We are being asked to calculate the equilibrium concentration of X_{2} for the given equilibrium reaction:

** H _{2}(g) + X_{2}(g) ⇌ 2 HX(g) K_{c} = 24.4 at 300 K. **

**When dealing with equilibrium and K _{c}:**

• **K _{c} **→ equilibrium units are in molarity

•

$\overline{){{\mathbf{K}}}_{{\mathbf{c}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

▪ **only aqueous and gaseous species** are included in the equilibrium expression

▪ the **coefficient** of each compound in the reaction equation will be the **exponent **of the concentrations in the equilibrium expression

**Given: **

**Initial Concentrations:**

initial H_{2} = 0.150 M

initial X_{2} = 0.200 M

initial HX = 0.600 M

**Let’s calculate the Reaction Quotient (Q) using the given initial concentration to determine which direction the equilibrium will proceed:**

$\overline{){\mathbf{Q}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

For the reaction system H_{2}(g) + X_{2}(g) ⇌ 2 HX(g)

K_{c} = 24.4 at 300 K. If the reaction is set up with the following initial concentrations, what will the equilibrium concentration of X_{2} be?

initial H_{2} = 0.150 M initial X_{2} = 0.200 M initial HX = 0.600 M

A. 0.0365 M

B. 0.114 M

C. 0.164 M

D. 0.0730 M

E. 0.500 M

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