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The partial pressures at equilibrium are: = 0.001714 atm P Pso₂ Po₂ = 0.001717 atm Pso₂ = 0.0166 atm Calculate Kp for the reaction. See Periodic Table See Hint

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Calculate the equilibrium constant for the reaction ammonia combining with oxygenforms nitrogen dioxide and water all the reactants and products are in gaseous state at425oC. If the initial number of moles in a 2.00L container for ammonia, oxygen , nitrogendioxide and water are 8mol, 12mol, 2 mol and 3mol respectively. The equilibriumconcentration of water vapour is 3.00mol/L

physical chem

Give detailed  solution..show work..don't give Handwritten answer..don't use Ai for answering this

Give detailed Solution..show work..don't give Handwritten answer..don't use Ai for answering this

Please don't provide handwritten solution .....

For the equilibrium reaction.   2IBr (g) I2 (g) + Br2 (g) Kc=.0085.  If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components.   Consider the decomposition reaction at 555 K   4POCl3 (g)    P4  (g) + 2O2  (g) + 6Cl2  (g)   If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm.  Find Kp and Kc.