Learning Goal: To use the equilibrium constant and Le Châtelier's principle to determine how a reaction will respond to external

Question

Learning Goal:
To use the equilibrium constant and Le Châtelier's
principle to determine how a reaction will respond
to external factors.
A reaction is at equilibrium when the concentrations
of the reactants and products no longer change
over time. This does not mean the reaction is over;
rather, two competing reactions continue to occur
simultaneously at equal rates. The two competing
reactions are the forward reaction (reactants →
products) and the reverse reaction (products →→
reactants).
If a reaction at equilibrium is subjected to a stress,
the concentrations of reactants and products adjust
to reestablish equilibrium. This is called Le
Châtelier's principle. A stress might be a change in
the concentration of reactants or products, a
change in the volume of the reaction container, a
change in temperature, or the addition of a catalyst.
Given the concentrations, calculate the equilibrium constant for this reaction:
PC13 (g) +Cl₂ (g) = PCL5 (g)
At equilibrium, the molar concentrations for reactants and products are found to be [PC13] = 0.20 M, [Cl₂] = 0.25 M,
and [PC15] 1.20 M. What is the equilibrium constant (Kc) for this reaction?
Express your answer using two significant figures.
► View Available Hint(s)
K = 24
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Part B
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Previous Answers
[PC15]
[PC13][Cl₂]
The concentration of PC13 (g) is increased to 1.2 M, disrupting equilibrium. Calculate the new ratio of products to
reactants with this higher concentration of phosphorus trichloride. Assume that the reaction has not yet regained
equilibrium.
Express your answer using two significant figures.
► View Available Hint(s)
=
Review | Constants | Periodic Table
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Kunduz · Accepted Answer

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