Equilibrium Constant

Equilibrium • Chemistry

Set 5 — Mastery

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

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

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

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

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

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

$K_{s p} = [A g^{+}] [C^{}$

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 ?

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

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

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