The equilibrium constant, Ke, for the reaction N2O4 (g) 2NO2(g) is 4.8 x 10-3 If the equilibrium mixture contains [NO₂] = 0.055 M, what is the molar concentration of N₂O4 Express the concentration to two significant figures and include the appropriate units. O ? B μA [N₂04] = Value Units

O KINETICS AND EQUILIBRIUM Try again. 2/5 Calculating equilibrium composition from an equilibrium constant Try Again Suppose a 500. mL flask is filled with 1.5 mol of O, and 0.60 mol of NO. The following reaction becomes possible: N,(g) +0,(2) – 2No(2) The equilibrium constant K for this reaction is 5.01 at the temperature of the flask. Calculate the equilibrium molarity of O,. Round your answer to two decimal places. 3.36 M II

Mass, Volume and Keq An equilibrium mixture, at 712°C in a 1972-mL container, involving the chemical system N2(g) + 3H2(g) — 2NH3(g) is found to contain 1.26 g of №₂, 0.227 g of H₂, and 9.76×10-³ g of NH3. Calculate the equilibrium constant (Keq expressed in terms of the molar concentrations) at the given temperature. (No units required.) 0.0148

2NO(g) + 2H₂(g) = N₂(g) + 2H₂O(g) The system initially contained 0.2500 M NO, 0.1300 M H2, and 0.2500 M H₂O. At equilibrium, the concentration of NO is 0.1296 M. What is the equilibrium concentration of H₂? [H₂] = [?] x 10¹ M K= [N₂] [H₂O]2 [NO]2[H₂]2 Coefficient (green) Exponent (yellow) Enter