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Equilibrium Constant

This worksheet covers Equilibrium Constant, which is part of the Equilibrium module in the Chemistry course. Practice problems are designed to strengthen key concepts and build confidence.

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Equilibrium Constant

Equilibrium • Chemistry

Set 5 — Mastery

What is the expression for the equilibrium constant $K_c$ for the reaction $aA + bB \rightleftharpoons cC + dD$ ?

$K_c = \frac{[C]^c[D]^d}{[A]^a[B]^b}$

$K_c = \frac{[A]^a[B]^b}{[C]^c[D]^d}$

$K_c = \frac{[C]^c}{[A]^a}$

$K_c = [C][D]$

For the reaction $2SO_{2}(g) + O_{2}(g) \rightleftharpoons 2SO_{3}(g)$ , what is the correct expression for the equilibrium constant $K_p$ ?

$K_p = \frac{(P_{SO_{3}})^{2}}{(P_{SO_{2}})^{2}(P_{O_{2}})}$

$K_p = \frac{(P_{SO_{2}})^{2}(P_{O_{2}})}{(P_{SO_{3}})^{2}}$

$K_p = (P_{SO_{3}})^{2} \times (P_{O_{2}})$

$K_p = \frac{P_{SO_{3}}}{P_{O_{2}}}$

If $K_c = 10$ for the reaction $A \rightleftharpoons B$ , what is the relationship between the concentrations of $A$ and $B$ at equilibrium?

$[B] = 10[A]$

$[A] = 10[B]$

$[B] = \frac{1}{10}[A]$

$[A] = \frac{1}{10}[B]$

For the exothermic reaction $A + B \rightleftharpoons C + D$ , if the temperature is increased, how does $K_c$ change?

$K_c$ increases$

$K_c$ decreases$

$K_c$ remains constant$

$K_c$ can increase or decrease$

What is the value of the equilibrium constant $K_{sp}$ for the sparingly soluble salt $AgCl$ at equilibrium?

$K_{sp} = [Ag^{+}][Cl^{-}]$

$K_{sp} = [AgCl]$

$K_{sp} = [Ag^{+}] + [Cl^{-}]$

$K_{sp} = [Ag^{+}][Cl^{-}]^{2}$

For a reaction with a $K_c$ value of 0.02, which of the following statements is true?

The reaction favors the products.

The reaction favors the reactants.

The reaction is at equilibrium.

The reaction cannot proceed.

In the reaction $N_{2}(g) + 3H_{2}(g) \rightleftharpoons 2NH_{3}(g)$ , what is the expression for the equilibrium constant $K_c$ ?

$K_c = \frac{[NH_{3}]^{2}}{[N_{2}][H_{2}]^{3}}$

$K_c = \frac{[N_{2}][H_{2}]^{3}}{[NH_{3}]^{2}}$

$K_c = \frac{[NH_{3}]}{[H_{2}]}$

$K_c = [NH_{3}]^{2}$

If the equilibrium constant $K_{eq}$ for the reaction $P + Q \rightleftharpoons R$ is 5, what happens if the concentration of $P$ is doubled?

The equilibrium constant remains the same.

The equilibrium constant increases.

The equilibrium constant decreases.

The reaction will favor the products.

For the reaction $2A \rightleftharpoons B + C$ , if $K_c = 4$ , what is the relation between $[B]$ and $[C]$ at equilibrium?

$[B] = 2[C]$

$[C] = 2[B]$

$[B] = [C]$

$[B] = \frac{1}{2}[C]$

10.

In a closed system at equilibrium, if the volume is increased, what happens to the equilibrium position for the reaction $N_{2}(g) + 3H_{2}(g) \rightleftharpoons 2NH_{3}(g)$ ?

The equilibrium shifts to the right.

The equilibrium shifts to the left.

The equilibrium remains unchanged.

The reaction proceeds to completion.

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