$\overline{){\mathbf{K}}_{\mathbf{p}}\mathbf{}\mathbf{=}\frac{{\mathbf{\left[}\mathbf{NOCl}\mathbf{\right]}}^{\mathbf{2}}}{{\mathbf{\left[}\mathbf{NO}\mathbf{\right]}}^{\mathbf{2}}\mathbf{}\mathbf{\left[}{\mathbf{Cl}}_{\mathbf{2}}\mathbf{\right]}}}\phantom{\rule{0ex}{0ex}}\mathbf{0}\mathbf{.}\mathbf{27}\mathbf{}\mathbf{=}\mathbf{}\frac{{\mathbf{\left(}\mathbf{115}\mathbf{\right)}}^{\mathbf{2}}}{{\mathbf{(}\mathbf{x}\mathbf{-}\mathbf{115}\mathbf{)}}^{\mathbf{2}}\mathbf{(}\mathbf{x}\mathbf{-}\mathbf{57}\mathbf{.}\mathbf{5}\mathbf{)}}\phantom{\rule{0ex}{0ex}}\mathbf{0}\mathbf{.}\mathbf{27}{\mathbf{(}\mathbf{x}\mathbf{-}\mathbf{115}\mathbf{)}}^{\mathbf{2}}\mathbf{(}\mathbf{x}\mathbf{-}\mathbf{57}\mathbf{.}\mathbf{5}\mathbf{)}\mathbf{}\mathbf{=}\mathbf{}\mathbf{13225}\phantom{\rule{0ex}{0ex}}{\mathbf{(}\mathbf{x}\mathbf{-}\mathbf{115}\mathbf{)}}^{\mathbf{2}}\mathbf{(}\mathbf{x}\mathbf{-}\mathbf{57}\mathbf{.}\mathbf{5}\mathbf{)}\mathbf{}\mathbf{=}\mathbf{}\mathbf{48981}\mathbf{.}\mathbf{48}$

Nitric oxide reacts with chlorine gas according to the following reaction: 2NO(g) + Cl_{2}(g) ⇌ 2NOCl(g); K_{p} = 0.27 at 700 K

A reaction mixture initially contains equal partial pressures of NO and Cl_{2}. At equilibrium, the partial pressure of NOCl was measured to be 115 torr. What were the initial partial pressures of NO and Cl_{2}?

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