Consider the reaction
N2(g)+O2(g)↽−−⇀2NO(g)N2(g)+O2(g)↽−−⇀2NO(g)
that has an equilibrium constant, ?cKc, fof 4.10×10−44.10×10−4 at 17001700 °C. What percentage of O2O2 will react to form NO if 0.4850.485 mol N2N2and 0.4850.485 mol O2O2 are added to a 0.6870.687 L container and allowed to come to equilbrium at 17001700 °C?
Consider the reaction N2(g)+O2(g)↽−−⇀2NO(g)N2(g)+O2(g)↽−−⇀2NO(g) that has an equilibrium constant, ?cKc, fof 4.10×10−44.10×10−4 at 17001700 °C. What...
Even at high temperatures, the formation of NO is not favored: (Kc = 4.10 ×10−4 at 2000°C) N2(g) + O2(g) ⇌ 2 NO(g) What is [NO] when a mixture of 0.20 mol of N2(g) and 0.17 mol of O2(g) reach equilibrium in a 1.0−L container at 2,000°C?
Consider the reaction N2(g) + O2(g) ⇌ 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.26, 0.36, and 0.030 atm, respectively, at 2200°C, what is KP?
Consider the reaction N2(g) + O2(g) ⇌ 2NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.20, 0.35, and 0.030 atm, respectively, at 2200° C, what is KP?
For the reaction N2(g) + O2(g) 2NO(g), Kc = 4.0 at a particular temperature. In a 1.0-L container, 1.0 mol of N2 and O2 are mixed. Determine the concentration of NO once equilibrium is reached at the given temperature. =________ Please explain so I understand
The equilibrium constant for the reaction N2(g) +O2(g) =2 NO (g) is 1.69 x 10-3 at 2300 K. A mixture consisting of 5 g of nitrogen and 2 g of oxygen in a container of volume 1 dm3 is heated to 2300 K and allowed to come to equilibrium. Calculate the mole fraction of NO at equilibrium (Note: this is a process that happens all the time when running an engine that heats air. NO is always produced when heating...
The equilibrium constant KcKc for the reaction 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) is 6.9×1056.9×105 at 500 KK. A 5.0 LL reaction vessel at 500 KK was filled with 0.052 molmol of NONO, 1.1 molmol of O2O2, and 0.90 molmol of NO2NO2. Part A What is the value of QcQc? Express your answer to two significant figures.
Identify the proper form of the equilibrium-constant expression for the equation N2(g)+O2(g)⇌2NO(g)
Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature K 400 1.9x10^7 425 2.5x10^6 465 1.6x10^5 515 8.8x10^3 600 2.0x10^2 Use the data to find ΔrS∘ΔrS∘ for the reaction. (answer in J K-1 mol-1) The answer is NOT 158
4. For the reaction Nzco) + O2(0)+-> 2NO(9), K = 0.0017 at 2300 K. 0.15 mol of Na and 0.25 mol of O2 are placed in a 10.0 L flask and allowed to react and reach equilibrium at 2300 K. Find the concentrations of N2, Oz, and NO at equilibrium.
Part ADetermine the value of the equilibrium constant, Kgoal, for the reactionN2(g)+H2O(g)→NO(g)+12N2H4(g), Kgoal=?by making use of the following information:1. N2(g)+O2(g)→2NO(g), K1 =4.10