We are being asked to calculate the equilibrium constant, K_{p} for the given equilibrium reaction:

**X _{2}(g) ⇌ 2X(g)**

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

•**K _{p}**→ equilibrium units are in terms of pressure

•

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

▪ **only 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:**

**P _{X}_{2}** = 1.75 atm

**In order to calculate the equilibrium concentrations of species, we need to use an ****ICE Chart. **

**Given values at equilibrium:**

P_{total} = 2.75 atm

**Calculate ****x:**

${\mathit{P}}_{\mathbf{t}\mathbf{o}\mathbf{t}\mathbf{a}\mathbf{l}\mathbf{}}\mathbf{=}\mathbf{}{\mathit{P}}_{{\mathbf{X}}_{\mathbf{2}}}\mathbf{}\mathbf{+}{\mathit{P}}_{\mathbf{X}}\phantom{\rule{0ex}{0ex}}\mathbf{2}\mathbf{.}\mathbf{75}\mathbf{=}\mathbf{}\mathbf{1}\mathbf{.}\mathbf{75}\mathbf{-}\mathit{x}\mathbf{}\mathbf{+}\mathbf{2}\mathbf{x}\phantom{\rule{0ex}{0ex}}\mathbf{2}\mathbf{.}\mathbf{75}\mathbf{=}\mathbf{}\mathbf{1}\mathbf{.}\mathbf{75}\mathbf{}\mathbf{+}\mathbf{}\mathbf{x}\phantom{\rule{0ex}{0ex}}\mathbf{}\mathbf{x}\mathbf{}\mathbf{=}\mathbf{}\mathbf{2}\mathbf{.}\mathbf{75}\mathbf{}\mathbf{-}\mathbf{}\mathbf{1}\mathbf{.}\mathbf{75}$

**x = 1.00 atm**

**We can now ****calculate the equilibrium constant, K _{p}:**

** ****X _{2}(g) ⇌ 2X(g)**

The reaction X_{2}(g) ⇌ 2X(g) occurs in a closed reaction vessel at constant volume and temperature. Initially, the vessel contains only X_{2} at a pressure of 1.75 atm. After the reaction reaches equilibrium, the total pressure is 2.75 atm.

What is the value of the equilibrium constant, K_{p}, for the reaction?

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