Question

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question 11 (1 point)
the variable, ( q_{eq} ), represents which of these?

• the equilibrium constant using partial pressure
• the equilibrium constant using concentration
• the reaction quotient using partial pressure
• the reaction quotient using concentration
• the equilibrium constant using partial pressure and concentration

question 12 (1 point)
if ( q_{eq} > k_{eq} ), then ------

• the system is at equilibrium
• the ratio of products to reactants is less than ( k_{eq} )
• the ratio of products to reactants is greater than ( k_{eq} )
• the reaction shifts toward product formation
• more reactants must be consumed to reach equilibrium

question 13 (1 point)

Explanation:

Question 11

The reaction quotient \( Q \) (or \( Q_{eq} \), but here \( Q_{aq} \) likely has a typo or is \( Q_c \)) using concentration is for concentrations of reactants and products at any time, while equilibrium constants (\( K_p \), \( K_c \)) are at equilibrium. \( Q_p \) is reaction quotient with partial pressures. So \( Q_{aq} \) (assuming \( Q_c \)) is reaction quotient using concentration.

When \( Q_{eq} > K_{eq} \) (or \( Q > K \)), the reaction has more products (or higher ratio of products to reactants) than at equilibrium. So the ratio of products to reactants is greater than \( K_{eq} \), and the reaction shifts left (toward reactants), not products. The system isn't at equilibrium. "more reactants must be consumed" is wrong (it's products consumed). So the correct logic is \( Q > K \) means product/reactant ratio (from \( Q \)) is greater than \( K \).

Answer:

the reaction quotient using concentration

Question 12