3. The equilibrium constant for the reaction N2(g) + O2(g) = 2 NO(g) is 3.4x10-21. What...
At 4124 oC the equilibrium constant for the reaction: 2 NO(g) N2(g) + O2(g) is KP = 7.16. If the initial pressure of NO is 0.00663 atm, what are the equilibrium partial pressures of NO, N2, and O2? p(NO) = . p(N2) = . p(O2) = .
) Consider the following reaction a 25 oC: N2(g) + 2 O2(g) D N2O4(g) An equilibrium mixture contains O2(g) and N2O4(g) at partial pressures of 2.5 atm and 4.5 atm, respectively. Determine the equilibrium partial pressure of N2 in the mixture.
At 7075 °C the equilibrium constant for the reaction: 2 NO(g) N2(g) + 02(9) is Kp 0.983. If the initial pressure of NO is 0.00863 atm, what are the equilibrium partial pressures of NO, N2, and O2? P(NO) P(N2) p(02)
1. (14 pts) Consider the following unbalanced gas-phase exothermic reaction, N2 + O2 = NO2 This is a reaction involved in the production of smog. The heat of formation of NO2 from the elements is A He = 33.18 kJ/mol. This is an endothermic process. The 4, Gof NO2 is 51.31 kJ/mol. a) Balance the reaction. b) Calculate the equilibrium constant at room temperature (300 K). c) If we assume that in our atmosphere the partial pressure of oxygen is...
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?
14.49. If the equilibrium constant K, for the reaction N2(g) + O2(g) – 2 NO(g) is 1.5 X 10%, in which direction will the reaction proceed if the partial pressures of the three gases are all 1.00 X 10-3 atm?
Consider the following reaction. N2(g) + O2(g) 2 NO(g) If the equilibrium partial pressures of N2, O2, and NO are 0.15 atm, 0.33 atm, and 0.050 atm, respectively, at 2200°C, what is KP?
For the reaction 2 A(g) + 3 B(g) <-->2 C(g) + 2 D(g), the equilibrium constant at 298 K is 1.605×10-11. If the initial partial pressures of A, and B are 0.564 bar, and 0.728 bar, respectively, determine the partial pressure of D (in bar) once equilibrium has been reached at 298 K.
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...