Consider the general reaction belo X₂(g) + 2Y₂(g) = 2XY₂(g) K = 3.9 x 10-8 @ 298 K 0.50 M X2 and Y2 were added to a sea vessel. Calculate the equilibrium concentrations of the components. Wha the equilibrium concentration of XY2 ?] [XY₂] = [?] x 10 M

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**Chemical Equilibrium: Calculating Equilibrium Concentrations**

**Consider the general reaction below:**

\( \mathbf{X_2(g) + 2Y_2(g) \rightleftharpoons 2XY_2(g)} \)

**Given:**
- Equilibrium Constant, \( K = 3.9 \times 10^{-8} \) at \( 298 \, \text{K} \)

**Initial Conditions:**
- 0.50 M \( \mathbf{X_2} \) and 0.50 M \( \mathbf{Y_2} \) were added to a sealed vessel.

**Objective:**
Calculate the equilibrium concentrations of the components. What is the equilibrium concentration of \( \mathbf{XY_2} \)?

\[ [XY_2] = \boxed{?} \times 10^{\boxed{?}} \, \text{M} \]

**Steps to Solve:**
1. **Set up the ICE Table** (Initial, Change, Equilibrium) to find the equilibrium concentrations:
    - **Initial Concentrations:** 
      \[
      \begin{aligned}
      [X_2] &= 0.50 \, \text{M} \\
      [Y_2] &= 0.50 \, \text{M} \\
      [XY_2] &= 0 \, \text{M} 
      \end{aligned}
      \]
    - **Change in Concentrations:** 
      \[
      \begin{aligned}
      [X_2] &= -x \\
      [Y_2] &= -2x \\
      [XY_2] &= +2x 
      \end{aligned}
      \]
    - **Equilibrium Concentrations:**
      \[
      \begin{aligned}
      [X_2] &= 0.50 - x \\
      [Y_2] &= 0.50 - 2x \\
      [XY_2] &= 2x 
      \end{aligned}
      \]

2. **Write the expression for the equilibrium constant \( K \):**
   \[
   K = \frac{[XY_2]^2}{[X_2][Y_2]^2}
   \]
   Plug in the equilibrium concentrations:
   \[
   3.9 \times 10
Transcribed Image Text:**Chemical Equilibrium: Calculating Equilibrium Concentrations** **Consider the general reaction below:** \( \mathbf{X_2(g) + 2Y_2(g) \rightleftharpoons 2XY_2(g)} \) **Given:** - Equilibrium Constant, \( K = 3.9 \times 10^{-8} \) at \( 298 \, \text{K} \) **Initial Conditions:** - 0.50 M \( \mathbf{X_2} \) and 0.50 M \( \mathbf{Y_2} \) were added to a sealed vessel. **Objective:** Calculate the equilibrium concentrations of the components. What is the equilibrium concentration of \( \mathbf{XY_2} \)? \[ [XY_2] = \boxed{?} \times 10^{\boxed{?}} \, \text{M} \] **Steps to Solve:** 1. **Set up the ICE Table** (Initial, Change, Equilibrium) to find the equilibrium concentrations: - **Initial Concentrations:** \[ \begin{aligned} [X_2] &= 0.50 \, \text{M} \\ [Y_2] &= 0.50 \, \text{M} \\ [XY_2] &= 0 \, \text{M} \end{aligned} \] - **Change in Concentrations:** \[ \begin{aligned} [X_2] &= -x \\ [Y_2] &= -2x \\ [XY_2] &= +2x \end{aligned} \] - **Equilibrium Concentrations:** \[ \begin{aligned} [X_2] &= 0.50 - x \\ [Y_2] &= 0.50 - 2x \\ [XY_2] &= 2x \end{aligned} \] 2. **Write the expression for the equilibrium constant \( K \):** \[ K = \frac{[XY_2]^2}{[X_2][Y_2]^2} \] Plug in the equilibrium concentrations: \[ 3.9 \times 10
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