# Problem: At a particular temperature, Kp = 0.25 for the reaction N2O4(g) ⇌ 2NO2(g)b. A flask containing only NO2 at an initial pressure of 9.0 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases.

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###### FREE Expert Solution

N2O4(g) ⇌ 2NO2(g)              Kp = 0.25

Step 1: Construct an ICE chart for the equilibrium reaction. Step 2: Calculate the change (x) in the reaction using the equilibrium constant.

N2O4(g) ⇌ 2NO2(g)              Kp = 0.25

$\overline{){\mathbf{K}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}\phantom{\rule{0ex}{0ex}}\mathbf{K}\mathbf{=}\frac{{\mathbf{\left[}{\mathbf{NO}}_{\mathbf{2}}\mathbf{\right]}}^{\mathbf{2}}}{\mathbf{\left[}{\mathbf{N}}_{\mathbf{2}}{\mathbf{O}}_{\mathbf{4}}\mathbf{\right]}}\phantom{\rule{0ex}{0ex}}\mathbf{0}\mathbf{.}\mathbf{25}\mathbf{=}\frac{{\mathbf{\left(}\mathbf{9}\mathbf{.}\mathbf{0}\mathbf{-}\mathbf{2}\mathbf{x}\mathbf{\right)}}^{\mathbf{2}}}{\mathbf{x}}\phantom{\rule{0ex}{0ex}}\mathbf{0}\mathbf{.}\mathbf{25}\mathbf{x}\mathbf{=}\mathbf{81}\mathbf{-}\mathbf{36}\mathbf{x}\mathbf{+}\mathbf{4}{\mathbf{x}}^{\mathbf{2}}\phantom{\rule{0ex}{0ex}}\overline{)\mathbf{0}\mathbf{=}\mathbf{4}{\mathbf{x}}^{\mathbf{2}}\mathbf{-}\mathbf{36}\mathbf{.}\mathbf{25}\mathbf{x}\mathbf{+}\mathbf{81}}$

Now, we will use the quadratic formula to solve for x. The quadratic formula is: ###### Problem Details

At a particular temperature, Kp = 0.25 for the reaction

N2O4(g) ⇌ 2NO2(g)

b. A flask containing only NO2 at an initial pressure of 9.0 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases.