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Equilibrium: Constant

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Wize High School Grade 12 Chemistry Textbook > Equilibrium

The Equilibrium Constant (K)

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At 25 ˚C, KP = 5.2 × 10–2 for the following decomposition reaction:

NH4HS(s)⇌NH3(g)+H2S(g)NH_4HS (s) ⇌ NH_3 (g) + H_2S (g)

(a) Calculate the equilibrium partial pressures of ammonia (NH3) and hydrogen sulfide (H2S) if a sample of solid NH4HS is placed in a closed vessel initially containing 11 atm of NH3 gas. Note that the vessel still contains some solid NH4HS at equilibrium. State and justify any assumptions you might make during your calculation.

(b) Does the mass of NH4HS (s) in the vessel increase / decrease / stay the same ? Circle one.
More The Equilibrium Constant (K) Questions:
Equilibrium constant
For the following equilibria determine whether K>1K > 1, K<1K < 1 or K≈1K \approx 1. Enter your answers as "Greater", "Less", "1" respectively.
A)
B)
Equilibrium: Reaction quotient
If the reaction A⇌BA⇌B has an equilibrium constant of K = 10–4, which one of the following statements is always true?
Equilibrium and Le Chatelier's Principle
At time = t0, 0.40 mol of Br2 (ℓ) and 0.40 mol of Cℓ2 (g) are placed in an empty, rigid 10.00 L flask and allowed to reach equilibrium.
After reaching equilibrium at time = t2, the flask is found to contain 0.20 mol of BrCℓ (g). The temperature is held constant throughout the reaction.
Equilibrium Constant
Balance each reaction and write its equilibrium constant expression
NO(g)+O2(g)↔N2O3(g)NO_{(g)}+O_{2(g)} \leftrightarrow N_2O_{3(g)}
SF6(g)+SO3(g)↔SO2F2(g)SF_{6(g)}+SO_{3(g)}\leftrightarrow SO_2F_{2(g)}
Le Chatelier's Principle: Equilibrium constant
Consider the following reaction:
PCℓ5(g)⇌PCℓ3(g)+Cℓ2(g)PCℓ_5 (g) ⇌ PCℓ_3 (g) + Cℓ_2 (g)
The measured equilibrium constant is 5.0x10–4 at 373 K and 0.20 at 473 K. Which of the following statements about the reaction must be true?
Equilibrium plots: Equilibrium constant
You mix three unknown compounds in a container: a solid (A), and two gases (E and X). You do not know the chemical formula of any of the compounds, but you are able to track the progress of the reaction by measuring changes in the concentrations of both gases, as shown in the graph below.
Which of these reactions and equilibrium constants could be represented by the data shown in this graph?