to the state in a reversible reaction where the rate of the forward reaction equals that of the reverse reaction, resulting in constant concentrations of reactants and products over time. It is a dynamic balance that can be disturbed by changes in concentration, pressure, or temperature.

Le Chatelier's Principle

Le Chatelier's principle predicts how a system at equilibrium will respond to disturbances. When a change is imposed on a system, the equilibrium shifts in a direction that tends to reduce the effect of the change, such as by consuming an added reactant or product.

Coupled Equilibria

Coupled equilibria occur when two or more reactions share common species, such that a change in one equilibrium can affect the other. Removing or adding a species in one reaction can shift the equilibrium positions of both coupled reactions.

Equilibrium Constant

The equilibrium constant quantifies the ratio of product concentrations to reactant concentrations at equilibrium, each raised to the power of their stoichiometric coefficients. It provides insight into the position of equilibrium and how the system will respond to changes, particularly when one reaction has a much larger constant than the other.

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