12. In the following reaction ( mathrm{COCl}_{2}(mathrm{~g}) leftrightarrow mathrm{CO}(mathrm{g})+mathrm{Cl}_{2}(mathrm{~g}) ) with ( mathrm{Kp}=6.7 imes 10^{-9} ) at ( 100 .{ }^{circ} mathrm{C} ), if a reaction vessel is initially filled with only ( mathrm{COCl}_{2}(mathrm{~g}) ) at ( 2.3 mathrm{~atm} ) and ( 100 .{ }^{circ} mathrm{C} ), what will be the equilibrium partial pressures of all three gases?
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Step 1: Write the balanced chemical equation for the reaction: COCl2 ⇌ CO + Cl2 Show more…
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In the following reaction COCl2<>CO+Cl with Kp = 6.7 x 10-9 at 100.°c, if a reaction vessel is initially filled with only COCl2 at 2.3 atm and 100°c, what will be the equilibrium partial pressure of all three gases
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The equilibrium constant for the reaction COCl2(g) ⇌ CO(g) + Cl2(g) is Kp = 2.2 × 10−10 at 100°C. If the initial concentration of COCl2 is 3.05 × 10−3 M, what is the partial pressure of each gas at equilibrium at 100°C?
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