A 1.0 mol sample of X(g) and a 1.0 mol sample of Q(g) are introduced into an evacuated, rigid 10.0 L container and allowed to re

Question

14 days ago

11

A 1.0 mol sample of X(g) and a 1.0 mol sample of Q(g) are introduced into an evacuated, rigid 10.0 L container and allowed to re

ach equilibrium at 50ºC according to the equation above. At equilibrium, which of the following is true about the concentrations of the gases?
X(g) + 2 Q(g) --> R(g) + Z(g)

Kc = 1.3 x 105 at 50ºC

[R] = ½ [Q]
[X] = [Q] = [R] = [Z]
[Q] = ½ [X]
[R] = [Z] > Q

Chemistry

2 answers:

castortr0y [2.9K] · Answer 1 · 2026-03-25T00:49:09+03:00

At equilibrium, [R] = [Z] > [Q]. Explanation: In analyzing the equilibrium conditions, the provided reaction of X(g) + 2 Q(g) ⇄ R(g) + Z(g) establishes that at a temperature of 50ºC, the equilibrium constant Kc = 1.3 x 105. This indicates a scenario where the concentrations of the products greatly exceed those of the reactants.

eduard [2.6K] · Answer 2 · 2026-03-25T00:50:12+03:00

At equilibrium, the valid statement is [R] = [Z] > [Q]. Explanation: Given the initial quantities of 1.0 moles each for X and Q within a 10.0 L chamber, the calculations yield molarities that show the concentration of products at equilibrium—indicating that [R] and [Z] surpass [Q].