A mixture of 1.00 Atm of NO, 0.50 Atm of H2, and 1.00 Atm of N2 was allowed to reach equilibrium according to the reaction given below (initially there was no H2O). At equilibrium, the partial pressure of NO was found to be 0.62 Atm. Determine the value of the equilibrium constant, Kp, for the reaction: 2NO(g) + 2H2(g) ⇄ N2(g) + 2H2O(g

Consider the equilibrium below.CH₄ (g) + H₂O (g) ⇄ CO (g) + 3 H₂ (g)At a certain temperature, a container is fill with CH₄ and H₂O gases until the pressures of CH₄ = 8.000 atm and the pressure of H₂O = 10.000 atm. When equilibrium is reached, the total pressure in the container is 21.466 atm. Calculate the value of the equilibrium constant Kp at this temperature.Very large or very small numbers should be entered in scientific notation using the 'E' format, just like your calculator. A number such as 2.34×10-7 should be entered as 2.34E-7Kp=

At 2000 K the partial pressures of an equilibrium mixture of H2S, H2, and S are O.0252,0.0331, and 0.0352 atm, respectively. Calculate the value of the equilibrium constant Kp at 2000 K. H,S (g) - H, (g) +S(g)

4. At 100.°C, Kp = 60.6 for the reaction: 2 NOBr (g) → 2 NO (g) + Br₂ (g). In an experiment, 0.10 atm of each component is placed in a sealed container. Is the mixture at equilibrium? If not, in which direction will the reaction proceed? Show your work to justify your answer.