10.4.1: Practice Equilibrium Constants

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Exercise \(\PageIndex{1}\)

\[3 H_{2 (g)} + N_{2 (g)} \longleftrightarrow 2 NH_{3 (g)}\]

What is the equilibrium constant expression of the reaction above?

Answer: \(K_{eq} = \dfrac{[NH_{3}]^{2}}{[H_{2}]^{3}[N_{2}]}\)

Exercise \(\PageIndex{1}\)

\[2 SO_{2 (g)} + O_{2 (g)} \longleftrightarrow 2 SO_{3 (g)}\]

The K_eq of the reaction above is 3.4 x 10². Is the equilibrium mixture mostly SO₂ and O₂ or mostly SO₃?

Answer: mostly SO₃

Exercise \(\PageIndex{1}\)

\[C_{(s)} + 2 S_{(g)} \longleftrightarrow CS_{2 (g)}\]

What is the equilibrium constant expression of the reaction above?

Answer: \(K_{eq} = \dfrac{[CS_{2}]}{[S]^{2}}\)

Exercise \(\PageIndex{1}\)

\[Pb^{2+}_{(aq)} + 2 Cl^{1–}_{(aq)} \longleftrightarrow PbCl_{2 (s)}\]

What is the equilibrium constant expression of the reaction above?

Answer: \(K_{eq} = \dfrac{1}{[Pb^{2+}][Cl^{1–}]^{2}}\)