Consider the following generic reaction: 2A2B(g) ⇌ 2A2(g) + B2(g) Some molecules of A2B are placed in a 1.0- L container. As time passes, several snapshots of the reaction mixture are taken as illustrated below.
Which illustration is the first to represent an equilibrium mixture? Explain. How many molecules of A2B were initially placed in the container? The Equilibrium Constant.
Answer to relevant QuestionsThere is only one value of the equilibrium constant for a particular system at a particular temperature, but there are an infinite number of equilibrium positions. Explain. At a particular temperature, a 3.0- L flask contains 2.4 moles of Cl2, 1.0 mole of NOCl, and 4.5 × 10-3 mole of NO. Calculate K at this temperature for the following reaction. 2NOCl(g) ⇌ 2NO(g) + Cl2(g) The reaction 2NO(g) + Br2(g) ⇌ 2NOBr(g) as Kp = 109 at 25oC. If the equilibrium partial pressure of Br2 is 0.0159 atm and the equilibrium partial pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at ...The equilibrium constant is 0.0900 at 25oC for the reaction H2O(g) + Cl2O(g) ⇌ 2HOCl(g) For which of the following sets of conditions is the system at equilibrium? For those which are not at equilibrium, in which direction ...At a particular temperature, K = 2.0 × 10-6 for the reaction 2CO2(g) ⇌ 2CO(g) + O2(g) If 2.0 moles of CO2 is initially placed into a 5.0-L vessel, calculate the equilibrium concentrations of all species.
Post your question