3. A flask initially containing 0.815 atm of NOBr decomposed to give an equilibrium mixture for...
Consider the reaction: 2 NO(g) + Br2(g) ↔ 2 NOBr(g) Kp = 28.4 atm-1 at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 173 Torr and that of Br2 is 142 Torr. What is the partial pressure (in Torr) of NOBr in this mixture? PNOBr = ___ Torr
Consider the equilibrium 4. N2(g) 02(g) Br2(g) 2NOBr (g) Calculate the equilibrium constant Kp for this reaction, give the following information (298.15 K) NO (g) +1/2Br2(g) NOBr(g) Ke 4.5 2 NO (g)N2(g) 02(g) Ke 3.0 x 102 5. For the BrCl decomposition reaction 2BrCl(g) Br2(g Cl2(g) Initially, the vessel is charged at 500 K with BrCl at a partial pressure of 0.500 atm. At equilibrium, the partial pressure of BrC is 0.040 atm. Calculate Kp value at 500K Consider the...
• Calculate the equilibrium concentration of all the species in a flask initially containing only 3.00 atm of NO2. 2NO2 (g) ⇌ N2O4 (g) Kp = 9.3 x 10-7
At a particular temperature, Kp-0.39 for the reaction below. N204(g) 2 NO2(g) (a) A flask containing only N204 at an initial pressure of 4.8 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. N2O4 NO2 atm (b) A flask containing only NO2 at an initial pressure of 9.6 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. No2 (e) From your answers to parts (e) and (b), does it matter...
Consider the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K. In a reaction mixture at equilibrium, the partial pressure of NO is 108 torr and that of Br2 is 158 torr . What is the partial pressure of NOBr in this mixture?
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.
Consider the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 130 torr and that of Br2 is 146 torr What is the partial pressure of NOBr in this mixture? Express your answer using three significant figures.
Consider the reaction: 2NO(g)+Br2(g)⇌2NOBr(g) Kp=28.4 at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 101 torr and that of Br2 is 150 torr . What is the partial pressure of NOBr in this mixture? Express your answer using three significant figures.
10. Using the equation shown below, calculate the equilibrium concentration of each species in a mixture containing 0.0500 M PCls and 5,00 M PCI K for this reaction is 3.33 x 10' at 487 °C. PCs () PC:(8) + Cl() Suvishortliwabidi a llo 11. At equilibrium, the partial pressures of NO2, NO, and O, were found to be 0.200 atm, 0.00026 atm, and 0.600 atm, respectively, in a 1-liter flask. 2NO, (g) 2NO(g) + O2(g) s obomb (a) Write the...
Consider the following reaction: 2NO(g)+Br2(g)⇌2NOBr(g) ,Kp=28.4, at 298 K In a reaction mixture at equilibrium, the partial pressure of NO is 102 torr and that of Br2 is 134 torr . Part A What is the partial pressure of NOBr in this mixture? Express your answer in torrs to three significant figures.