this system has an equilibrium constant of 50.5 at 448°c: h₂(g) + i₂(g) → 2hi(g). what is the reaction…

this system has an equilibrium constant of 50.5 at 448°c: h₂(g) + i₂(g) → 2hi(g). what is the reaction quotient, q, for this system when h₂=0.200 m, i₂=0.100 m, and hi=3.00 m? how does q compare to k_eq? q > k_eq q < k_eq q = k_eq

this system has an equilibrium constant of 50.5 at 448°c: h₂(g) + i₂(g) → 2hi(g). what is the reaction quotient, q, for this system when h₂=0.200 m, i₂=0.100 m, and hi=3.00 m? how does q compare to k_eq? q > k_eq q < k_eq q = k_eq

Answer

Explanation:

Step1: Write reaction - quotient formula

The reaction quotient $Q$ for the reaction $H_2(g)+I_2(g)\rightleftharpoons 2HI(g)$ is given by $Q = \frac{[HI]^2}{[H_2][I_2]}$.

Step2: Substitute given concentrations

Substitute $[H_2]=0.200\ M$, $[I_2]=0.100\ M$, and $[HI]=3.00\ M$ into the formula: $Q=\frac{(3.00)^2}{0.200\times0.100}=\frac{9.00}{0.0200}=450$.

Step3: Compare $Q$ and $K_{eq}$

Given $K_{eq} = 50.5$. Since $450>50.5$, we have $Q > K_{eq}$.

Answer:

The reaction - quotient $Q = 450$ and $Q>K_{eq}$