A mixture of 0.430 M H₂O, 0.398 M C₁₂O, and 0.732 M HCIO are enclosed in a vessel at 25 °C. H₂O(g) +Cl₂O(g)=2 HOCI(g) Ke=0.0900 at 25°C Calculate the equilibrium concentrations of each gas at 25 °C. [H₂O]= [C₁₂0]= [HOCI]= M M M

A mixture containing 5.6 Atm of N2O and 2.8 Atm of O2 was prepared and after the equilibrium                         2 N2O(g) + 3 O2(g)  ⇆  4 NO2(g) was established the O2 partial pressure was found to be 0.31 Atm. What is the equilibrium constant Kp?

Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react according to the following reaction. PCI3(g)+ Cl2(g) = PCl5(g) The equilibrium constant for the reaction is Kc, = 37.5 at 145 °C. If 0.222 mol of phosphorus trichloride is added to 0.750 mol of chlorine in a 1.69 - L reaction vessel and allowed to react at this temperature, what is the equilibrium concentration (in mol/L) of phosphorus pentachloride? Report your answer to THREE significant figures.

A mixture of 0.592 M H₂O, 0.480 M Cl₂O, and 0.747 M HClO are enclosed in a vessel at 25 °C. H₂O(g) + Cl₂O(g) = 2 HOCI(g) Kc = 0.0900 at 25°C Calculate the equilibrium concentrations of each gas at 25 °C. [H₂O]= [C1₂O]= [HOCI]= M M M

Cyclohexane, C6H12, a hydrocarbon, can isomerize or change into methylcyclopentane, a compound of the same formula (C5 H9 CH3) but with a different molecular structure. Cyclohexane Methylcyclopentane The equilibrium constant has been estimated to be 0.12 at 25 °C. If you had originally placed 0.053 mol of cyclohexane in a 2.8 L flask, what would be the concentrations of cyclohexane and methylcyclopentane when equilibrium is established? [cyclohexane] = M [methylcyclopentane] = M

Phosphorous pentachloride decomposes at 600. °C according to the following equation. PCI, = PCl (g) + Cl,(g) After the system comes to equilibrium the partial pressures of both Cl and PCl; are found to be 3.14 atm, and the partial pressure of PCI5 was 0.858 atm. Calculate K (not Kp) for this reaction at 600 °C.

At a particular temperature the equilibrium constant K = 2.50 for the following reaction in the gas phase: SO2(g) + NO2(g) = SO3(g) + NO(g). Calculate the equilibrium pressure of SO3(g) in the reaction if the initial pressures of SO2(g) and NO2(g) were both 1.00 bar. and no products had been formed. O 0.20 bar 0.39 bar 1.39 bar 0.61 bar 1.61 bar

Hand written solutions are strictly prohibited.

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Consider the following reaction: (NH,),CO; (g) → 2 NH3 (g) + CO, (g) + H,O (1) If a reaction mixture is set up with 0.41 atm of (NH,),CO3, 3.2 atm of NH3, and 2.3 atm of CO2, what will be the equilibrium concentration of all gases present? K, = 1.8 x 10°[