Question 10 5 pts The value of the equilibrium constant for the reaction, N2(e)+0,6)=2NO(g), is 4.1...
Question 8 5 pts Calculate the pressures of all species at equilibrium in a mixture of NOCI, NO, and Cl2 produced when a sample of NOCI with an initial pressure of 0.500 atm comes to equilibrium according to this reaction: 2NOCI() 2NOE) + Cl2(g) Kp- 4.0 x 10 You may use the Module 3 File Upload to show your work or type as much as you can here. If you use the Module 3 File Upload, be sure to upload...
D Question 9 5 pts The equilibrium constant for the decomposition of PCIsle) into PC13(g) and Ca(e) is 0.0211. What is the equilibrium concentration of PC, if the initial concentration of PCIs was 4.32 M? Record to the thousandth's place. You may use the Module 3 File Upload to show your work for partial credit. If you use the Module 3 File Upload, be sure to upload your file within 15 minutes of completing your quiz.
The following reaction establishes equilibrium at 2000K: N2(g) + O2(g) 2NO(g) where Keq - 4.1 x 10-4 If the reaction began with 0.150 M of N2 and 0.150 M of O2, the equilibrium concentration of NO would be Note: If there is no exponent then you must enter a O for answer 2.
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?
5. The equilibrium constants for the following reactions are known 2NO(g) N(g)+ O(g) Ki-2.4x 100 2NO(g)+ O:(g) in 2NO:(g) K2=2.4 102 a) Sum these reactions to obtain the reaction. (10p) N2(g)+20(g) 2NO (g) b) Use the equilibrium constants of the first two reactions to determine the equilibrium. constant for the last reaction. (10p) oitei mundil Some Formulas K,-Peosbesto P(reactants) K= [products [reactants Rate = k[A]"[B]T R 0.08206 L atm/K mol R-8.314 J/mol K CHEM-1043-PO02
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?
The equilibrium constant, Kp, for the following reaction is 0.160 at 298K. 2NOBr(g) 2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 19.9 L container at 298K contains NOBr at a pressure of 0.297 atm and NO at a pressure of 0.251 atm, the equilibrium partial pressure of Br2 is ? atm.
At a certain temperature, the equilibrium constant K for the following reaction is 0.0018: N2(8) + O2(8) 2NO(g) Use this information to complete the following table. Suppose a 27. L reaction vessel is filled with 1.0 mol of N2 and 1.0 mol of O2. What can you say about the composition of the mixture in the vessel at equilibrium? There will be very little N2 and O2. There will be very little NO. Neither of the above is true. What...
The equilibrium constant, Kc, for the following reaction is 6.50×10-3 at 298K. 2NOBr(g) 2NO(g) + Br2(g) If an equilibrium mixture of the three gases in a 11.1 L container at 298K contains 0.376 mol of NOBr(g) and 0.396 mol of NO, the equilibrium concentration of Br2