Consider the following equilibrium:
C₂H₆(g) + C₅H₁₂(g)
CH₄(g) + C₆H₁₄(g) ; K_p = 9.57 at 500 K
Suppose 11.6 g each of CH₄,C₂H₆,C₅H₁₂,and C₆H₁₄ are placed in a 30.0-L reaction vessel at 500 K.Which of the following statements is correct?

Question

Consider the following equilibrium:
C₂H₆(g) + C₅H₁₂(g)

Consider the following equilibrium: C<sub>2</sub>H<sub>6</sub>(g) + C<sub>5</sub>H<sub>12</sub>(g) CH<sub>4</sub>(g) + C<sub>6</sub>H<sub>14</sub>(g) ; K<sub>p</sub> = 9.57 at 500 K Suppose 11.6 g each of CH<sub>4</sub>,C<sub>2</sub>H<sub>6</sub>,C<sub>5</sub>H<sub>12</sub>,and C<sub>6</sub>H<sub>14</sub> are placed in a 30.0-L reaction vessel at 500 K.Which of the following statements is correct? A) Because Q<sub>c</sub> < K<sub>c</sub>,more products will be formed. B) Because Q<sub>c</sub> = 1,the system is at equilibrium. C) Because Q<sub>c</sub> = 1,more products will be formed. D) Because Q<sub>c</sub> = 1,more reactants will be formed. E) Because Q<sub>c</sub> > K<sub>c</sub>,more reactants will be formed.

CH₄(g) + C₆H₁₄(g) ; K_p = 9.57 at 500 K
Suppose 11.6 g each of CH₄,C₂H₆,C₅H₁₂,and C₆H₁₄ are placed in a 30.0-L reaction vessel at 500 K.Which of the following statements is correct?

Quizplus · Accepted Answer

Since the equilibrium constant, K, is greater than 1 (K=9.57), we know that the products are favored at equilibrium. Initially, there are equal amounts of reactants and products. Therefore, the reaction will proceed in the forward direction to reach equilibrium, producing more products. This is also supported by the fact that the reaction quotient, Q, is less than the equilibrium constant (Q<K). Therefore, choice A is the correct answer.

Consider the Following Equilibrium