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Reaction Quotients

This worksheet covers Reaction Quotients, 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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Reaction Quotients

Equilibrium • Chemistry

Set 4 — Mastery

For the reaction $aA + bB \rightleftharpoons cC + dD$ , the reaction quotient $Q_c$ is defined as which of the following?

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

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

$Q_c = [C]^c + [D]^d$

$Q_c = [A]^a + [B]^b$

If the reaction $2NO(g) + O_{2}(g) \rightleftharpoons 2NO_{2}(g)$ is at equilibrium and $Q_c = 0.5$ , what can be inferred about the system?

The reaction will shift to the right.

The reaction will shift to the left.

The system is at equilibrium.

The reaction is not favored in either direction.

For the reaction $N_{2}(g) + 3H_{2}(g) \rightleftharpoons 2NH_{3}(g)$ , if the concentrations are $[N_{2}] = 0.1$ , $[H_{2}] = 0.3$ , and $[NH_{3}] = 0.4$ , what is the value of $Q_c$ ?

$Q_c = 1.2$

$Q_c = 0.5$

$Q_c = 0.03$

$Q_c = 0.1$

Which of the following statements is true regarding the reaction quotient $Q_p$ ?

$Q_p$ is the same as $Q_c$ for gaseous reactions.

$Q_p$ uses partial pressures instead of concentrations.

$Q_p$ is always equal to 1 at equilibrium.

$Q_p$ is independent of temperature.

Consider the reaction $A(g) \rightleftharpoons B(g) + C(g)$ . If $Q_c < K_c$ , what does this imply about the concentrations of $A$ , $B$ , and $C$ ?

$[A]$ is high and $[B], [C]$ are low.

$[A]$ , $[B]$ , and $[C]$ are all equal.

$[A]$ is low and $[B], [C]$ are high.

$[A]$ is low and $[B]$ , $[C]$ are low.

In the reaction $aA + bB \rightleftharpoons cC + dD$ , if $Q_c = K_c$ , which statement is correct?

The reaction is at equilibrium.

The reaction favors the formation of products.

The reaction favors the formation of reactants.

The forward reaction is faster than the reverse reaction.

For the endothermic reaction $A + B \rightleftharpoons C + D$ , what happens to $Q_c$ when temperature is increased?

$Q_c$ increases.

$Q_c$ decreases.

$Q_c$ remains unchanged.

$Q_c$ becomes zero.

When the volume of a gas-phase reaction is decreased, what is the effect on $Q_c$ for the reaction $2A(g) \rightleftharpoons B(g) + C(g)$ ?

$Q_c$ increases.

$Q_c$ decreases.

$Q_c$ remains unchanged.

$Q_c$ becomes undefined.

In the reaction $A + 2B \rightleftharpoons C + D$ , if $[C]$ increases, what will happen to $Q_c$ ?

$Q_c$ increases.

$Q_c$ decreases.

$Q_c$ remains the same.

$Q_c$ becomes undefined.

10.

For the reaction $2H_{2}(g) + O_{2}(g) \rightleftharpoons 2H_{2}O(g)$ , if $Q_c = 4$ and $K_c = 25$ , what does this indicate about the system?

The reaction favors products.

The reaction favors reactants.

The system is at equilibrium.

The reaction will shift to the left.

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