Determine the K, if the Kp = 2.89 for the reaction below at 327 °C. 2 NO2 (g) N₂O4 (g) Recall that K₁= K (RT)An

Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh with oxides as a catalyst. For the reaction: N2(g) + 3H2(g) 2NH3(g) equilibrium constants (K values) as a function of temperature are: 300 Celsius, 4.34 x 10^-3  500 Celsius, 1.45 x 10^-5 600 Celsius, 2.25 x 10^-6 Is the reaction exothermic or endothermic? How did you determine this? How do I show that it is exothermic?

The equilibrium constant for the following reaction is 260 at -1 °C. 2 NO(g) + Br₂(g) 2 NOBr(g) K 260 at -1 °C - Calculate the equilibrium constant for the following reactions at -1 °C. (a) 2 NOBr(g) (b) NOBr(g) ? 2 NO(g) + Br₂(g) NO(g) + 1/2 Br₂(g) K = K =

At a particular temperature, K = 3.68 for the reaction SO2(g) + NO2(g) = SO3(g) + NO(g) Calculate the concentrations of all four gases at equilibrium when 0.574 mol of each gas is mixed in a 1.000-L flask. (In other words, the concentration of each gas is 0.574 M.) HOW DO WE GET THERE? We will define the change in the concentrations to reach equilibrium in terms of x. Let x equal the number of moles per liter of SO, and NO, consumed to reach equilibrium. SO2(g) + NO2(g) = SO3(g) + NO(g) Initial: 0.574 0.574 0.574 0.574 Change: -X +x +x -x Equilibrium: 0.574-x 0.574-x 0.574+x 0.574+x Therefore, [SO,]]NO] [SO,]]NO,] (0.574+æ)(0.574+æ) (0.574 – x)(0.574 – x) K = 3.68 = What is the value of x? X =

25.00 g of solid ammonium hydrogen sulfide is introduced into a 750.-mL flask at 25°C, the flask is sealed, and the system is allowed to reach equilibrium.  What is the partial pressure of ammonia in this flask if Kp = 0.108 at 25°C for NH4HS(s) (equilibrium sign) NH3(g) + H2S (g)?

Given the reaction shown below with a Kp= 142 occurring at 941 K: Fe3O4(s) + 4H2(g) to 3Fe(s) + 4H2O(g)  calculate Kc for the reaction